estion 8At a certain temperature K for the reaction 2NO, NO4 is 7.5 liters/mole. If 2.0 moles of NO, are placedt yetsweredin a 2.0-liter container and permitted to react at this temperature, calculate the concentration of N,04 atarked out ofequilibrium.Select one:- Flag questionO a. 0.65 moles/literO b. 7.5 moles/literO C. none of theseO d. 0.82 moles/literO e. 0.39 moles/literType here to searchF4F5F6FZF8F108.EDGH

Answered: Image /qna-images/answer/4ce94b17-e1be-494b-aef0-88da28436cfb.jpg

At a certain temperature K for the reaction 2NO N2O4 is 7.5 liters/mole. If 2.0 moles of NO, are placed in a 2.0-liter container and permitted to react at this temperature, calculate the concentration of Ny04 at equilibrium. Select one: O a. 0.65 moles/liter O b. 7.5 moles/liter O C. none of these O d. 0.82 moles liter O e. 0.39 moles liter

At a certain temperature K for the reaction 2NO N2O4 is 7.5 liters/mole. If 2.0 moles of NO, are placed in a 2.0-liter container and permitted to react at this temperature, calculate the concentration of Ny04 at equilibrium. Select one: O a. 0.65 moles/liter O b. 7.5 moles/liter O C. none of these O d. 0.82 moles liter O e. 0.39 moles liter

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 moles each of CO and Br2 were placed into a 1L container and allowed to reach equilibrium, the resulting mixture contained .60 Moles of CO. How many moles of Br2 and C2O2Br2 are present at equilibrium? 2CO + Br2 <---> C2O2Br2
At 373 K, The Kc for the ff reaction is 0.078.Suppose 0.50 mol SO2 and 0.50 mol Cl2 are added to a 2.0 L container, what will be the concentration of SO2Cl2 at equilibrium? a. 13.32 Mb. 0.018 Mc. 5.075 x 10^-3 Md. 4.69 x 10^-3 Me. 7.16 M
A mixture of CO and Cl2 is placed in a reaction flask: [CO] = 0.0103 M and [Cl2] = 0.00610 M. At equilibrium, the concentration of Cl2 is 0.00311 M. Using an ICE table, calculate the equilibrium concentration of CO. a. 0.00731 M b. 0.00311 M c. 0.0103 M d. 0.0206 M e. 0.00299 M
The equilibrium constant is equal to 5.00 at 1300 K for the reaction: If initial concentrations are [SO2] = 0.60 M, [O2] = 0.20 M, and [SO3] = 0.50 M, the system is: A. at equilibrium B. Need to know the volume of the container before deciding. C. not at equilibrium and will shift to the right to achieve an equilibrium state D. not at equilibrium and will shift to the left to achieve an equilibrium state E. not at equilibrium and will remain in an unequilibrium state 2 SO2(g) + O2(g) ⇌ 2 SO3(g) Determine how the following changes affect the given equilblirium reaction that is held in a closed container. A(g) + 2 B(s) ⇌ 3 C(g) + 3 D(s) ΔH°rxn = −0.25 kJ/mol Adding some A(g) Adding some D(s) Removing some C(g) Increasing the temperature Halving the volume of the container The following mechanism is proposed for the reaction 2 A2 + B2 → 2 C A2 + B2 → R + C slow A2 + R → C fast What is the rate law…
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2 x 104 at a certain temperature. If a solid sample of NH.SH decomposes, what will the equilibrium concentration of NH3 be? NH:SH(s) = NH3(g) + H2S(g) 1 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. NH.SH(s) NH:(g) H2S(g) Initial (M) Change (M) Equilibrium (M) RESET 1.2 x 104 +x +2x -2x 1.2 x 104 + x 1.2 x 104 - x 1.2 x 104 + 2x 1.2 x 104- 2x
The equilibrium constants at a fixed temperature for several reactions are listed below. Which equilibrium constant indicates a reaction that is favored in the forward direction? a. Keq = 1.0 × 10^5 b. Keq = 1.0 × 10^-5 c. Keq = 1.0 d. Keq = 0.0 e. none of the above choices
For the system below at equilibrium, which changes will increase the amount of H2(g)? C(s) + H20(g) CO(g) + H2(g) AH>0 I. Adding C(s) II. Increasing the volume of the container III. Increasing the temperature a. I only b. III only c. II and III only d. I, II and III
Choose the process that will not disturb the following equilibrium. Co(g) + H20(g) CO2(g) + H2(g) O A. Adding co B. Increasing the temperature O C. Increasing the volume D. Removing H2
At a given temperature 0.80 mole of N, and 0.90 mole of H, were introduced in an evacuated 1.00 Iliter container. After equilibrium was established, the equilibrium concentrations were determined to be 0.20 mole of NH3, 0.70 moles N2, and 0.60 moles H2. Calculate K. for the reaction. WINE MO
The equilibrium constant, K, for the following reaction is 1.0 x 10 -5 at 1500 K. N2(g) + O2(g) <---> 2 NO(g) If 0.750 M N2 and 0.750 M O2 are allowed to reach equilibrium at 1500 K, what is the concentration of NO? a. 2.4 x 10-3M b. 6.7 x 10-4M c. 5.5 x 10-3M d. 2.7 x 10-3M e. 1.2 x 10-3M
Please answer all it’s my last question
18. Which equilibrium shows a decrease in [products] when the volume decreases? 1. 2H,(g)+O,(g) 2HI(g) d. III and IV 1I a. b. I and II IV e. C.