For the following reaction, cO (g) + H20 (g) CO2 (g) + H2 (g) Kc = 1.845 a. Write the Kc expression for this reaction. b. If a 1.00L vessel is charged with 0.250 moles of CO, 0.250 moles of H2O, 0.450 moles of CO2, and 0.450 moles of H2, what is the value of Q? c. In which direction does the reaction progress to establish equilibrium? d. What are the equilibrium concentration of all species? Attach File Browse Local Files

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For the following reaction,

\[ \text{CO (g)} + \text{H}_2\text{O (g)} \leftrightharpoons \text{CO}_2\text{ (g)} + \text{H}_2 \text{ (g)} \]

\[ K_c = 1.845 \]

a. Write the \( K_c \) expression for this reaction.

b. If a 1.00 L vessel is charged with 0.250 moles of CO, 0.250 moles of \( \text{H}_2\text{O} \), 0.450 moles of \( \text{CO}_2 \), and 0.450 moles of \( \text{H}_2 \), what is the value of Q?

c. In which direction does the reaction progress to establish equilibrium?

d. What are the equilibrium concentrations of all species?
Transcribed Image Text:For the following reaction, \[ \text{CO (g)} + \text{H}_2\text{O (g)} \leftrightharpoons \text{CO}_2\text{ (g)} + \text{H}_2 \text{ (g)} \] \[ K_c = 1.845 \] a. Write the \( K_c \) expression for this reaction. b. If a 1.00 L vessel is charged with 0.250 moles of CO, 0.250 moles of \( \text{H}_2\text{O} \), 0.450 moles of \( \text{CO}_2 \), and 0.450 moles of \( \text{H}_2 \), what is the value of Q? c. In which direction does the reaction progress to establish equilibrium? d. What are the equilibrium concentrations of all species?
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