**Equilibrium Reaction and Calculation of \( K_p \):**Gaseous \(\text{NH}_3\) is placed in a closed container at **33 °C**, where it partially decomposes to \(\text{N}_2\) and \(\text{H}_2\), according to the following equilibrium reaction:\[ 2 \text{NH}_3(g) \rightleftharpoons 1 \text{N}_2(g) + 3 \text{H}_2(g) \]At equilibrium, the partial pressures are measured as follows:- \( p(\text{NH}_3) = 0.008450\) atm,- \( p(\text{N}_2) = 0.007140\) atm,- \( p(\text{H}_2) = 0.003440\) atm.**Objective:**Determine the value of \( K_p \) for this reaction at 33 °C.**Calculation:**The equilibrium constant \( K_p \) for the reaction is expressed as:\[K_p = \frac{(p(\text{N}_2) \times (p(\text{H}_2))^3)}{(p(\text{NH}_3))^2}\]Insert the given partial pressures into the expression to find \( K_p \).\[ K_p = \frac{(0.007140) \times (0.003440)^3}{(0.008450)^2} \]**Note to Educators:**Ensure students are aware that the units for partial pressures must be consistent when calculating \( K_p \). This exercise is useful for reinforcing concepts of chemical equilibrium and the use of equilibrium constants in gaseous reactions.

Gaseous NH3 is placed in a closed container at 33 °C, where it partially decomposes to N₂ and H₂: 2 NH3(g) = 1 N₂(g) + 3 H₂(g) At equilibrium it is found that p(NH3) = 0.008450 atm, p(N₂) = 0.007140 atm, and p(H₂) = 0.003440 atm. What is the value of Kp at this temperature? Kp =

Gaseous NH3 is placed in a closed container at 33 °C, where it partially decomposes to N₂ and H₂: 2 NH3(g) = 1 N₂(g) + 3 H₂(g) At equilibrium it is found that p(NH3) = 0.008450 atm, p(N₂) = 0.007140 atm, and p(H₂) = 0.003440 atm. What is the value of Kp at this temperature? Kp =

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...

See similar textbooks

Similar questions

Gaseous NH3 is placed in a closed container at 47 °C, where it partially decomposes to N₂ and H₂: 2 NH3(g) = 1 N₂(g) + 3 H₂(g) At equilibrium it is found that p(NH3) = 0.004010 atm, p(N₂) = 0.005080 atm, and p(H₂) = 0.003840 atm. What is the value of Kp at this temperature? Kp =
Consider the synthesis of ammonia: N2(g) + 3H2(g)<=>2NH3(g) At 926.5 °C, the equilibrium constant Kp is 4.09 × 10–5. What is the value of Kc?
A student ran the following reaction in the laboratory at 329 K: CH4(g) + CCl4(g) 2CH₂Cl₂(g) When he introduced CH4(g) and CCl4(g) into a 1.00 L evacuated container, so that the initial partial pressure of CH4 was 0.602 atm and the initial partial pressure of CCl4 was 0.262 atm, he found that the equilibrium partial pressure of CCl4 was 0.219 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр = ?
The reaction N₂O4(g) 2NO₂(g) has a Kp = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N₂O4 was 0.287 atm. (a) What was the partial pressure of NO₂ in the reaction mixture? pressure of NO₂ = atm (b) What was the total pressure of the mixture of gases? total pressure = i atm
A 2.0 mol sample of CO(g) and a 2.0 mol sample of H₂O(g) are introduced into a previously evacuated 100. L rigid container, and then temperature is held constant as the reaction below reaches equilibrium. Which of the following is true at equilibrium? CO(g) + H₂O(g) CO₂(g) + H₂(g) K = 1.5 × 103 (A) [H₂O] > [CO] and [CO₂] > [H₂] (B) [H₂O] > [H₂] (C) [CO₂] > [CO] (D) [CO] = [H,O] = [CO,] = [H2]
b For the reaction H2(g) + Br2(g)→ 2HB1(g) Kp = 3.4 x 104 at 1493 K. What is the value of K, for the following reaction at 1493 K? 2HB1(g) H2(g) + Br2(g) K"p=
A 10.0 g sample of liquid water is sealed in a 1515 mL flask and allowed to come to equilibrium with its vapor at 27 °C. What is the mass of H2O (g) present when equilibrium is established?
The two common chlorides of phosphorus, PCl3 and PCl5, both important in the production of other phosphorus compounds, coexist in equilibrium through the reaction PCl3 (g) +Cl2 (g) ⇌ PCl5 (g) At 250∘C, an equilibrium mixture in a 2.50−L flask contains 0.105 g PCl5, 0.235 g PCl3 and 2.27 g Cl2. What is the value of KC for this reaction at 250∘C? What is the value of KP for this reaction at 250∘C?
For the reaction PCL5 (g) = PCl3 (g) + Cl₂ (g) at equilibrium, Kp = 321. The equilibrium partial pressures of PCl3 and Cl₂ are 1.00E0 atm and 4.50E0 atm, respectively. What is the equilibrium partial pressure of PCl5?
Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4 (g) + H2O (g) ⇌ H2 (g) + CO (g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations, at a temperature of 760 °C? CH4 = 0.126 M H2O = 0.242 M CO = 0.126 M H2 = 1.15 M Please show Given, Required, Solution. Thank you very much.
The formation of nitrogen monoxide from its elements has an equilibrium which favors reactants: N2 (g) + 02 (g) 2 NO (g) K, = 0.0290 at 2400°C If the initial partíal pressures of both reactant gases are 0.717 atm, what will be the equilibrium partial pressure of nitrogen monoxide? (A certain simplification is valid in solving this problem). 0.112 atm (A) (B) 0.0290 atm (C) 0.688 atm (D) 0.0563 atm (E) 0.0611 atm
At 1000 K, a sample of pure NO2 gas decomposes: 2NO₂(g) 2NO(g) + O₂(g) The equilibrium constant, Kp, is 158. Analysis shows that the partial pressure of O₂ is 0.19 atm at equilibrium. Calculate the pressure of NO and NO₂ in the mixture.