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At a particular temperature, K,-100. If the temperature is 298 K, what is the value of K, for this reaction? H2(e) + Cl2e) --> 2HCI This problem doesn't necessarily require math work. x x, E E 12pt Paragraph 回 P fr B I U A - A

At a particular temperature, K,-100. If the temperature is 298 K, what is the value of K, for this reaction? H2(e) + Cl2e) --> 2HCI This problem doesn't necessarily require math work. x x, E E 12pt Paragraph 回 P fr B I U A - A

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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### Equilibrium Constants in Chemical Reactions At a particular temperature, \( K_p = 100 \). If the temperature is 298 K, what is the value of \( K_c \) for this reaction? \[ \text{H}_2 (g) + \text{Cl}_2 (g) \rightarrow 2\text{HCl} (g) \] This problem doesn't necessarily require math work. #### Explanation: In the problem provided, the equilibrium constant for the reaction written in the form of partial pressures (\( K_p \)) is given as 100 at a certain temperature. The goal is to determine the equilibrium constant in terms of concentrations (\( K_c \)) at the specified temperature of 298 K. The reaction given is: \[ \text{H}_2 (g) + \text{Cl}_2 (g) \rightarrow 2\text{HCl} (g) \] Note: This problem may not require actual calculations, depending on the context provided in the educational material. We are often able to interrelate \( K_p \) and \( K_c \) through the equation: \[ K_p = K_c(RT)^{\Delta n} \] where: - \( K_p \) is the equilibrium constant in terms of partial pressure, - \( K_c \) is the equilibrium constant in terms of concentration, - \( R \) is the universal gas constant (0.0821 L·atm/(K·mol)), - \( T \) is the temperature in Kelvin, - \( \Delta n \) is the change in the number of moles of gas (moles of gaseous products - moles of gaseous reactants). In this case: - \( \Delta n = 2 - (1 + 1) = 0 \) When \( \Delta n \) equals zero: \[ K_p = K_c \] This implies that \( K_p \) is equal to \( K_c \) at the given temperature of 298 K, since \( (RT)^0 = 1 \). Therefore: \[ K_c = K_p = 100 \] There are no graphs or diagrams included that need further explanation.
Transcribed Image Text:### Equilibrium Constants in Chemical Reactions At a particular temperature, \( K_p = 100 \). If the temperature is 298 K, what is the value of \( K_c \) for this reaction? \[ \text{H}_2 (g) + \text{Cl}_2 (g) \rightarrow 2\text{HCl} (g) \] This problem doesn't necessarily require math work. #### Explanation: In the problem provided, the equilibrium constant for the reaction written in the form of partial pressures (\( K_p \)) is given as 100 at a certain temperature. The goal is to determine the equilibrium constant in terms of concentrations (\( K_c \)) at the specified temperature of 298 K. The reaction given is: \[ \text{H}_2 (g) + \text{Cl}_2 (g) \rightarrow 2\text{HCl} (g) \] Note: This problem may not require actual calculations, depending on the context provided in the educational material. We are often able to interrelate \( K_p \) and \( K_c \) through the equation: \[ K_p = K_c(RT)^{\Delta n} \] where: - \( K_p \) is the equilibrium constant in terms of partial pressure, - \( K_c \) is the equilibrium constant in terms of concentration, - \( R \) is the universal gas constant (0.0821 L·atm/(K·mol)), - \( T \) is the temperature in Kelvin, - \( \Delta n \) is the change in the number of moles of gas (moles of gaseous products - moles of gaseous reactants). In this case: - \( \Delta n = 2 - (1 + 1) = 0 \) When \( \Delta n \) equals zero: \[ K_p = K_c \] This implies that \( K_p \) is equal to \( K_c \) at the given temperature of 298 K, since \( (RT)^0 = 1 \). Therefore: \[ K_c = K_p = 100 \] There are no graphs or diagrams included that need further explanation.
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