The table below shows the equilibrium % pressures and temperatures. of product in a mixture of A, B and C at vario Please note that A, B and C are all gases Pressure (bar) Temperature 100 200 1000 100 10 25 30 98 20 70 Consider the following possible reactions Reaction 1: Reaction 2: A+2B C A+B=>2C What is the correct answer? A. The values in the table represent Reaction 1 and this reaction is endothermic B. The values in the table represent Reaction 2 and this reaction is endothermic C. The values in the table represent Reaction land this reaction is exothermic D. The values in the table represent Reaction 2 and this reaction is exothermic

The table below shows the equilibrium % pressures and temperatures. of product in a mixture of A, B and C at vario Please note that A, B and C are all gases Pressure (bar) Temperature 100 200 1000 100 10 25 30 98 20 70 Consider the following possible reactions Reaction 1: Reaction 2: A+2B C A+B=>2C What is the correct answer? A. The values in the table represent Reaction 1 and this reaction is endothermic B. The values in the table represent Reaction 2 and this reaction is endothermic C. The values in the table represent Reaction land this reaction is exothermic D. The values in the table represent Reaction 2 and this reaction is exothermic

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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A gas mixture consists of 3.74 atm of C₂H5Br, 4.22 atm of HBr, 0.11 atm of C₂H6, and 0.882 atm of Br₂. Calculate the reaction quotient for this system prior to the establishment of the equilibrium below. C₂H5Br(g) + HBr(g) = C₂H6(g) + Br₂(g) Report your answer to three significant figures in scientific notation. Submit Answer Tries 0/5
Calculate the Keg from the given concentrations, all are gases. C2H6 1.000 M 2 Cl2 1.000 M C2H4CI2 + 0.000 M 0.250 M + 2 HCI start: 0.000 M equilibrium: 0.750 M 0.500 M 0.500 M 0.500 M used First put in the chemicals, then put in the numbers. The concentrations for both Cl2 and HCl are squared due to their coefficients. [ Kea %3D Keg = a. H3O*1 b. Он1 c. C2H6 d. C2HĄCI2 e. Cl2 f. HCI g. H2SO3 h. HC2H3O2 i. C2H3O21 j. H2S k. HS-1 I. s2 m. HX п. X1 o. 0.750 р. 2 q. 1 r. 0.250 s. 0.500 t. 0.333 u. 8.00 х 10-5 v. 1.75 x 10-6 w. 1.11 x 10-8 x. 5.5 x 10-2 у. О.7000 z. 1.60 x 10-5 aа. 1.143 х 10-5 bb. 0.6000 СС. 1.104 х 10-5 dd. 0.7100 ее. 1.26 х 10-5 ff. 4.901 gg. 7.93 hh. 4.942 ii. 4.957
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■ 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], =…
Consider the following equilibrium: N₂(g) + 3H₂(g)2NH3(g) AG = -34. KJ Now suppose a reaction vessel is filled with 3.40 atm of hydrogen (H₂) and 9.24 atm of ammonia system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. rise O fall yes Ono X (NH3) at 736. °C. Answer the following questions about this S
The reaction mixture below contains 0.112 atm of H2, 0.077 atm of S2, and 0.224 atm of H2S. 2 H2S(g) 2 H2(g) + S2(g) K, = 2.4x104 at a particular temperature. Based on the information provided, select the correct relationship. O Q > K; the reaction will proceed to form more H2S(g). O More experimental data are always needed to answer a question like this. OQ < K; the reaction will proceed to form more products. OQ= K; the reaction is at equilibrium and no change is expected.
Consider the equilibrium, 2 NO (g) N2₂ (g) + O₂ (g), 2 for which AH = -180 kJ mol-1. How will adding more N₂ (g) affect an equilibrium mixture of the three gases? Select one: a. Reaction will proceed to the right (in the forward direction) to generate more product. b. Reaction will proceed to the left (in the reverse direction) to generate more product. C. Reaction will proceed to the right (in the forward direction) to generate more reactant. d. Reaction will proceed to the left (in the reverse direction) to generate more reactant. e. There will be no change to equilibrium mixture.
▸ 69 20 E Consider the following system at equilibrium at 723 K: N₂(g) + 3H₂(g) 2NH3(g) + 26.6 kcal Indicate whether each individual change would favor the production of NH3(g). Evaluate each change separately, assuming that all other conditions remain constant. D Decreasing the temperature. Decreasing the pressure. Increasing the volume. Removing NH3. Removing H₂. C Submit Answer $ 4 R F % 5 V Retry Entire ♫ FS T G [References] the References to access important values if needed for this question. A 6 v yes no B MacBook Air F6 3 more group attempts remaining Y H & 7 B F7 U N * 8 00 D--ll FB J J ( T 1 M 9 K DD FO O O L ge A F10 P command Previous Email Instructor 4 i A AN = Next> Save and Exit ( { ? 912 option delete retu