At 200 C, the standard Gibbs free energy of the reaction: 3A + B <---> 2C + D is -15000 kJ/kmol. What is the reaction equilibrium constant?
Question
Solution 1
To calculate the reaction equilibrium constant (K), we can use the relationship between the standard Gibbs free energy change (ΔG°) and the equilibrium constant, which is given by the equation:
ΔG° = -RT ln(K)
Where:
- ΔG° is the standard Gibbs free energy change,
- R is the universal gas constant Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI
Similar Questions
At 298 K, H0 = -314 kJ/mol and S0 = -0.372 kJ/(K•mol). What is the Gibbs free energy of the reaction?A.-425 kJB.0.393 kJC.34,900 kJD.-203 kJ
In the equilibrium system N2(g) + 3H2(g) → 2NH3(g)Kc = 2.0 mol-2dm6 at 620 K. What is the value of Kp at this temperature.
If equilibrium constant is 2 at 300 K then the standard free energy change at 300 K and 1 atm pressure is
The cell in which the following reaction occurs has at 298 K. The standard Gibbs energy will be
Equilibrium pressure at which 50% of reactant A(g) will be consumed, keeping constant temperature of 300 K inthe given equilibrium is equal
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.