Homework Answers
According to Le Chatelier principle decrease the volume cause to shift the equilibrium to the side with fewer number of gases molecules.
Among given reactions reaction D has fewer number of molecules on right side. So decreasing volume for this system cause the equilibrium to shift to the right.
Answer: D)
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For which of the following systems at equilibrium and at constant temperature will decreasing the volume...
Ammonia will burn in the presence of a platinum catalyst to produce nitric oxide, NO. 4NH_3(g)...
Ammonia will burn in the presence of a platinum catalyst to produce nitric oxide, NO. 4NH_3(g) + 5O_2(g) rightarrow 4NO(g) + 6 H_2 O(g) What is the heat of reaction at constant pressure? Use the following thermochemical equations: N_2(g) + O_2 (g) rightarrow 2NO(g): Delta H = 180.6 kJ N_2(g) + 3H_2 (g) rightarrow 2 NH_3 (g) Delta H = -91.8 kJ 2H_2 (g) + O_2 (g) rightarrow 2H_2O(g): Delta H = -483.7 kJ
All four please thank you Which of the following is necessary for a process to be...
All four please thank you
Which of the following is necessary for a process to be spontaneous? A) Delta H_sys < 0 B) Delta S_sys > 0 C) Delta S < 0 D) Delta S_univ > 0 E) Delta G_sys = 0 Which reaction has the largest Delta S degree? A) 2 N_2H_4(g) rightarrow 2 NH_3(g) + H_2(g) B) O_2(g) + 2 H_2(g) rightarrow 2 H_2O(l) C) O_2(g) + 2 H_2(g) rightarrow 2H_2O(g) D) N_2(g) + 3H_2(g) rightarrow 2NH_3(g) E)...
For which of the following processes would Delta S degree be expected to be most positive?...
For which of the following processes would Delta S degree be expected to be most positive? a) O_2(g) + 2H_2(g) rightarrow 2 H_2O(g) b) H_2O(l) rightarrow H_2O(s) c) NH_3(g) + HCl(g) rightarrow NH_4Cl(g) d) 2NH_4NO_3(s) rightarrow 2 N_2(g) + O_2(g) + 4H_2O(g) e) N_2O_4 rightarrow 2NO_2(g)
Predict the effect of increasing the temperature on the amounts of products in the following reactions:...
Predict the effect of increasing the temperature on the amounts of products in the following reactions: CO(g) + 2H_2(g) rightleftharpoons CH_3OH(g) delta H^0_rxn = -90.7 kJ C(s) + H_2O(g) rightleftharpoons CO(g) + H_2(g) delta H^0_rxn = 131 kJ 2NO_2(g) rightleftharpoons 2NO(g) + O_2(g) (endothermic) 2C(s) + O_2(g) rightleftharpoons 2CO(g) (exothermic)
Write the equilibrium constant expression (K) for the following reaction: N_2(g) + 3H_2(g) doubleheadarrow 2NH_3(g) For...
Write the equilibrium constant expression (K) for the following reaction: N_2(g) + 3H_2(g) doubleheadarrow 2NH_3(g) For the equilibrium in question #3, if the value of K at 25 degree C is 3.7 x 10^8. and the equilibrium concentrations for N_2 and H_2 are 1.05 x 10^-4M and 5.42 x 10^-5M, respectively, use the expression above to calculate the equilibrium concentration of NH.
For the following equilibrium: N_2(g) + H_2(g) rightarrow NH_3(g) delta H= -386 kJ/mole Predict the direction...
For the following equilibrium: N_2(g) + H_2(g) rightarrow NH_3(g) delta H= -386 kJ/mole Predict the direction the equilibrium will shift if: N_2 is added? H_2 is removed? NH_3 is added? NH_3 is removed? the volume of the container is decreased? the pressure is increased by adding Argon gas? the reaction is cooled? equal number of moles of H_2 and NH_3 are added? a catalyst is added The equilibrium constant for the following reaction is 5.0 at 400 degree C. CO_(g)...
At a certain temperature the rate of this reaction is second order in NH_3 with a...
At a certain temperature the rate of this reaction is second order in NH_3 with a rate constant of 0.100 M^-1 middot s^-1 2NH_3 g) rightarrow N_2 (g) + 3H_2 (g) Suppose a vessel contains NH_3 at a concentration of 0.960 M. Calculate how long it takes for the concentration of NH_3 to decrease to 0.134 M. You may assume no other reaction is important. Round your answer to significant digits.
At a given temperature, the equilibrium constant K_c for the reaction 2 NO(g) + 2 H_2(g)...
At a given temperature, the equilibrium constant K_c for the reaction 2 NO(g) + 2 H_2(g) implies N_2(g) + 2 H_2O(g) What is the equilibrium constant for the following reaction? NO(g) + H_2(g) implies 1/2 N_2(g) + H_2 O(g) Correct. Think About It When we multiply a chemical reaction by a number, the new value of the equilibrium constant is the first equilibrium constant raised to the number.
An decrease in temperature increases the reaction rate because temperature affects the equilibrium constant of the...
An decrease in temperature increases the reaction rate because temperature affects the equilibrium constant of the reaction a smaller fraction of the collisions have the correct orientation of molecules. the activation energy of the reaction will decrease. less collisions will have enough energy to exceed the activation energy. the activation energy of the reaction will increase. The equilibrium constant, K_p, for the reaction H_2(g) + I_2(g) doubleheadarrow 2HI(g) is 10.0 at 450 degree C. A rigid cylinder at that temperature...
In each of the following, determine the direction in which the equilibrium will shift in response...
In each of the following, determine the direction in which the equilibrium will shift in response to the indicate stress. (a) N_2(g) + 3 H_2(g)boubleheadarrow 2 NH_3(g): pressure is decreased (b) CO_2(g) + H_2(g)boubleheadarrow CO(g) + H_2O(g): pressure is increased
Ammonia will burn in the presence of a platinum catalyst to produce nitric oxide, NO. 4NH_3(g) + 5O_2(g) rightarrow 4NO(g) + 6 H_2 O(g) What is the heat of reaction at constant pressure? Use the following thermochemical equations: N_2(g) + O_2 (g) rightarrow 2NO(g): Delta H = 180.6 kJ N_2(g) + 3H_2 (g) rightarrow 2 NH_3 (g) Delta H = -91.8 kJ 2H_2 (g) + O_2 (g) rightarrow 2H_2O(g): Delta H = -483.7 kJ
All four please thank you
Which of the following is necessary for a process to be spontaneous? A) Delta H_sys < 0 B) Delta S_sys > 0 C) Delta S < 0 D) Delta S_univ > 0 E) Delta G_sys = 0 Which reaction has the largest Delta S degree? A) 2 N_2H_4(g) rightarrow 2 NH_3(g) + H_2(g) B) O_2(g) + 2 H_2(g) rightarrow 2 H_2O(l) C) O_2(g) + 2 H_2(g) rightarrow 2H_2O(g) D) N_2(g) + 3H_2(g) rightarrow 2NH_3(g) E)...
For which of the following processes would Delta S degree be expected to be most positive? a) O_2(g) + 2H_2(g) rightarrow 2 H_2O(g) b) H_2O(l) rightarrow H_2O(s) c) NH_3(g) + HCl(g) rightarrow NH_4Cl(g) d) 2NH_4NO_3(s) rightarrow 2 N_2(g) + O_2(g) + 4H_2O(g) e) N_2O_4 rightarrow 2NO_2(g)
Predict the effect of increasing the temperature on the amounts of products in the following reactions: CO(g) + 2H_2(g) rightleftharpoons CH_3OH(g) delta H^0_rxn = -90.7 kJ C(s) + H_2O(g) rightleftharpoons CO(g) + H_2(g) delta H^0_rxn = 131 kJ 2NO_2(g) rightleftharpoons 2NO(g) + O_2(g) (endothermic) 2C(s) + O_2(g) rightleftharpoons 2CO(g) (exothermic)
Write the equilibrium constant expression (K) for the following reaction: N_2(g) + 3H_2(g) doubleheadarrow 2NH_3(g) For the equilibrium in question #3, if the value of K at 25 degree C is 3.7 x 10^8. and the equilibrium concentrations for N_2 and H_2 are 1.05 x 10^-4M and 5.42 x 10^-5M, respectively, use the expression above to calculate the equilibrium concentration of NH.
For the following equilibrium: N_2(g) + H_2(g) rightarrow NH_3(g) delta H= -386 kJ/mole Predict the direction the equilibrium will shift if: N_2 is added? H_2 is removed? NH_3 is added? NH_3 is removed? the volume of the container is decreased? the pressure is increased by adding Argon gas? the reaction is cooled? equal number of moles of H_2 and NH_3 are added? a catalyst is added The equilibrium constant for the following reaction is 5.0 at 400 degree C. CO_(g)...
At a certain temperature the rate of this reaction is second order in NH_3 with a rate constant of 0.100 M^-1 middot s^-1 2NH_3 g) rightarrow N_2 (g) + 3H_2 (g) Suppose a vessel contains NH_3 at a concentration of 0.960 M. Calculate how long it takes for the concentration of NH_3 to decrease to 0.134 M. You may assume no other reaction is important. Round your answer to significant digits.
At a given temperature, the equilibrium constant K_c for the reaction 2 NO(g) + 2 H_2(g) implies N_2(g) + 2 H_2O(g) What is the equilibrium constant for the following reaction? NO(g) + H_2(g) implies 1/2 N_2(g) + H_2 O(g) Correct. Think About It When we multiply a chemical reaction by a number, the new value of the equilibrium constant is the first equilibrium constant raised to the number.
An decrease in temperature increases the reaction rate because temperature affects the equilibrium constant of the reaction a smaller fraction of the collisions have the correct orientation of molecules. the activation energy of the reaction will decrease. less collisions will have enough energy to exceed the activation energy. the activation energy of the reaction will increase. The equilibrium constant, K_p, for the reaction H_2(g) + I_2(g) doubleheadarrow 2HI(g) is 10.0 at 450 degree C. A rigid cylinder at that temperature...
In each of the following, determine the direction in which the equilibrium will shift in response to the indicate stress. (a) N_2(g) + 3 H_2(g)boubleheadarrow 2 NH_3(g): pressure is decreased (b) CO_2(g) + H_2(g)boubleheadarrow CO(g) + H_2O(g): pressure is increased
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