At - 14.6 °C the pressure equilibrium constant Kp =9.1 for a certain reaction. Here are some facts about the reaction: • If the reaction is run at constant pressure, 100. kJ/mol of heat are absorbed. • The net change in moles of gases is - 1. • If the reaction is run at constant pressure, the volume increases by 13.%. Using these facts, can you calculate Ko at -3.7 °C? If you said yes, then enter your answer at right. Round it to 2 significant digits. P If you said no, can you at least decide whether K at -3.7 °C will be bigger or smaller than K₂ at -14.6 °C? O Yes. O No. 0 Yes, and K will be bigger. Yes, and K will be smaller. No. 10 X

At - 14.6 °C the pressure equilibrium constant Kp =9.1 for a certain reaction. Here are some facts about the reaction: • If the reaction is run at constant pressure, 100. kJ/mol of heat are absorbed. • The net change in moles of gases is - 1. • If the reaction is run at constant pressure, the volume increases by 13.%. Using these facts, can you calculate Ko at -3.7 °C? If you said yes, then enter your answer at right. Round it to 2 significant digits. P If you said no, can you at least decide whether K at -3.7 °C will be bigger or smaller than K₂ at -14.6 °C? O Yes. O No. 0 Yes, and K will be bigger. Yes, and K will be smaller. No. 10 X

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 89AP

See similar textbooks

Similar questions

Hydrogen gas and iodine gas react to form hydrogen iodide. If 0.500 mol H2 and 1.00 mol I2 are placed in a closed 10.0-L vessel, what is the mole fraction of HI in the mixture when equilibrium is reached at 205C? Use data from Appendix C and any reasonable approximations to obtain K.
12.108 A nuclear engineer is considering the effect of discharging waste heat from a power plant into a lake and estimates that this may warm the water locally to 25 °C. One question to be considered is the effect of this temperature change on the uptake of CO2 by the water. The equilibrium constant for the reaction CO2+H2OH2CO3 ; is K=1.7103 at 25 °C. Because bonds form, the reaction is exothermic. (a) Will this reaction progress further toward products at higher temperatures near the water discharge with its warmer water than it would in the cooler lake water? Explain your reasoning. (b) Carbonic acid has a Kaof 2.5104 at 25 °C. What is the equilibrium constant for the CO2+2H2OHCO3+H3O+? (c) What additional factor should the engineer be considering about CO2 gas, probably before considering this reaction chemistry?
Consider the reaction CO(g)+H2O(g)CO2(g)+H2(g) Use the appropriate tables to calculate (a) G at 552C (b) K at 552C
Calculate K for the formation of methyl alcohol at 100C: CO(g)+2H2(g)CH3OH(g) given that at equilibrium, the partial pressures of the gases are PCO=0.814 atm, PH2=0.274 atm, and PCH3OH=0.0512 atm.
Given the following data at a certain temperature, 2N2(g)+O2(g)2N2O(g)K=1.2 10 35 N2O4(g)2NO2(g)K=4.6 10 3 12 N2(g)+O2(g)NO2(g)K=4.1 10 9 calculate K for the reaction between one mole of dinitrogen oxide gas and oxygen gas to give dinitrogen tetroxide gas.
Indicate whether each statement below is true or false. If a statement is false, rewrite it to produce a closely related statement that is true. For a given reaction, the magnitude of the equilibrium constant is independent of temperature. If there is an increase in entropy and a decrease in enthalpy when reactants in their standard states are converted to products in their standard states, the equilibrium constant for the reaction must be negative. The equilibrium constant for the reverse of a reaction is the reciprocal of the equilibrium constant for the reaction itself. For the reaction H2O2(ℓ) ⇌ H2O(ℓ) + O2(g) the equilibrium constant is one half the magnitude of the equilibrium constant for the reaction 2H2O2(ℓ) ⇌ 2H2O(ℓ) + O2(g)
When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above 200. °C in a closed container, the hydrogen and bromine react to form hydrogen bromide and a gas-phase equilibrium is established. Write a balanced chemical equation for the equilibrium reaction. Use bond enthalpies from Table 6.2 ( Sec. 6-6b) to estimate the enthalpy change for the reaction. Based on your answers to parts (a) and (b), which is more important in determining the position of this equilibrium, the entropy effect or the energy effect? In which direction will the equilibrium shift as the temperature increases above 200. °C? Explain. Suppose that the pressure were increased to triple its initial value. In which direction would the equilibrium shift? Why is the equilibrium not established at room temperature?
Hypothetical elements A(g) and B(g) are introduced into a container and allowed to react according to the reaction A(g)+2B(g)AB2(g). The container depicts the reaction mixture after equilibrium has been attained. a Is the value of S for the reaction positive, negative, or zero? b Is the value of H for the reaction positive, negative, or zero? c Prior to equilibrium, is the value of G for the reaction positive, negative, or zero? d At equilibrium, is the value of G for the reaction positive, negative, or zero?
1. A process is spontaneous in the direction that moves it away from equilibrium toward equilibrium
Consider the following reaction at 298 K: 2SO2(g)+O2(g)2SO3(g) An equilibrium mixture contains O2(g) and SO3(g) at partial pressures of 0.50 atm and 2.0 atm, respectively. Using data from Appendix 4, determine the equilibrium partial pressure of SO2 in the mixture. Will this reaction be most favored at a high or a low temperature, assuming standard conditions?
Sodium acetate crystallizes from a supersaturated solution (see Figure 12.4). What can you say about the sign of G? WTiat would you expect for the sign of S? What about the sign of H? Is the crystallization exothermic or endothermic? Explain your answers
At 627C, K=0.76 for the reaction 2SO2(g)+O2(g)2SO3(g) Calculate K at 627C for (a) the synthesis of one mole of sulfur trioxide gas. (b) the decomposition of two moles of SO3.