Using data from Appendix C of your textbook calculate the temperature, To, at which this reaction will be at equilibrium under standard conditions (AG 0) and choose whether A>Gº will increase, decrease, or not change with increasing temperature from the pulldown menu. K. and AG will -Select- with increasing temperature. For each of the temperatures listed below calculate AG for the reaction above, and select from the pulldown menu whether the reaction under standard conditions will be spontaneous, nonspontaneous, or near equilibrium ('near equilibrium" means that T is within 5 K of T₂). (a) At T-10959 K AG - (b) At T 3653 K AG - (c) At T-7306 K AG k3/mol, and the reaction is Select- kJ/mol, and the reaction is-Select- kJ/mol, and the reaction is-Select- under standard conditions. under standard conditions. under standard conditions

Using data from Appendix C of your textbook calculate the temperature, To, at which this reaction will be at equilibrium under standard conditions (AG 0) and choose whether A>Gº will increase, decrease, or not change with increasing temperature from the pulldown menu. K. and AG will -Select- with increasing temperature. For each of the temperatures listed below calculate AG for the reaction above, and select from the pulldown menu whether the reaction under standard conditions will be spontaneous, nonspontaneous, or near equilibrium ('near equilibrium" means that T is within 5 K of T₂). (a) At T-10959 K AG - (b) At T 3653 K AG - (c) At T-7306 K AG k3/mol, and the reaction is Select- kJ/mol, and the reaction is-Select- kJ/mol, and the reaction is-Select- under standard conditions. under standard conditions. under standard conditions

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 6QRT: Indicate whether each statement below is true or false. If a statement is false, rewrite it to...

See similar textbooks

Similar questions

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
For each reaction, an equilibrium constant at 298 K is given. Calculate G for each reaction. (a) Br2()+ H2(g)2HBr(g) KP = 4.4 1018 (b) H2O()H2O(g) KP = 3.17 102 (c) N2(g) +3H2(g)2NH3(g) Kc = 3.5 108
5.22. True or false: If for a gas-phase reaction, then all equilibrium partial pressures of reactants and products must equal . Explain your choice.
1. A process is spontaneous in the direction that moves it away from equilibrium toward equilibrium
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
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?
The equilibrium constant for a reaction decreases as temperature increases. Explain how this observation is used to determine the sign of either H or S.
Kp for the following reaction is 0.16 at 25 C: 2 NOBr(g) 2 NO(g) + Br2(g) The enthalpy change for the reaction at standard conditions is + 16.3 kJ/mol-rxn. 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 Br2(g) (b) removing some NOBr(g) (c) decreasing the temperature (d) increasing the container volume
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?
Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of A(NO3)2 is made to react with 25.00 mL of 0.195 M NaOH. A precipitate, A(OH)2, forms. Along with the precipitation, the temperature increases from 24.8C to 28.2C. What is H for the precipitation of A(OH)2? The following assumptions can be made. â€¢ The density of the solution is 1.00 g/mL. â€¢ Volumes are additive. â€¢ The specific heat of the solution is 4.18 J/g C.