### Equilibrium Constants in Chemical ReactionsAt 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.

The relationship between Kc and Kp is given as, Kp=KcRT∆n Here, ∆n=Moles of gaseous products-Moles…

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

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

### 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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