Consider the following equilibrium: 2NO, (g) -N,04(g) AG" = - 5.4 kJ Now suppose a reaction vessel is filled with 7.18 atm of dinitrogen tetroxide (N,0.) at 463. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N,O, tend to rise or fall? 4 O fall Is it possible to reverse this tendency by adding NO,? In other words, if you said the pressure of N,04 will tend to rise, can that yes be changed to a tendency to fall by adding NO,? Similarly, if you said the O no N204 will tend to fall, can that be changed to a tendency to pressure of rise by adding NO,? If you said the tendency can be reversed in the second question, calculate | atm the minimum pressure of NO, needed to reverse it. Round your answer to 2 significant digits.

Consider the following equilibrium: 2NO, (g) -N,04(g) AG" = - 5.4 kJ Now suppose a reaction vessel is filled with 7.18 atm of dinitrogen tetroxide (N,0.) at 463. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N,O, tend to rise or fall? 4 O fall Is it possible to reverse this tendency by adding NO,? In other words, if you said the pressure of N,04 will tend to rise, can that yes be changed to a tendency to fall by adding NO,? Similarly, if you said the O no N204 will tend to fall, can that be changed to a tendency to pressure of rise by adding NO,? If you said the tendency can be reversed in the second question, calculate | atm the minimum pressure of NO, needed to reverse it. Round your answer to 2 significant digits.

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 121CP: If wet silver carbonate is dried in a stream of hot air. the air must have a certain concentration...

See similar textbooks

Similar questions

For the system SO3(g)SO2(g)+12 O2(g)at 1000 K, K=0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. What is its partial pressure at equilibrium?
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)
At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627. What is the equilibrium constant at 555C?
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.
Red phosphorus is formed by heating white phosphorus. Calculate the temperature at which the two forms are at equilibrium, given white P: H f =0.00 kJ/mol; S =41.09 J/mol K red P: H f =17.6 kJ/mol; S =22.80 J/mol K
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
Hf for iodine gas is 62.4 kJ/mol, and S° is 260.7 J/mol K. Calculate the equilibrium partial pressures of I2(g), H2(g), and HI(g) for the system 2HI(g)H2(g)+I2(g) at 500°C if the initial partial pressures are all 0.200 atm.
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.
For the reaction C(s)+CO2(g)2CO(g) K=168 at 1273 K. If one starts with 0.3 atm of CO2 and 12.0 g of C at 1273 K, will the equilibrium mixture contain (a) mostly CO2? (b) mostly CO? (c) roughly equal amounts of CO2 and CO? (d) only C?
Consider the following hypothetical reactions and their equilibrium constants at 75C, 3A(g)3B(g)+2C(g)K1=0.31 3D(g)+2B(g)2C(g)K1=2.8 Find the equilibrium constant at 75C for the following reaction A(g)D(g)+53B(g)
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?