Question

In Part A, we saw that ΔG∘=−242.1 kJ for the hydrogenation of acetylene under standard conditions...

In Part A, we saw that ΔG∘=−242.1 kJ for the hydrogenation of acetylene under standard conditions (all pressures equal to 1 atm and the common reference temperature 298 K). In Part B, you will determine the ΔG for the reaction under a given set of nonstandard conditions.

At 25 ∘C the reaction from Part A has a composition as shown in the table below.

Substance Pressure
(atm)
C2H2(g) 5.35
H2(g) 3.95
C2H6(g) 4.25×10−2

What is the free energy change, ΔG, in kilojoules for the reaction under these conditions?

Express your answer numerically in kilojoules.

((Kp in Part A = 2.7 x 10^42 ))

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
In Part A, we saw that ΔG∘=−242.1 kJ for the hydrogenation of acetylene under standard conditions...
In Part A, we saw that ΔG∘=−242.1 kJ for the hydrogenation of acetylene under standard conditions (all pressures equal to 1 atm and the common reference temperature 298 K). In Part B, you will determine the ΔG for the reaction under a given set of nonstandard conditions. Part B At 25 ∘C the reaction from Part A has a composition as shown in the table below. Substance Pressure (atm) C2H2(g) 3.95 H2(g) 5.65 C2H6(g) 5.25×10−2 What is the free energy...
Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation. The reaction...
Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation. The reaction is C2H2(g)+2H2(g)⇌C2H6(g) Given the following data at standard conditions (all pressures equal to 1 atm and the common reference temperature 298 K), what is the value of Kp for this reaction? Substance ΔG∘f (kJ/mol) C2H2(g) 209.2 H2(g) 0 C2H6(g) −32.89 Express your answer using two significant figures.
Item 5 The equilibrium constant of a system, K, can be related to the standard free...
Item 5 The equilibrium constant of a system, K, can be related to the standard free energy change, ΔG, using the following equation: ΔG∘=−RTlnK where T is standard temperature in kelvins and R is the gas constant. Under conditions other than standard state, the following equation applies: ΔG=ΔG∘+RTlnQ In this equation, Q is the reaction quotient and is defined the same manner as K except that the concentrations or pressures used are not necessarily the equilibrium values. Part A Acetylene,...
Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation. The reaction...
Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation. The reaction is C2H2(g)+2H2(g)⇌C2H6(g) Given the following data at standard conditions (all pressures equal to 1 atm and the common reference temperature 298 K), what is the value of Kp for this reaction? Substaance .. G∘f (kJ/mol) C2H2(g)               209.2 H2(g) 0   C2H6(g)                -32.89   
The equilibrium constant of a system, K, can be related to the standard free energy change,...
The equilibrium constant of a system, K, can be related to the standard free energy change, ΔG∘, using the following equation: ΔG∘=−RTlnK where T is a specified temperature in kelvins (usually 298 K) and R is equal to 8.314 J/(K⋅mol). Under conditions other than standard state, the following equation applies: ΔG=ΔG∘+RTlnQ In this equation, Q is the reaction quotient and is defined the same manner as K except that the concentrations or pressures used are not necessarily the equilibrium values....
Part B At 25 ?C the reaction from Part A has a composition as shown in...
Part B At 25 ?C the reaction from Part A has a composition as shown in the table below. Substance/Pressure (atM): C2H2(g) / 4.05 H2(g) / 5.55 C2H6(g) / 5.25×10?2 What is the free energy change, ?G, in kilojoules for the reaction under these conditions? Express your answer numerically in kilojoules.
The equilibrium constant of a system, K, can be related to the standard free energy change,...
The equilibrium constant of a system, K, can be related to the standard free energy change, ΔG∘, using the following equation: ΔG∘=−RTlnK where T is a specified temperature in kelvins (usually 298 K) and R is equal to 8.314 J/(K⋅mol). Under conditions other than standard state, the following equation applies: ΔG=ΔG∘+RTlnQ In this equation, Q is the reaction quotient and is defined the same manner as K except that the concentrations or pressures used are not necessarily the equilibrium values....
± Free Energy and Chemical Equilibrium The equilibrium constant of a system, K, can be related...
± Free Energy and Chemical Equilibrium The equilibrium constant of a system, K, can be related to the standard free energy change, ΔG, using the following equation: ΔG∘=−RTlnK where T is standard temperature in kelvins and R is equal to 8.314 J/(K⋅mol). Under conditions other than standard state, the following equation applies: ΔG=ΔG∘+RTlnQ In this equation, Q is the reaction quotient and is defined the same manner as K except that the concentrations or pressures used are not necessarily the...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction C2H6(g)+H2(g)↽−−⇀2CH4(g) the standard change in Gibbs free energy is Δ?°=−69.0 kJ/mol. What is ΔG for this reaction at 298 K when the partial pressures are ?C2H6=0.300 atm, ?H2=0.500 atm, and ?CH4=0.950 atm?
Consider the following reaction occurring at 298 K: N2O(g)+NO2(g)⇌3NO(g) Part A Show that the reaction is...
Consider the following reaction occurring at 298 K: N2O(g)+NO2(g)⇌3NO(g) Part A Show that the reaction is not spontaneous under standard conditions by calculating ΔG∘rxn. Part B If a reaction mixture contains only N2O and NO2 at partial pressures of 1.0 atm each, the reaction will be spontaneous until some NO forms in the mixture. What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous? Part C Can the reaction be made more spontaneous by an...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT