60) The following are the values of the equilibrium constant, K, for four different chemical reaction systems. For each of the chemical reaction systems, describe the equilibrium position of the given temperature as mostly products, mostly reactants, or equal concentrations of reactants and products. a) K= 10-12 at 25 °C

60) The following are the values of the equilibrium constant, K, for four different chemical reaction systems. For each of the chemical reaction systems, describe the equilibrium position of the given temperature as mostly products, mostly reactants, or equal concentrations of reactants and products. a) K= 10-12 at 25 °C

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

Given this equilibrium 2A(g)+3B———C(g)+4D+ energy Discuss what happens to this equilibrium if the temperature increases while the pressure is held constant. Make sure to include a discussion of rates of the forward and reverse reactions as well as changes in the concentrations of A, B, C and D.
A chemical engineer is studying the following reaction: 2 NO(g)+2H,(g) – N(a)+2H,0(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.17. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, 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. db Predict the changes in the compositions the engineer should expect next time she measures the compositions. Ar reaction vessel compound pressure expected change in pressure NO 7.34 atm Ot increase OI decrease O (no change) H, 1.96 atm O f increase OI decrease O (no change) N 1.66 atm O t increase OI decrease O (no change) H,0 10.20 atm O f increase OI decrease O (no change) NO 9.18 atm O t increase OI decrease O (no change) H. 3.80 atm O f increase OI decrease O (no change) B N, 0.74 atm O f increase OI decrease O (no change) HO 8.36 atm O f…
Consider the following endothermic reaction at 345.0 °C HBr (g) = > H2 (g) + Bi2 (g) Kp=4.18×10^-9 A reaction vessel initially contains a partial pressure of HBr of 0.20 atm. Calculate: 1) the equilibrium pressure of HBr2(g) in atm 2) the equilibrium constant kc for this reaction at this temperature
Consider the following chemical equilibrium: A(s) + B(g) ⇄ 3 C(s) + 4 D(g) If the initial pressure of B is 4.26 bar, the total pressure at equilibrium is 7.15 bar. Use these pressures to calculate Keq.
Write the equilibrium constant expression. Solid carbon and carbon dioxide gas react and form carbon monoxide: C(s) + CO₂(g) = 2CO(g)
A chemical engineer is studying the following reaction: N₂(g) + 3H₂(g) → 2 NH3(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.018. The engineer charges ("fills") three reaction vessels with nitrogen and hydrogen, 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 compound pressure expected change in pressure N₂ 11.46 atm ↑ increase ↓decrease (no change) H, 18.35 atm A ↑ increase ↓ decrease (no change) NH3 32.54 atm ↑ increase (no change) N₂ 10.77 atm ↑ increase ↓ decrease ↓decrease ↓decrease decrease B H₂ 16.30 atm (no change) (no change) (no change) ↑ increase 33.91 atm ↑ increase NH3 N₂₂ 11.20 atm ↑ increase ↓ decrease (no change) H₂ 17.58 atm с ↑ increase ↓decrease (no change) NH₂ 33.05 atm ↑…
An equilibrium mixture contains 0.700 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 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) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished? moles of CO₂ I mol
Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 200. mL flask with 1.1 atm of ammonia gas, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 1.2 atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = 0 P X Ś
Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O2(g)→2 HgO(5) At a certain temperature, a chemist finds that a 3.6 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound amount Hg 9.7 g O2 21.8 g HgO 10.2 g Calculate the value of the equilibrium constant K̟ for this reaction. Round your answer to 2 significant digits. K_ = 0
Nitrosyl bromide decomposes to NO and Br2 in an endothermic process (A,H° = 16.3 kJ/mol-rxn). 2 NOBr(g) ⇒ 2 NO(g) + Br2 (g) Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. a. adding more NOBr(g) shift left shift right O no change b. adding more Br₂(g) shift left shift right O no change c. increasing the volume of the reaction flask shift left shift right O no change d. lowering the temperature shift left shift right O no change
Calcium oxide and carbon dioxide react to form calcium carbonate, like this: CaO(s)+CO,(g)→CaCO3(s) At a certain temperature, a chemist finds that a 7.9 L reaction vessel containing a mixture of calcium oxide, carbon dioxide, and calcium carbonate at equilibrium has the following composition: compound amount СаО 43.4 g CO2 19.6 g CaCO3 85.7 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = []
7. Suppose for a synthesis of hydrogen fluoride from hydrogen and fluorine, 3.000 moles of H2 and 6.000 moles of F2 are mixed in a 3.000-L flask. Assume that the equilibrium constant for the synthesis reaction at this temperature is 1.15x102. H2 (g) + F2 (g) ↔ 2HF (g) What is the molar concentration of HF at equilibrium? What is the molar concentration of F2 at equilibrium? At a Kc of 4.15x103, predict the direction of the reaction if the starting concentrations are [H2]=2.30 M, [F2]= 1.25x10-3 M, and [HF]= 4.37 M