**Equilibrium Concentration Calculation:****Problem Statement:**5. The following reaction begins initially with 0.500 mol of H₂ and 0.500 mol of Br₂ in a 2.0 L flask. The reaction mixture has Kc = 64 at 427 °C. What are the equilibrium concentrations of each species (in M to two decimal places) at this temperature?\[ \text{H}_2(g) + \text{Br}_2(g) \rightleftharpoons 2\text{HBr}(g) \]**Solution:****Given Data:**- Initial moles of H₂ = 0.500 mol- Initial moles of Br₂ = 0.500 mol- Volume of the flask = 2.0 L- Equilibrium constant, Kc = 64- Temperature = 427 °C**Equilibrium Concentrations:**The equilibrium concentrations of each species are given as:- [H₂] = 0.05 M- [Br₂] = 0.05 M- [HBr] = 0.40 M**Answer (A):** 0.05, 0.05, 0.40This solution involves calculating the changes in concentration due to the reaction reaching equilibrium and applying the expression for Kc to solve for these equilibrium concentrations.

Answered: Image /qna-images/answer/03e351f1-11ed-4372-b091-15059478fde6.jpg

5. The following reaction begins initially with 0.500 mol of H₂ and 0.500 mol of Br₂ in a 2.0 L flask. The reaction mixture has K = 64 at 427 °C. What are the equilibrium concentrations of each species (in M to two decimal places) at this temperature? H₂(g) + Br₂(g) = 2HBr(g) A: 0.05, 0.05, 0.40

5. The following reaction begins initially with 0.500 mol of H₂ and 0.500 mol of Br₂ in a 2.0 L flask. The reaction mixture has K = 64 at 427 °C. What are the equilibrium concentrations of each species (in M to two decimal places) at this temperature? H₂(g) + Br₂(g) = 2HBr(g) A: 0.05, 0.05, 0.40

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

Consider the following chemical reaction and equilibrium constant at 20 °C :CH4 (g) + 2O2 (g) ⇌ 2H2O (g) + CO2 (g) K = 2.10 x 102Based on the previous chemical reaction, what is the equilibrium constant for the following reaction at 20 °C? (Please provide your answer to 3 significant figures in scientific notation (1.23*10^5)) 2CH4 (g) + 4O2 (g) ⇌ 4H2O (g) + 2CO2 (g) K = ?
The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) H2(g) + I2(g) An equilibrium mixture of the three gases in a 1.00 L flask at 698 K contains 0.314 M HI, 4.21×10-2 M H2 and 4.21×10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 2.56×10-2 mol of H2(g) is added to the flask? [HI] = M [H2] = M [I2] = M
At a certain temperature, the equilibrium constant K for the following reaction is 0.0036: H₂(g) + 1₂(g) → 2 HI(g) Use this information to complete the following table. O There will be very little H₂ and I2. Suppose a 6.0 L reaction vessel is filled with 1.9 mol of H₂ and 1.9 mol of I₂. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little HI. ONeither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 2 HI(g) H₂(9)+1₂(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 2 H₂(g) +21₂(g) 4 HI(g) 0x10 ?
The equilibrium constant, Kc, 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 0.228 moles of H2 and 0.228 moles of I2 are introduced into a 1.00 L vessel at 698 K. [ H2 ] = M [ I2 ] = M [ HI ] = M
The equilibrium constant, Kc, for the following reaction is 0.00650 at 298 K. 2NOBr(g) ⇒ 2NO(g) + Br₂ (g) If an equilibrium mixture of the three gases in a 15.6 L container at 298 K contains 0.201 mol of NOBr(g) and 0.284 mol of NO, the equilibrium concentration of Br₂ is | M.
At a certain temperature, the equilibrium constant k for the following reaction is 6.3 x 10*: NO,(g) + CO(g) = NO(g) + CO,(g) Use this information to complete the following table. Suppose a 40. L reaction vessel is filled with 1.1 mol of NO2 and 1.1 mol of Co. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little NO2 and CO. There will be very little NO and CO2. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = NO(9)+CO2(9) NO2(9)+CO(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = | 3 NO,(9)+3CO(9) 3 NO(9)+3CO2(9)