At -11.5 °C the concentration equilibrium constant K = 9.2 × 10 for a certain reaction. Here are some facts about the reaction: • If the reaction is run at constant pressure, 136. kJ/mol of heat are absorbed. • The initial rate of the reaction is 6.2 mol-L¯¯¹-s¯¯¹. • The net change in moles of gases is -1. Using these facts, can you calculate Kat 1.4 °C? If you said yes, then enter your answer at right. Round it to 2 significant digits. Yes. O No. 0 D

At -11.5 °C the concentration equilibrium constant K = 9.2 × 10 for a certain reaction. Here are some facts about the reaction: • If the reaction is run at constant pressure, 136. kJ/mol of heat are absorbed. • The initial rate of the reaction is 6.2 mol-L¯¯¹-s¯¯¹. • The net change in moles of gases is -1. Using these facts, can you calculate Kat 1.4 °C? If you said yes, then enter your answer at right. Round it to 2 significant digits. Yes. O No. 0 D

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 119AP

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12.100 A reaction important in smog formation is O3(g)+NO(g)O2(g)+NO2(g)K=6.01034 (a) If the initial concentrations are [O3]=1.0106M,[NO]=1.0105M,[NO2]=2.5104M, and [O2]=8.2103M , is the system at equilibrium? If not, in which direction does the reaction proceed? (b) If the temperature is increased, as on a very warm day, will the concentrations of the products increase or decrease? (HINT: You may have to calculate the enthalpy change for the reaction to find out if it is exothermic or endothermic.)
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