### Chemical Equilibrium Problem**Consider the following reaction:**\[ \text{PCl}_5(\text{g}) \rightleftharpoons \text{PCl}_3(\text{g}) + \text{Cl}_2(\text{g}) \]If \( 3.07 \times 10^{-2} \) moles of \( \text{PCl}_5(\text{g}) \), 0.456 moles of \( \text{PCl}_3 \), and 0.620 moles of \( \text{Cl}_2 \) are at equilibrium in a 18.9 L container at 613 K, the value of the equilibrium constant, \( K_c \), is _______.

Dear student I have given answer to your question in the image format.

Answered: (g) PCI3(g) + Cl,(g) 7×10² moles of…

Science

Chemistry

(g) PCI3(g) + Cl,(g) 7×10² moles of PCI5(g), 0.456 moles of PCI3, and 0.620 moles of Cl, are at equilibriu

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

When 1.0 mol each of H2(g) and I2(g) are mixed at a certain temperature, they react to give a final mixture consisting of 0.50mol each of H2(g) and I2(g) and 1.0 mol HI(g). Why do you obtain the same final mixture when you bring 2.0 mol HI(g) to the same temperature?
t a certain temperature, 0.36110.3611 mol of N2N2 and 1.6611.661 mol of H2H2 are placed in a 4.504.50 L container. N2(g)+3H2(g)↽−−⇀2NH3(g)N2(g)+3H2(g)↽−−⇀2NH3(g) At equilibrium, 0.12010.1201 mol of N2N2 is present. Calculate the equilibrium constant, ?cKc.
At 400 K, N₂O4 decomposes into NO₂ in the gas phase: N₂O4(8) 2NO₂(g) In an experiment, 0.328 g of of N₂O4(g) were placed in a 0.500 L evacuated flask at 400 K, and allowed to come to equilibrium, the final pressure was 0.331 atm. What were the partial pressures of N₂O4 and NO2, and what is the equilibrium constant? PN204 = i PNO2 = i Kc = i kada atm atm
2H₂S(g) 2H₂(g) + S₂(g) At equilibrium, there are 0.06605 mol H2 in the 0.500 L container. Calculate the partial pressure of H2 in the container at 490 K. PH₂ = [?] atm P of H,, atm Enter
Consider the following reaction where Kc = 55.6 at 698 K. H2(g) + I2(g) ----> 2HI(g) A reaction mixture was found to contain 4.26×10-2 moles of H2(g), 4.04×10-2 moles of I2(g) and 0.270 moles of HI(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 (fill in the blank) ____ A. must run in the forward direction to reach equilibrium.B. must run in the reverse direction to reach equilibrium.C. is at equilibrium.
Please do it...
In a 3.0 L vessel, the following equilibrium partial pressures were measured at a certain temperature. N2(g) + 3 H2(g) 2 NH3(g) Peq(N2) = 186 torr, Peq(H2) = 318 torr, Peq(NH3) = 988 torr Nitrogen is removed from the vessel until the partial pressure of hydrogen, at equilibrium, is 394 torr. Calculate the partial pressures (in torr) of the other substances under the new conditions. P(NH3) torrP(N2) torr
need it will upvote
physical chem
= [Review Topics] [References] Use the References to access important values if needed for this question. The equilibrium constant, Ke, for the following reaction is 10.5 at 350. K. 2CH₂Cl2 (9) CH4 (9) + CCl4 (9) = Calculate the equilibrium concentrations of reactant and products when 0.315 moles of CH₂Cl2 (g) are introduced into a 1.00 L vessel at 350. K. [CH₂Cl₂] = [CH4] [CC14] = = Submit Answer Show Hint NOV 30 Q F4 M M M Retry Entire Group 9 F5 + tv ♫ 8 9 more group attempts remaining MacBook Air C F6 < F7 DII F8 Previous Email Instructor F9 O Next Save and Exit J F10
Gaseous NO is placed in a closed container at 477 oC, where it partially decomposes to NO2 and N2O: 3 NO(g) 1 NO2(g) + 1 N2O(g) At equilibrium it is found that p(NO) = 0.009840 atm, p(NO2) = 0.008270 atm, and p(N2O) = 0.008870 atm. What is the value of KP at this temperature?KP =
Consider the following reaction where Kc = 55.6 at 698 K. H2(g) + I2(g) ----> 2HI(g) A reaction mixture was found to contain 4.26×10-2 moles of H2(g), 4.04×10-2 moles of I2(g) and 0.270 moles of HI(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 (fill in the blank) ____ A. must run in the forward direction to reach equilibrium.B. must run in the reverse direction to reach equilibrium.C. is at equilibrium.