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Consider the Following System at Equilibrium at 25°C:
PCl₃(g)+ Cl₂(g) $\Delta$

question 22

Multiple Choice

Consider the following system at equilibrium at 25°C:
PCl₃(g) + Cl₂(g) $Consider the following system at equilibrium at 25°C: PCl3(g) + Cl2(g) PCl5(g) for which \Delta H° = -92.5kJ at 25°C. -Water gas,a commercial fuel,is made by the reaction of hot coke carbon with steam. C(s) + H2O(g) CO(g) + H2(g) When equilibrium is established at 844°C the concentrations of CO,H2,and H2O are 4.00 \times 10-2,4.00 \times 10-2,and 1.00 \times 10-2 mole/liter,respectively.Calculate the value of \Delta G° for this reaction at 844°C. A) 12.9 kJ B) -12.87 kJ C) 55.64 kJ D) 17.02 kJ E) none of these$ PCl₅(g)
for which $\Delta$ H° = -92.5kJ at 25°C.
-Water gas,a commercial fuel,is made by the reaction of hot coke carbon with steam. C(s) + H₂O(g) $Consider the following system at equilibrium at 25°C: PCl3(g) + Cl2(g) PCl5(g) for which \Delta H° = -92.5kJ at 25°C. -Water gas,a commercial fuel,is made by the reaction of hot coke carbon with steam. C(s) + H2O(g) CO(g) + H2(g) When equilibrium is established at 844°C the concentrations of CO,H2,and H2O are 4.00 \times 10-2,4.00 \times 10-2,and 1.00 \times 10-2 mole/liter,respectively.Calculate the value of \Delta G° for this reaction at 844°C. A) 12.9 kJ B) -12.87 kJ C) 55.64 kJ D) 17.02 kJ E) none of these$ CO(g) + H₂(g)
When equilibrium is established at 844°C the concentrations of CO,H₂,and H₂O are 4.00 $\times$ 10^-²,4.00 $\times$ 10^-²,and 1.00 $\times$ 10^-² mole/liter,respectively.Calculate the value of $\Delta$ G° for this reaction at 844°C.

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Consider the Following System at Equilibrium at 25°C: PCl3(g)+ Cl2(g) Δ\DeltaΔ

Definitions:

Consider the Following System at Equilibrium at 25°C:
PCl₃(g)+ Cl₂(g) $\Delta$