Question

C. 3 D. 2 E. 4 7. Which of the following reactions MUST be a spontaneous process? A. An endothermic reaction with zero \( \Delta S_{r \times n} \) \( \qquad \) B. An exothermic reaction with positive \( \Delta S_{r \times n} \) \( \qquad \) C. An exothermic reaction with negative \( \Delta S_{r \times n} \times \) D. An endothermic reaction with positive \( \Delta S_{r x n} \) E. An endothermic reaction with negative \( \Delta S_{r \times n} \) \( x \) 8. Consider the reaction: \( 2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g}) \quad \mathrm{K}=1.8 \times 10^{2} \) The reaction chamber was initially filled with only \( \mathrm{SO}_{3}(\mathrm{~g}) \) at an unknown pressure. At equilibrium, the partial pressure of \( \mathrm{SO}_{3}(\mathrm{~g}) \) was determined to be \( 0.55 \mathrm{~atm} \). Calculate the partial pressure of \( \mathrm{O}_{2}(\mathrm{~g}) \) at equilibrium. \[ 2 \mathrm{SO}_{2}+\mathrm{O}_{2} \rightarrow 2 \mathrm{SO}_{3} \] A. \( 0.085 \mathrm{~atm} \) B. \( \quad 0.13 \mathrm{~atm} \) \[ K=\frac{\left[\mathrm{SO}_{3}\right]^{2}}{\left[\mathrm{SO}_{2}\right]^{2}+\left[\mathrm{O}_{2}\right]} \] C. \( 0.065 \mathrm{~atm} \) D. \( 0.055 \mathrm{~atm} \) \[ 1,8 \times 10^{2}=\frac{[0,55]^{2}}{x^{2}} \] E. \( \quad 0.075 \mathrm{~atm} \)

          C. 3
D. 2
E. 4
7. Which of the following reactions MUST be a spontaneous process?
A. An endothermic reaction with zero \( \Delta S_{r \times n} \) \( \qquad \)
B. An exothermic reaction with positive \( \Delta S_{r \times n} \) \( \qquad \)
C. An exothermic reaction with negative \( \Delta S_{r \times n} \times \)
D. An endothermic reaction with positive \( \Delta S_{r x n} \)
E. An endothermic reaction with negative \( \Delta S_{r \times n} \)
\( x \)
8. Consider the reaction: \( 2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g}) \quad \mathrm{K}=1.8 \times 10^{2} \)
The reaction chamber was initially filled with only \( \mathrm{SO}_{3}(\mathrm{~g}) \) at an unknown pressure. At equilibrium, the partial pressure of \( \mathrm{SO}_{3}(\mathrm{~g}) \) was determined to be \( 0.55 \mathrm{~atm} \). Calculate the partial pressure of \( \mathrm{O}_{2}(\mathrm{~g}) \) at equilibrium.
\[
2 \mathrm{SO}_{2}+\mathrm{O}_{2} \rightarrow 2 \mathrm{SO}_{3}
\]
A. \( 0.085 \mathrm{~atm} \)
B. \( \quad 0.13 \mathrm{~atm} \)
\[
K=\frac{\left[\mathrm{SO}_{3}\right]^{2}}{\left[\mathrm{SO}_{2}\right]^{2}+\left[\mathrm{O}_{2}\right]}
\]
C. \( 0.065 \mathrm{~atm} \)
D. \( 0.055 \mathrm{~atm} \)
\[
1,8 \times 10^{2}=\frac{[0,55]^{2}}{x^{2}}
\]
E. \( \quad 0.075 \mathrm{~atm} \)

C. 3
D. 2
E. 4
7. Which of the following reactions MUST be a spontaneous process?
A. An endothermic reaction with zero Δ Sr × n
B. An exothermic reaction with positive Δ Sr × n
C. An exothermic reaction with negative Δ Sr × n×
D. An endothermic reaction with positive Δ Sr x n
E. An endothermic reaction with negative Δ Sr × n
x
8. Consider the reaction: 2 SO2( g)+O2( g) ⇌ 2 SO3( g) K=1.8 × 10^2
The reaction chamber was initially filled with only SO3( g) at an unknown pressure. At equilibrium, the partial pressure of SO3( g) was determined to be 0.55 atm. Calculate the partial pressure of O2( g) at equilibrium.

2 SO2+O2→ 2 SO3

A. 0.085 atm
B. 0.13 atm

K=([SO3]^2)/([SO2]^2+[O2])

C. 0.065 atm
D. 0.055 atm

1,8 × 10^2=([0,55]^2)/(x^2)

E. 0.075 atm

Added by Jessica G.

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