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CHEM 1023 WI01-04 General Chemistry 2 2025 Winter

CHEM 1023 WI01-04 General Chemistry 2 2025 Winter

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BONUS QUESTION:

What is the IUPAC systematic name of the following compound?

5,5-dimethyl-3-ethylheptane

5-ethyl-3,3-dimethylheptane

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3,3-methyl-5-ethylheptane

3,3-dimethyl-5-ethylheptane

3-ethyl-5,5-dimethylheptane

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For a given reaction, Δ_rH = -51.9 kJ mol^-1 and Δ_rS = -72.5 J K^-1 mol^-1.

Above or below what temperature will the reaction be spontaneous? Express the temperature in °C to three significant figures.

Which

of the following pairs shows the correct relative magnitude of standard molar entropy (S°)?

All systems are for the same amount of substance at 25°C.

H₂O(g) > H₂(g)

Which of the following statements is true?

The total energy of the universe increases for a spontaneous process.

A reaction with ΔG>0 is spontaneous in the reverse direction.

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If a reaction has an equilibrium constant, K = 1×10^-5, the equilibrium lies towards the products.

S° for Hg(l) is zero.

The number of microstates,W, is the number of smallest particles in a system.

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For a certain reaction at 25.0°C, the value of K is 5.8×10^-9. At 10.0°C the value of K is 3.4×10^-1. What does this tell you about the reaction?

The reaction is endothermic.

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This information is useless.

The reaction is exothermic.

The reaction is very tempermental.

The reaction rate increases.

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Consider the following reaction and its equilibrium constant:

H₂(g) + I₂(g) ⇌

2HI(g) K=50.3

A reaction mixture contains the following:

0.500 bar H₂

0.100 bar I₂

2.30 bar HI

A) Calculate Q for the above reaction for the amounts given. Express your answer to three significant figures.

Q =

B) Which position on the correct Gibbs energy plot does this value of Q correspond to?

C) What can you say happens to the reaction?

The system is at equilibrium.

The reaction will shift in the direction of products.

The reaction will shift in the direction of reactants

There is not enough information to determine this.

The equilibrium constant will increase.

The equilibrium constant will decrease.

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At constant pressure, the reaction A(g) → 2B(g)

is exothermic.

Which of the following statements is true for this reaction?

The reaction is spontaneous at low temperatures.

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is not possible to determine the spontaneity without more information.

The reaction is spontaneous at all temperatures.

The reaction is spontaneous at high temperatures.

The reaction is never spontaneous at any temperature.

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A particular reaction has Δ_rS = 45.3 J K^-1mol^-1 and Δ_rH = 75.1 kJ mol^-1. Calculate ΔS_univ for this reaction at 375 K. Express your answer to three significant figures.