1- Using graph below, find the following: a=1 for aA + bB → cC b=2 C=1 X5 A Х4 X3 X2 X1 10 15 20 25 30 35 40 45 50 Time (s) a. Find Q when t=0 b. How many additives and remove processes have been done? Find Q for all and tell at what time did that happened for each process? How many equilibriums state is reached? Also find Kc for all d. From t=19 to t=25 what was the direction of the reaction? Prove your answer From t=27 to t=44 what was the direction of the reaction? Prove your answer f. From t=45 to t=50 what was the direction of the reaction? Prove your answer g. If Kc increased when temperature is increased what is the type of such reaction? Explain why? с. е. Molarity (mol/L)

1- Using graph below, find the following: a=1 for aA + bB → cC b=2 C=1 X5 A Х4 X3 X2 X1 10 15 20 25 30 35 40 45 50 Time (s) a. Find Q when t=0 b. How many additives and remove processes have been done? Find Q for all and tell at what time did that happened for each process? How many equilibriums state is reached? Also find Kc for all d. From t=19 to t=25 what was the direction of the reaction? Prove your answer From t=27 to t=44 what was the direction of the reaction? Prove your answer f. From t=45 to t=50 what was the direction of the reaction? Prove your answer g. If Kc increased when temperature is increased what is the type of such reaction? Explain why? с. е. Molarity (mol/L)

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...

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Consider this equilibrium reaction at 400 K. Br, (g) + Cl, (g) 2 BrCl(g) K. = 7.0 If the composition of the reaction mixture at 400 K is [BrCl] = 0.00509 M, [Br,] = 0.00173 M, and [Cl,] = 0.000318 M, what is the reaction quotient, Q? Q = How is the reaction quotient related to the equilibrium constant, Ke, for this reaction? Q = Ke Q Kc
2NO(g) + 2H₂(g) = 2H₂O(g) + N₂(g) K = 0.110 AH° = -707 kJ What is the equilibrium constant for the reaction when it is altered as below? H₂O(g) + N₂(g) ⇒ NO(g) + H₂(g) K' = [?] K' Enter
Consider the following reaction: SO2Cl2 (g) SO2 (g) + Cl2 (g) A reaction mixture is made containing an initial [SO₂Cl₂] of 2.2x10-2 M. At equilibrium, [C1₂] = 1.1x10-² M. Calculate the value of the equilibrium constant (Kc). Express your answer using two significant figures. ΓΙ ΑΣΦ Kc = Submit Request Answer ?
■ W Chapter... G N. O LCG a Ⓒ BA H H The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (The system is considered in equilibrium if K, and Q are within 5% of each other.) (a) 2 NH3(g) = N₂(g) + 3 H₂(g) [NH3] = 0.485 M, [N₂]; = 0.160 M, [H₂] = 0.110 M, K = 18 What is the reaction quotient? What direction will the reaction shift to? O To the left, i.e. the reactant-side. O To the right, i.e. the product-side. O It will not shift. (b) 2 NH3(9) N₂(g) + 3 H₂(g) What is the reaction quotient? What direction will the reaction shift to? O To the left, i.e. the reactant-side. P (NH3) = 1.90 atm, P(N₂) = 11.65 atm, P(H₂) = 11.65 atm, K = 6.6x104 O To the right, i.e. the product-side. O It will not shift. (c) 2 SO 3(g) 2 SO₂(g) + O₂(9) What is the reaction quotient? webassign.net [SO3] = 1.65 M, [SO₂), = 1.65 M, [0₂], =…
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For the following reaction, N204(g) → 2NO2(g), the value of Ke is 1.2x10-5 at a certain temperature. If the reaction mixture is found to contain 0.0020 M NO2 and 0.0075 M N204, what is the value of Q and what does this mean? Periodic Table and Datasheet Q K and the reaction will proceed towards the reactants. Q > K and the reaction will proceed towards the products.
Consider the following equilibrium: N204(g) = 2NO2(g) Suppose two different experiments were conducted on this equilibrium, at two different temperatures. Trial Temperature Initial Moles of N204 Equilibrium Moles of N204 1 25°C 1.00 0.815 55°C 1.00 0.500 What conclusion may be drawn from the above data? O Kc> Kp at all temperatures. The reaction is exothermic. The forward reaction proceeds faster than the reverse reaction. OKp =D1 at 55°C. O The equilibrium constant increases with increasing temperature.
7. Consider the following reaction: HCH4 (g)+ 2 O2(g)<=> CO2 (g) + 2 H2O (g) Δ H = -658 kJ predict the equilibrium shift (R- right, L - left, N - no change) in the following situations: 1, The reactor is heated select R, N, L 2. o2 is injected in the reactor. SELECT L, R, N 3, H2O is injected in the reactor SELECT R, L, N 4,Helium is added and total pressure increased L, N, R 5. Catalyst is removed R, N, L 6, Reactor with a smaller volume is used. R, L, N