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r which one of the following reactions is Kp equal to Kc? NH41(s) = NH3(g) + HI(g) 2NH3(g) = 3H₂(g) + N₂(g) CaCO3(s) CaO(s) + CO₂(g) = 302(g) = 203(g) SnO₂(s) + 2H₂(g) = Sn(s) + 2H₂O(g)

r which one of the following reactions is Kp equal to Kc? NH41(s) = NH3(g) + HI(g) 2NH3(g) = 3H₂(g) + N₂(g) CaCO3(s) CaO(s) + CO₂(g) = 302(g) = 203(g) SnO₂(s) + 2H₂(g) = Sn(s) + 2H₂O(g)

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
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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**Title: Understanding the Relationship Between \( K_p \) and \( K_c \) in Chemical Reactions** **Introduction:** In chemistry, the equilibrium constant can be expressed in terms of concentration (\( K_c \)) or pressure (\( K_p \)). The relationship between \( K_p \) and \( K_c \) depends on the change in the number of gas moles during the reaction. When the change in the number of moles of gas, \(\Delta n\), is zero, \( K_p \) equals \( K_c \). **Question:** For which one of the following reactions is \( K_p \) equal to \( K_c \)? **Options:** 1. \( \text{NH}_4\text{I(s)} \rightarrow \text{NH}_3\text{(g)} + \text{HI(g)} \) 2. \( 2\text{NH}_3\text{(g)} \rightarrow 3\text{H}_2\text{(g)} + \text{N}_2\text{(g)} \) 3. \( \text{CaCO}_3\text{(s)} \rightarrow \text{CaO(s)} + \text{CO}_2\text{(g)} \) 4. \( 3\text{O}_2\text{(g)} \rightarrow 2\text{O}_3\text{(g)} \) 5. \( \text{SnO}_2\text{(s)} + 2\text{H}_2\text{(g)} \rightarrow \text{Sn(s)} + 2\text{H}_2\text{O(g)} \) **Analysis:** To determine the correct answer, calculate \(\Delta n\) for each reaction, where \(\Delta n\) is the change in the moles of gases between the reactants and products. - **Reaction 1:** \(\Delta n = 2 - 0 = 2\) - **Reaction 2:** \(\Delta n = (3 + 1) - 2 = 2\) - **Reaction 3:** \(\Delta n = 1 - 0 = 1\) - **Reaction 4:** \(\Delta n = 2 - 3 = -1\) - **Reaction 5:** \(\
Transcribed Image Text:**Title: Understanding the Relationship Between \( K_p \) and \( K_c \) in Chemical Reactions** **Introduction:** In chemistry, the equilibrium constant can be expressed in terms of concentration (\( K_c \)) or pressure (\( K_p \)). The relationship between \( K_p \) and \( K_c \) depends on the change in the number of gas moles during the reaction. When the change in the number of moles of gas, \(\Delta n\), is zero, \( K_p \) equals \( K_c \). **Question:** For which one of the following reactions is \( K_p \) equal to \( K_c \)? **Options:** 1. \( \text{NH}_4\text{I(s)} \rightarrow \text{NH}_3\text{(g)} + \text{HI(g)} \) 2. \( 2\text{NH}_3\text{(g)} \rightarrow 3\text{H}_2\text{(g)} + \text{N}_2\text{(g)} \) 3. \( \text{CaCO}_3\text{(s)} \rightarrow \text{CaO(s)} + \text{CO}_2\text{(g)} \) 4. \( 3\text{O}_2\text{(g)} \rightarrow 2\text{O}_3\text{(g)} \) 5. \( \text{SnO}_2\text{(s)} + 2\text{H}_2\text{(g)} \rightarrow \text{Sn(s)} + 2\text{H}_2\text{O(g)} \) **Analysis:** To determine the correct answer, calculate \(\Delta n\) for each reaction, where \(\Delta n\) is the change in the moles of gases between the reactants and products. - **Reaction 1:** \(\Delta n = 2 - 0 = 2\) - **Reaction 2:** \(\Delta n = (3 + 1) - 2 = 2\) - **Reaction 3:** \(\Delta n = 1 - 0 = 1\) - **Reaction 4:** \(\Delta n = 2 - 3 = -1\) - **Reaction 5:** \(\
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Kp is equilibrium constant expressed as when equilibrium concentration is measured by atmospheric pressure.   Kc is equilibrium constant expressed as when equilibrium concentration is measured by molarity 

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