+6013011. The reaction SbFs (g) + 4 Cl2 (g) SbCl3 (g) + 5 CIF (g) has an equilibrium constantof 0.02 at 300°C. Portions of the SbFs (g) and Cl2 (g) are mixed at 300°C and each havea partial pressure of 0.12 atm before the reaction. What is the reaction quotient, Q, beforethe reaction?ba. 0.02d. 0.12b. 1e. 04/7c. 2.5x10-5

Step 1: Step 2: Step 3: Step 4:

Answered: +60130 11. The reaction SbFs (g) + 4…

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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#5 Q3
Consider this equilibrium reaction at 400 K. Br, (g) + Cl,(g) = 2 BICI(g) K. = 7.0 If the composition of the reaction mixture at 400 K is [BrCI] = 0.00248 M, [Br,] = 0.00570 M, and [Cl,] = 0.00105 M, what is the reaction quotient, Q? Q = How is the reaction quotient related to the equilibrium constant, Kç, for this reaction? Oe K. Oe = K.
. To which direction will the equilibrium of the reaction 2СО (g) + О2(g) 2СО2(g) be shifted after increase in pressure?
Consider the reaction: CO(g) + Cl₂(g) COC12 (g) € Kp At equilibrium, this reaction is At equilibrium, the rates of→ and reaction are equal. At equilibrium, reactant and product concentrations are constant. Reactions continue after equilibrium has been reached. Decreasing the temperature changes the K, value for this reaction. Removing COC1₂(g) changes the value of K, for this reaction. For the reaction: COCI, (g) = CO(g) + Cl₂(g), the value of K, is equal to 6.7 x 10¹1 at 25°C V V
Consider the following reaction at 25oC: A2(g) + B2(g) 2 AB(g) Which of the following statements is true? A. K > 1; at equilibrium there is more products than reactants. B. K > 1; at equilibrium there is more reactants than products. C. K < 1; at equilibrium there is more products than reactants. D. K < 1; at equilib thisrium there is more reactants than prroducts.
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
An equilibrium mixture contains 0.2500.250 mol of each of the products (carbon dioxide and hydrogen gas) and 0.2000.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g)+H2O(g)↽−−⇀CO2(g)+H2(g)CO(g)+H2O(g)⁢↽−−⇀⁢CO2⁢(g)+H2⁡(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.3000.300 mol once equilibrium has been reestablished? moles of CO2CO2 =
Consider the following reaction: 2 H20(g) + 2 SO2lg)=2 H2S(g) + 3 O2(g) A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2. Determine the equilibrium concentration of H2S if K. for the reaction at this temperature is 1.3 x 106. 0.058 M O 0.028 M O 0.045 M O 0.12 M O 3.1 x 10 M
The value of K, for the reaction 2 NO, (g) N204 (g) is 1.52 at 319 K. What is the value of the Kp of the reaction NO2 (g) 1/2 N204 (g) at this temperature: 0.761 O2.31 1.23 1.52 0.811 A Moving to another question will save this response. Esc AI C 中 F1 F2 F3 F4 F5 F6 F7 F8 F9 F10 23 %24
■ 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], =…
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 reaction 2SO2(g) + O2g) 2SO3(2) If K. = 4.3 x 10° and the following concentrations are present: [SO2] = 0.010 M, [SO3] = 10 M, [O2] = 0.01 M. Which of the following statements is correct? A. The system is at equilibrium B. The system is not at equilibrium and is shifting from left to right C. The system is not at equilibrium and is shifting from right to left D. There is not enough information E. The system is at equilibrium and is shifting from left to right 3.

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