we cannot find the value of ΔS (kJ/mol) which determines change in entropy in standard state. for the reaction as we need to have the ΔH to find ΔS.
To calculate ΔS from the equation of the line y = -152.343x + 376.490, we need to know the value of ΔH for the reaction. Without this information, we cannot calculate ΔS. The equation of the line y = -152.343x + 376.490 represents the variation of ΔG with temperature. ΔG represents change in free energy . The slope of the line is -152.343 kJ/mol K, which is equal to -ΔG/T. The y-intercept of the line is 376.490 kJ/mol, which is equal to ΔG at T = 0.So, the plot of ΔG (kJ/mol) vs. T (K) gives us the information about ΔG and its variation with temperature. But we need to know ΔH to find ΔS.
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what is the solubility of KCI?
Answer:
Potassium chloride.
A[?] is a heterogeneous mixture which settles on standing and its components can be separated by filtration. colloid suspension
I think it should be suspension.
How is the rate of a reflection affected when the temperature increases
The rate of a reflection decreases when the temperature increases
This goes to say that the rate of reflection will go down more whenever there is an increase in temperature
What is reflection?Reflection can simply be defined as the the throwing back by a body of light without absorbing it.
reflection of
In conclusion, the rate of a reflection decreases when the temperature increases
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A mixture contains NaHCO3
together with unreactive components. A 1.68 g sample of the mixture reacts with HA
to produce 0.561 g of CO2
.
The molar mass of NaHCO3
is 84.01 g/mol
and the molar mass of CO2
is 44.01 g/mol.
What is the percent by mass of NaHCO3
in the original mixture?
Answer: 63.75 %
Explanation:
The balanced chemical equation for this reaction is:
NaHCO3 + HA = NaA + H2O + CO2
According to the chemical equation, one mole of NaHCO3 will react with one mole of HA to form one mole of NaA, H2O and CO2. All the components are in same mole ratio of 1:1:1:1
So,
Moles of CO2 = weight/molar mass = 0.561/44 = 0.01275 moles
Moles of CO2 will be equal to moles of NaHCO3 = 0.01275 moles
Moles = weight/mass
Weight = moles × mass
So the weight of NaHCO3 = 0.01275 × 84.01 = 1.071 g
The percentage mass of NaHCO3 in the original mixture =(1.071/1.68)× 100% = 63.75 %
Therefore, the percent by mass of NaHCO3 in the original mixture was 63.75 %
Calculate the freezing point of a solution that contains 8.0 g of sucrose (C12H22O11) in 100 g of H2O. Kf for H2O = 1.86C/m
Group of answer choices
A. 0.44 degrees Celsius
B. 0.044 degrees Celsius
C. 0.39 degress Celsius
D. 0.22 degress Celsius
The freezing point of the sucrose solution is -0.435°C.
What is the freezing point of the solution?The freezing point of the solution is determined from the freezing point depression formula below:
ΔT = mKf(H₂O)Kf(H₂O) = 1.86 Cm
m is molality of solution = moles of solute/mass of solvent
moles of sucrose = 8.0/342.3 = 0.0233 moles
m = 0.0233/0.1 = 0.233 molal
ΔT = 0.233 m * 1.86°C/m.
ΔT = 0.435 °C.
Freezing point of sucrose solution = 0°C - 0.435°C
Freezing point of sucrose solution = -0.435°C.
In conclusion, the freezing point of sucrose solution is determined from the freezing point depression.
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How many atoms are in 1.50 g of Al?
(A) 0.0556
(B) 18.0
(C) 3.35 x 10^22
(D) 2.44 x 10^25
What is the theoretical yield of bromobenzene in this reaction when 24.8 g of benzene reacts with 52.3 g of bromine?
Answer:
49.8 g C₆H₅Br
Explanation:
The theoretical yield is the maximum calculated amount of product that can be made from a reaction. To find the theoretical yield, you need to (1) determine the chemical reaction which is taking place, then (2) calculate the molar masses of the relevant reactants and product, then (3) convert grams of each reactant to grams of bromobenzene (using molar masses and mole-to-mole ratio from reaction coefficients), and then (4) determine the limiting reagent and the theoretical yield.
(Step 1)
Bromine = Br₂
Benzene = C₆H₆
Bromobenzene = C₆H₅Br
The balanced equation:
Br₂ + 2 C₆H₆ ----> 2 C₆H₅Br + H₂
(Step 2)
Molar Mass (Br₂): 2(79.904 g/mol)
Molar Mass (Br₂): 159.808 g/mol
Molar Mass (C₆H₆): 6(12.011 g/mol) + 6(1.008 g/mol)
Molar Mass (C₆H₆): 78.114 g/mol
Molar Mass (C₆H₅Br): 6(12.011 g/mol) + 5(1.008 g/mol) + 79.904 g/mol
Molar Mass (C₆H₅Br): 157.01 g/mol
(Step 3)
52.3 g Br₂ 1 mole 2 moles C₆H₅Br 157.01 g
----------------- x ------------------ x ------------------------- x --------------- =
159.808 g 1 mole Br₂ 1 mole
= 103 g C₆H₅Br
24.8 g C₆H₆ 1 mole 2 moles C₆H₅Br 157.01 g
------------------- x --------------- x -------------------------- x --------------- =
78.114 g 2 moles C₆H₆ 1 mole
= 49.8 g C₆H₅Br
(Step 4)
Because C₆H₆ produces a smaller amount of product than Br₂, it must be the limiting reagent. This means that it will run out before all of the Br₂ is used up. Therefore, the actual theoretical yield of C₆H₅Br is 49.8 grams.
The molar heat of fusion of gold is 12.550 kJ mol–1. At its melting point, how much mass of melted gold must solidify to release 235.0 kJ of energy?
The mass of melted gold to release the energy would be 3, 688. 8 Kg
How to determine the massIt is important to note that the formula for energy is
Q = n × HF
Where
n = number of moles
HF = heat of fusion
Let's find number of moles
235.0 = n × 12.550
number of moles = [tex]\frac{235}{12. 550}[/tex] = 18. 725 moles
The molar mass of Gold is 197g/ mol
We have that;
Number of moles = mass/ molar mass
Mass = number of moles × molar mass
Substitute the values
Mass = 18. 725 × 197
Mass = 3, 688. 8 Kg
Thus, the mass of melted gold to release the energy would be 3, 688. 8 Kg
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How many moles of methane are produced when 85.1 moles of carbon dioxide gas react with excess hydrogen gas?
Taking into account the reaction stoichiometry, 340.0 moles of methane are produced when 85.1 moles of carbon dioxide gas react with excess hydrogen gas
Reaction stoichiometryIn first place, the balanced reaction is:
CO₂ + 4 H₄ → CH₄ + 2 H₂O
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
CO₂: 1 moleH₄: 4 moles CH₄: 1 moleH₂O: 2 molesMoles of CH₄ formedThe following rule of three can be applied: if by reaction stoichiometry 1 mole of CO₂ form 4 moles of CH₄, 85.1 moles of CO₂ form how many moles of CH₄?
[tex]moles of CH_{4} =\frac{85.1 moles of CO_{2}x4 moles of CH_{4} }{1 moles of CO_{2}}[/tex]
moles of CH₄= 340.4 moles
Then, 340.0 moles of methane are produced when 85.1 moles of carbon dioxide gas react with excess hydrogen gas
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Decide whether each pair of elements in the table below will form an ionic compound. If they will, write the empirical formula of the compound formed in the
space provided.
element #1 element #2
sulfur
magnesium
sulfur
cesium
cesium
fluorine
magnesium
strontium
Forms ionic
compound?
yes
yes
yes
O yes
no
no
no
no
empirical formula of
ionic compound
0
0
0
0
Do
5
Answer:
1.) Yes, Cs₂S
2.) Yes, MgF₂
3.) Yes, MgS
4.) No
Explanation:
Nonmetals are located on the right side of the periodic table in the p-block. It is safe to assume that all the other elements are metals.
Ionic bonds form between a metal and nonmetal. When determining the empirical formula, the cation (the element losing electrons) is written before the anion (the element gaining electrons). The charges can be balanced by modifying the quantity of element.
1.) Cs₂S
-----> Cesium = metal and Sulfur = nonmetal
-----> Cesium = Cs⁺
-----> Sulfur = S²⁻
2.) MgF₂
-----> Magnesium = metal and Fluorine = nonmetal
-----> Magnesium = Mg²⁺
-----> Fluorine = F⁻
3.) MgS
-----> Magnesium = metal and Sulfur = nonmetal
-----> Magnesium = Mg²⁺
-----> Sulfur = S²⁻
4.) Both cesium and strontium are metals
What volume would 20.0 moles of sulfur
dioxide occupy at 75.3 °C with a pressure of
3.50 atm? Answer is in L
Answer:
163 L
Explanation:
To find the volume, you need to use the Ideal Gas Law. The equation looks like this:
PV = nRT
In this equation,
-----> P = pressure (atm)
-----> V = volume (L)
-----> n = moles
-----> R = constant (0.0821 L*atm/mol*K)
-----> T = temperature (K)
Before you can plug the given values into the equation, you first need to convert Celsius to Kelvin.
P = 3.50 atm R = 0.0821 L*atm/mol*K
V = ? L T = 75.3 °C + 273.15 = 348.45 K
n = 20.0 moles
PV = nRT
(3.50 atm)V = (20.0 moles)(0.0821 L*atm/mol*K)(348.45 K)
(3.50 atm)V = 572.1549
V = 163 L
How many moles of chlorine gas at 120. °C
and 33.3 atm would occupy a vessel of 11.5
L?
Answer:
11.9 moles Cl₂
Explanation:
To find the number of moles, you need to use the Ideal Gas Law. The equation looks like this:
PV = nRT
In this equation,
-----> P = pressure (atm)
-----> V = volume (L)
-----> n = moles
-----> R = constant (0.0821 L*atm/mol*K)
-----> T = temperature (K)
Before you can plug the given values into the equation, you first need to convert Celsius to Kelvin.
P = 33.3 atm R = 0.0821 L*atm/mol*K
V = 11.5 L T = 120. °C + 273.15 = 393.15 K
n = ? moles
PV = nRT
(33.3 atm)(11.5 L) = n(0.0821 L*atm/mol*K)(393.15 K)
382.95 = n(0.0821 L*atm/mol*K)(393.15 K)
382.95 = (32.2776)n
11.9 = n
what are the factors affecting qualitative analysis in chemistry
Answer:
Techniques and Tests
Qualitative analysis typically measures changes in color, melting point, odor, reactivity, radioactivity, boiling point, bubble production, and precipitation.
How do you separate Sand Potassium Nitrate and Champhor
Analyze the following reaction and the given scenarios to discuss the relationship between volume and reaction rate. Determine which reaction will happen at a faster rate and explain why.
NH3(g) + 2O2(g) → HNO3(l) + H2O(l)
The first reaction is started in a gas chamber with a volume of 10 L. The second reaction is started in a gas chamber with a volume of 5 L.
The second reaction with the volume of 5L will occur faster as compared to the first reaction of volume 10L.
Volume is inversely proportional to the rate of reaction.
As volume increases rate of reaction decreases and as volume decreases rate of reaction increases.
Let's consider a reaction A → B.
r is rate of reaction and K is rate constant, A is the concentration of reaction.
r = k(A)
r is directly proportional to the A.
But the concentration of A is in Moles/liters (i.e. moles per unit volume)
r is inversely proportional to the volume of vessel or chamber.
Hence as volume increases rate of reaction decreases.
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If you react 9.10g of vinyl chloride with 7.80g of oxygen, what is the theoretical yield of carbon dioxide
The theoretical yield of the CO2 produced is 4.22 g.
What is the theoretical yield of carbon dioxide?The balanced reaction equation is;
2C2H3Cl + 5O2 ------>2CO2 + 2H2O + 2HCl
Number of moles of vinyl chloride = 9.10g /62 g/mol = 0.15 moles
Number of moles of oxygen = 7.80g/32 g/mol = 0.24 moles
Now;
2 moles of C2H3Cl reacts with 5 moles of oxygen
0.15 moles of C2H3Cl reacts with 0.15 moles * 5 moles / 2 moles
= 0.375 moles
Hence oxygen is the limiting reactant;
5 moles of oxygen produces 2 moles of CO2
0.24 moles of oxygen produces 0.24 moles * 2 moles /5 moles
= 0.096 moles
Mass of CO2 produced = 0.096 moles * 44 g/mol
= 4.22 g
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Identify the Brønsted–Lowry acid and the Brønsted–Lowry
base on the left side of each of the following equations, and
also identify the conjugate acid and conjugate base of each
on the right side:
HCOOH(aq) + PO43-(aq) gives HCOO-(aq) + HPO42-(aq)
The following applies to the above equation:
Brønsted–Lowry acid - HCOOHBrønsted–Lowry base - PO43-Conjugate acid - HPO42-Conjugate base - HCOO-What is Bronsted-Lowry acid and base?Brønsted-Lowry acid is the any chemical species that acts as a donor of protons while Brønsted-Lowry base is any chemical species that acts as a proton acceptor.
In the following equation: HCOOH(aq) + PO43-(aq) = HCOO-(aq) + HPO42-(aq)
HCOOH is the proton (H+) donor, hence, is the Brønsted-Lowry acidPO43- is the donor acceptor, hence, is the Brønsted-Lowry baseHCOO- is the conjugate base that forms from the acidHPO42- is the conjugate acid that forms from the baseLearn more about Brønsted-Lowry acid and base at: https://brainly.com/question/15885173
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Balance the following reactions
a) Ca (s) + H₂O (1)→ Ca(OH)2 (aq) + H₂ (g)
b) Al2O3 (s) + C(s) + Cl₂ (g) → AICI3 (s) + CO (g)
c) FeCl3 (aq) + H₂S (g) → Fe2S3 (s) + HCI (aq)
d) CaCO3 (s) + HCI (aq) → Ca Cl₂ (aq) + CO2 (g) + H₂O (1)
Answer:
a) Ca (s) + 2 H₂O (l) ---> Ca(OH)₂ (aq) + H₂ (g)
b) Al₂O₃ (s) + 3 C (s) + 3 Cl₂ (g) ---> 2 AICI₃ (s) + 3 CO (g)
c) 2 FeCl₃ (aq) + 3 H₂S (g) ---> Fe₂S₃ (s) + 6 HCI (aq)
d) CaCO₃ (s) + 2 HCI (aq) ---> CaCl₂ (aq) + CO₂ (g) + H₂O (l)
Explanation:
For an equation to be balanced, there must be an equal amount of each type of atom on both sides of the reaction. The reactants are on the left side and the products are on the right side.
a) ------------------------------------------------------------------------------------------------------
The unbalanced equation:
Ca (s) + H₂O (l) ---> Ca(OH)₂ (aq) + H₂ (g)
Reactants: 1 calcium, 2 hydrogen, 1 oxygen
Products: 1 calcium, 4 hydrogen, 2 oxygen
The balanced equation:
Ca (s) + 2 H₂O (l) ---> Ca(OH)₂ (aq) + H₂ (g)
Reactants: 1 calcium, 4 hydrogen, 2 oxygen
Products: 1 calcium, 4 hydrogen, 2 oxygen
b) ------------------------------------------------------------------------------------------------------
The unbalanced equation:
Al₂O₃ (s) + C (s) + Cl₂ (g) ---> AICI₃ (s) + CO (g)
Reactants: 2 aluminum, 3 oxygen, 1 carbon, 2 chlorine
Products: 1 aluminum, 1 oxygen, 1 carbon, 3 chlorine
The balanced equation:
Al₂O₃ (s) + 3 C (s) + 3 Cl₂ (g) ---> 2 AICI₃ (s) + 3 CO (g)
Reactants: 2 aluminum, 3 oxygen, 3 carbon, 6 chlorine
Products: 2 aluminum, 3 oxygen, 3 carbon, 6 chlorine
c) ------------------------------------------------------------------------------------------------------
The unbalanced equation:
FeCl₃ (aq) + H₂S (g) ---> Fe₂S₃ (s) + HCI (aq)
Reactants: 1 iron, 3 chlorine, 2 hydrogen, 1 sulfur
Products: 2 iron, 1 chlorine, 1 hydrogen, 3 sulfur
The balanced equation:
2 FeCl₃ (aq) + 3 H₂S (g) ---> Fe₂S₃ (s) + 6 HCI (aq)
Reactants: 2 iron, 6 chlorine, 6 hydrogen, 3 sulfur
Products: 2 iron, 6 chlorine, 6 chlorine, 3 sulfur
d) ------------------------------------------------------------------------------------------------------
The unbalanced equation:
CaCO₃ (s) + HCI (aq) ---> CaCl₂ (aq) + CO₂ (g) + H₂O (l)
Reactants: 1 calcium, 1 carbon, 3 oxygen, 1 hydrogen, 1 chlorine
Products: 1 calcium, 1 carbon, 3 oxygen, 2 hydrogen, 2 chlorine
The balanced equation:
CaCO₃ (s) + 2 HCI (aq) ---> CaCl₂ (aq) + CO₂ (g) + H₂O (l)
Reactants: 1 calcium, 1 carbon, 3 oxygen, 2 hydrogen, 2 chlorine
Products: 1 calcium, 1 carbon, 3 oxygen, 2 hydrogen, 2 chlorine
Modeling Periodic Trends 1:
Why are periodic trends useful?
What are some examples of periodic trends?
What is ionization energy?
What was the purpose of creating your three-dimensional model?
Answer these questions in the discussion and conclusion of your Lab Report:
How does your model represent ionization energy?
What happens to the ionization energy of elements as you move from left to right across a period? Explain the trend.
What happens to the ionization energy of elements as you move down a group? Explain the trend.
In reactions between metals and nonmetals, metals tend to form cations while nonmetals tend to form anions. How does your model show this trend?
The periodic trend is very useful because it helps is understand the properties and reactivities of elements in chemical reactions
Some examples of periodic trends are:
Melting and boiling pointIonization energyElectron affinityElectronegativityAtomic size/ radiusIonic size / radiusWhat is ionization energy?Ionization energy can simply be defined as that energy required to remove a valence electron from an atom of an element in a gaseous state to form a gaseous ions l
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Question 8
If I have an unknown quantity of gas at a pressure of 3.85 atm, a volume of 32.4 liters, and a temperature of
80.4°C, how many moles of gas do I have?
Answer:
4.30 moles
Explanation:
You need to use the Ideal Gas Law. The equation looks like this:
PV = nRT
In this equation,
-----> P = pressure (atm)
-----> V = volume (L)
-----> n = moles
-----> R = Ideal Gas Constant (0.08206 atm*L/mol*K)
-----> T = temperature (K)
Before you can plug the given values into the equation and simplify to find "n", you need to convert Celsius to Kelvin. The final answer should have 3 sig figs to match the sig figs of the given values.
P = 3.85 atm R = 0.08206 atm*L/mol*K
V = 32.4 L T = 80.4 °C + 273.15 = 353.55 K
n = ? moles
PV = nRT
(3.85 atm)(32.4 L) = n(0.08206 atm*L/mol*K)(353.55 K)
124.74 = n(29.012313)
4.30 = n
please help me with this question
1. The resulting concentration will be 0.00044 mol/L
2. The minimum mass of sodium sulfite to add will be 0.4032 grams.
Stoichiometric problems1. Using m1v1=m2v2
m1 = 0.01 mol/L, v1 = 20 mL, v2 = 450 mL
m2 = m1v1/v2 = 0.01 x 20/450 = 0.00044 mol/L
2. [tex]Na_2SO_3 + Ca(NO_3)_2 --- > 2NaNO_3 + CaSO_3[/tex]
Mole ratio of the reactants = 1:1
Mole of 80 mL, 0.0400 mol/L Ca(NO3)2 = 80/1000 x 0.0400 = 0.0032 mol
Equivalent mole of Na2SO3 = 0.0032 moles
Mass of 0.0032 moles Na2SO3 = 0.0032 x 126 = 0.4032 grams
Thus, the minimum mass of sodium sulfite to be added must be 0.4032 grams.
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Draw a levelled diagram of a Daniel cell and write the half cell equations.
The labelled diagram of Daniell cell is as shown below
The half-reactions of oxidation and reduction taking place on electrodes are shown:
Oxidation at anode: Zn(s)→Zn 2+(aq)+2e −
Reduction at cathode: Cu 2+ (aq)+2e − →Cu(s)
What is Daniell Cell?
A Daniell cell is the best model of a galvanic cell which converts chemical energy into electrical energy. The Daniell cell consists of two electrodes of different metals, Zn and Cu; each electrode is in communication with a solution of its own ion; Zinc sulphate and copper sulphate respectively.
What is the distinction between Daniel cell and voltaic cell?The key difference between Daniell cell and galvanic cell is that Daniell cell operates only copper and zinc as electrodes whereas a galvanic cell can have a mixture of metals as electrodes.
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A gaseous compound containing hydrogen and carbon is decomposed and found to contain 90.00% carbon and 10.00% hydrogen by mass. The mass of 371 mL of the gas, measured at 415 mm Hg and 41°C, is found to be 0.315 g. What is the molecular formula of the compound?
The molecular formula of the compound is C₃H₄.
What is the molecular formula of the compound?The molecular formula of the compound is determined from the molecular mass of the compound.
The molecular mass of the compound is derived using the general gas equation as follows:
P₁V₁/T₁ = P₂V₂/T₂
V₂ = P₁V₁T₂/P₂T₁
Volume at STP, V₂ = (415 * 371 * 298(760 * 314)
V₂ = 192.26 mL = 0.192 L
Molar mass of gas = 22.4/0.192 * 0.315 = 36.75 g
Molecular formula is then determined from the mole ratio of the elements;
Carbon = 0.9 * 36.75/12 = 3
Hydrogen = 0.1 * 40/1 = 4
Thus, the molecular formula of the compound is C₃H₄.
In conclusion, the molecular formula of the gas is derived from the molecular mass.
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In the following reaction, what element is losing mass?
Mg(s) + CuSO4(aq) -> MgSO4(aq) + Cu(s)
A. Mg
B. Cu
C.O
D. S
The element which is losing mass from the above reaction is Cu
Mg(s) + CuSO4(aq) -> MgSO4(aq) + Cu(s)
What is a compound?A compound simply refers to a chemical compound which contains two contains two or more elements which are chemically combined together.
So therefore, the element which is losing mass from the above reaction is Cu
Mg(s) + CuSO4(aq) -> MgSO4(aq) + Cu(s)
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Which is the number of moles of carbon dioxide produced from the complete combustion of 4.3 moles of ethanol?
The number of moles of carbon dioxide produced will be 8.6 moles.
Stoichiometri mole ratiosFirst, let's look at the balanced equation of the reaction. The complete combustion of ethanol gives carbon dioxide and water as follows:
[tex]C_2H_5OH + 3O_2 --- > 2CO_2 + 3H_2O[/tex]
We can see from the equation that the burning of 1 mole of ethanol produces 2 moles of carbon dioxide. In other words, the mole ratio is 1:2.
Thus, with 4.3 moles of ethanol, the amount, in moles, of carbon dioxide that will be produced will be:
4.3 x 2 = 8.6 moles
In other words, 8.6 moles of carbon dioxide will be produced from the complete combustion of 4.3 moles of ethanol.
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Select all the correct answers.
A worker is holding a filled gas cylinder still. Which two sentences are true about the energy of the filled gas cylinder?
A man in a blue dress holding a red color cylinder
It has no energy because it’s being held still.
It has gravitational potential energy because of its height.
Its atoms and molecules have thermal energy.
It has motion energy because it will fall if let go.
Its kinetic energy is being converted to potential energy.
Reset Next
The true statements are:
It has gravitational potential energy because of its height.Its atoms and molecules have thermal energy.What is energy?Energy is the ability to do work.
Energy can exist in many form, two of which are kinetic and potential energy.
The worker is holding a filled gas cylinder still gives the gas potential energy by lifting it above the ground.
The molecules of the gas also has kinetic energy by virtue of their constant random motion resulting in thermal energy.
In conclusion, the energy of the filled gas is both potential and kinetic.
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A 36.65g sample of solid is placed in a flask. Toluene in which the solid is insoluble ,is added to the flask so that the volume of solid and liquid together is 50.00mL.The solid and toluene together weigh 58.58 g .The density of toluene at temperature of the experiment is 0.864g/ml .what is the density of the solid?
The density of the solid is =0.3076g/ml
Calculation of the density of solidThe mass of solid in flask = 36.65g
The volume of both solid and Toluene = 50ml
The mass of both solid and Toluene = 58.58g
The density of toluene = 0.864g/ml
The density of the solid = X
Note: The density of the solid is calculated from the density of both the solid and toluene.
But the density of solid+ toluene;
=mass/volume
= 58.58g/50ml
= 1.1716g/ml
Therefore the density of solid alone = density of both solid +toluene - density of toluene.
= 1.1716g/ml - 0.864g/ml
= 0.3076g/ml
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How is the kinetic energy of the particles of a substance affected during a phase change?
O Kinetic energy increases during exothermic changes and decreases during endothermic changes.
O Kinetic energy decreases during exothermic changes and increases during endothermic changes.
O Kinetic energy does not change, but the potential energy does.
O Kinetic energy changes in the opposite way that the potential energy changes.
Answer:
O Kinetic energy does not change, but the potential energy does
Given the reaction below, if 0.003 g of carbon dioxide is used up, how many grams of oxygen will be produced? (show work)
6 CO2 + 6 H2O → C6H12O6 + 6 O2
State which substance is undergoing oxidation and which substance is undergoing reduction in the following reaction:
N2 (g) + 3 H2 (g) ---> 2 NH3 (g)
Answer:
H₂(g) = oxidized
N₂(g) = reduced
Explanation:
Oxidized substances lose electrons and increase in oxidation number. Reduced substances gain electrons and decrease in oxidation number.
Lone elements always have an oxidation number of 0. So, N₂(g) and H₂(g) have oxidation numbers of 0.
Within compounds, hydrogen generally always have an oxidation of +1. Therefore, the hydrogen in NH₃(g) has an oxidation number of +1. In order to make the overall compound neutral, the nitrogen in NH₃(g) must have an oxidation number of -3 (to balance the +3 from the 3 hydrogens).
Since H₂(s) is losing electrons (goes from 0 to +1), it is being oxidized. Since N₂(g) is gaining electrons (goes from 0 to -3), it is being reduced.