**Equilibrium Constant and Partial Pressure Calculation**The equilibrium constant, \( K_p \), for the reaction is given as \( 1.04 \times 10^{-2} \) at a temperature of 548 K.**Chemical Reaction:**\[ \text{NH}_4\text{Cl}(s) \rightleftharpoons \text{NH}_3(g) + \text{HCl}(g) \]**Problem Statement:**In an equilibrium mixture of the three compounds within a 6.78 L container at 548 K, the following quantities are present:- 2.85 mol of \(\text{NH}_4\text{Cl}(s)\) - 0.113 mol of \(\text{NH}_3(g)\)**Question:**Calculate the partial pressure of \(\text{HCl}(g)\) in the system. **Explanation:**This problem requires the application of the equilibrium constant to determine the unknown partial pressure of HCl in a gaseous state, given the state of the reaction at equilibrium.

Answered: Image /qna-images/answer/a97abf05-4a94-4600-a7eb-85769c146dda.jpg

The equilibrium constant, Kp, for the following reaction is 1.04x10-² at 548 K. NH4Cl(s) NH3(g) + HCI(g) If an equilibrium mixture of the three compounds in a 6.78 L container at 548 K contains 2.85 mol of NH4CI(s) and 0.113 mol of NH3(9), the partial pressure of HCI(g) is atm.

The equilibrium constant, Kp, for the following reaction is 1.04x10-² at 548 K. NH4Cl(s) NH3(g) + HCI(g) If an equilibrium mixture of the three compounds in a 6.78 L container at 548 K contains 2.85 mol of NH4CI(s) and 0.113 mol of NH3(9), the partial pressure of HCI(g) is atm.

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

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 = ?
While ethanol (CH3CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 25 L tank with 1.9 mol of ethylene gas and 5.7 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 0.97 mol of ethylene gas and 4.77 mol of water vapor. The engineer then adds another 0.95 mol of ethylene, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. mol x10 X
The equilibrium constant, Kp , for the following reaction is 0.215 at 673 K.NH4I(s) NH3(g) + HI(g)If an equilibrium mixture of the three compounds in a 7.23 L container at 673 K contains 2.70 mol of NH4I(s) and 0.128 mol of NH3(g), the partial pressure of HI(g) is atm.
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K.PCl3(g) + Cl2(g) PCl5(g)Calculate the equilibrium concentrations of reactant and products when 0.271 moles of PCl3 and 0.271 moles of Cl2 are introduced into a 1.00 L vessel at 500 K.
Consider the following reaction where K. = 1.29x102 at 600 K. COCl»(g) eCO(g) + Cl2(g) A reaction mixture was found to contain 0.107 moles of COCI,(g), 2.44x102 moles of CO(g), and 4.39×102 moles of Cl2(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.
The equilibrium constant, Kp, for the following reaction is 1.04×10-² at 548 K. NH4CI(S)2NH3(g) + HCI(g) If an equilibrium mixture of the three compounds in a 6.72 L container at 548 K contains 1.63 mol of NH4Cl(s) and 0.190 mol of NH3(g), the partial pressure of HCI(g) is I atm.
Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)
: Given : A (g) +B (g) 2C (g) An equilibrium mixture contains 0,5 mol of each of A and B and 3.5 mol of C in one-liter container at a certain temperature. (a) How many moles of C must be added to the con- tainer to increase the new equilibrium mole number of A to 0.75? (b) If 1 mol of each of A, B and C is added to the first equilibrium mixture, what will be the new equi- librium concentration of each species at the same temperature?
In a particular experiment 1.0 mole of H2O (g) and 1.0 mole of CO (g) are put into a flask and heated to 350 oC. In another experiment 1.0 mol of H2 (g) and 1.0 mole of CO2 (g) are put into a different flask with the same volume as the first. This mixture is also heated to 350 oC. After equilibrium is reached, will there be any difference in the composition of the mixture in the two flasks?
For the equilibrium N2O4(g) <----> 2 NO2(g), at 298 K, Kp = 0.15. For this reaction system, it is found that the partial pressure of N2O4 is 3.7 × 10^–2 atm at equilibrium. What is the partial pressure of NO2 at equilibrium?
The equilibrium constant, K., for the following reaction is 55.6 at 698 K. H2 (g) + I2 (g) = 2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.351 moles of H, and 0.351 moles of I, are introduced into a 1.00 L vessel at 698 K. [H2 ] = M [I ] M [HI ] = M
A student ran the following reaction in the laboratory at 588 K: CO(g) + Cl₂(g) —COCI₂(g) When she introduced CO(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 1.74 atm and the initial partial pressure of Cl2 was 0.951 atm, she found that the equilibrium partial pressure of COCI₂ was 0.685 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр =