Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- The reaction quotient, Q, for a system is 7.2 x 10^2. If the equilibrium constant for the system is 36, what will happen as equilibrium is approached? a) There will be a net gain in product b) There will be a net gain in reactant. c) There will be a net gain in both product and reactant. d) There will be no net gain in either product or reactant. e) The equilibrium constant will decrease until it equals the reaction quotient.arrow_forwardSetting up a reaction table Suppose a 500. mL flask is filled with 0.10 mol of H₂ and 0.60 mol of HI. This reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of H₂. You can leave out the M symbol for molarity. [H₂] [42] initial change equilibrium x [HI]arrow_forwardA chemical engineer is studying the following reaction: H₂(g) + Cl₂(g) → 2 HCl(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.33. The engineer charges ("fills") three reaction vessels with hydrogen and chlorine, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel A B с compound H₂ C1₂ HC1 H₂ CL, HCl H₂ CL₂2 HC1 pressure 4.42 atm 5.14 atm 1.90 atm 3.61 atm 4.33 atm 3.53 atm 4.59 atm 5.31 atm 1.57 atm expected change in pressure ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↓ decrease ↓decrease ↓ decrease ↓ decrease ↓ decrease ↓ decrease ↓decrease ↓decrease ↓ decrease (no change) (no change) (no change) (no change) (no change) (no change) (no…arrow_forward
- A chemical engineer is studying the following reaction: HCN(aq)+NH,(aq) → CN (aq)+NH(aq) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 1.0. The engineer charges ("fills") four reaction vessels with hydrogen cyanide and ammonia, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction compound concentration expected change in concentration vessel HCN 0.06 M O f increase OI decrease O (no change) NH, 0.22 M f increase OI decrease (no change) A CN 0.97 M increase I decrease (no change) NH, 1.23 M f increase OI decrease O (no change) HCN 0.53 M f increase OI decrease (no change) NH, 0.69 M f increase O I decrease (no change) В CN 0.50 M t increase OI decrease O (no change) NH, 0.76 M f increase Ot decrease (no change)…arrow_forwardGiven 0.50 mol of NOCI is placed in a one-liter reaction vessel at 700 K and after the system comes to equilibrium the concentration of NOCI became 0.440 M. What is the equilibrium constant? Given the reaction as: 2NOCI(g) → 2NO(g) +Cl2(g) 5.6 x 10-4 2.0 x 10-3 4.1 x 10-3 6.1 x 10-3 8.2 x 10-3arrow_forwardA chemical engineer is studying the following reaction: H₂(g)+I₂(g) → 2 HI(g) At the temperature the engineer picks, the equilibrium constant The engineer charges ("fills") three reaction vessels with hydrogen and iodine, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A B C compound H₂ 1₂ HI H₂ 1₂ HI H₂ 1₂ HI pressure 2.39 atm 3.83 atm 4.71 atm 2.82 atm 4.26 atm 3.85 atm 3.81 atm 5.76 atm 5.21 atm expected change in pressure ↑ increase increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase for this reaction is 1.2. р ↑ increase ↑ increase ↓ decrease ↓decrease ↓ decrease ↓ decrease ↓decrease ↓ decrease ↓ decrease ↓decrease ↓ decrease X (no change) (no change) (no change) (no change) (no change) (no change) (no change) (no change)…arrow_forward
- A chemical engineer is studying the following reaction: H₂(g) + Cl₂(g) → 2 HCl (g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.39. р The engineer charges ("fills") three reaction vessels with hydrogen and chlorine, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A B C compound H₂2 C1₂ HCl H₂ C12 H Cl H₂ C1₂ H Cl pressure 2.00 atm 2.71 atm 2.34 atm 2.70 atm 3.41 atm 0.93 atm 2.66 atm 3.37 atm 1.00 atm expected change in pressure ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↓ decrease ↓ decrease ↓ decrease ↓decrease ↓decrease ↓decrease ↓decrease ↓decrease ↓ decrease (no change) (no change) (no change) (no change) (no change) (no change) (no…arrow_forwardDraw the product(s) of the following reactions. CH3 H₂C-C-CEC-H OH 1. BH3/THF 2. H₂O₂/ aqueous NaOH • You do not have to consider stereochemistry. Separate multiple products using the + sign from the drop-down menu. • You do not have to explicitly draw H atoms. • If no reaction occurs, draw the organic starting material.arrow_forward2arrow_forward
- A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 CH₂(g) C₂H₂(g) + 3H₂(g) K₂=6. × 10 -8 He fills a reaction vessel at this temperature with 7.0 atm of methane gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of C₂H₂, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of C₂H₂ at right. Round your answer to 1 significant digit. 0 yes no atm x10 X Śarrow_forwardSulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 100. L tank with 42. mol of sulfur dioxide gas and 5.6 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 9.0 mol. Calculate the concentration equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K_ = ] x10arrow_forwardA chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 10 N,(9) + 2H,0(g) 2 NO(g) + 2H,(g) K,=4. × 10 He fills a reaction vessel at this temperature with 13. atm of nitrogen gas and 2.9 atm of water vapor. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of H,, using only the tools Oyes 24 K10 available to you within ALEKS? O no If you said yes, then enter the equilibrium pressure of H, at right. atm Round your answer to 1 significant digit. Explanation Check 2021 McGraw-Hill Education. All Rights Reserved Terms of Use Privacy Accessibility र hparrow_forward
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