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Consider the (unbalanced) endothermic system: q(heat) + P4s + NO + P.0619) + N2g) with equilibrium concentrations o...
5. Consider the (unbalanced) endothermic system: q(heat) + P41s) + NO + P,0615) + N2(e) with...
5. Consider the (unbalanced) endothermic system: q(heat) + P41s) + NO + P,0615) + N2(e) with equilibrium concentrations of 0.350 M for both nitrogen monoxide and nitrogen at a certain temperature. a. Determine the equilibrium constant K. b. At this temperature, the system is said to favor reactants/products/neither (circle one).
Use K and initial concentrations to calculate equilibrium concentrations. Consider the equilibrium system involving the decomposition...
Use K and initial concentrations to calculate equilibrium concentrations. Consider the equilibrium system involving the decomposition of nitrogen monoxide. 2NO(g) N2(g) + O2(g) [N2] [02] K=— = 3.62x10-2 at 286 K [NO] A flask originally contains 0.239 M nitrogen monoxide. Calculate the equilibrium concentrations of the three gases. [NO] = [N2] = [02] =
if a reaction quotient (Q) is larger than the equilibrium constant, ___. a. the reaction concentrations...
if a reaction quotient (Q) is larger than the equilibrium constant, ___. a. the reaction concentrations will shift in favor of reactants b. the reaction concentrations will shift in favor of products c. the initial reaction concentrations will stay the same
Q(22) Kp=Kc when? A) The reaction is at equilibrium B) The reaction is exothermic C) The reaction is endothermic D)...
Q(22) Kp=Kc when? A) The reaction is at equilibrium B) The reaction is exothermic C) The reaction is endothermic D) all of the gasses present are at the same temperature E) the number of moles of gas on both sides of the balanced equation is the same. Q(23) HAH +A at the equilibrium (HA) = 1.65* 10-2 M and [H") = (A-) = 5.44*10-4 M at equilibrium. Kc = A) 1.7 X 10-1 C) 1.7 X 103 D) 1.7 X...
8. Consider the reduction of carbon dioxide by hydrogen to water vapor and carbon monoxide at...
8. Consider the reduction of carbon dioxide by hydrogen to water vapor and carbon monoxide at 420°C. The equilibrium constant for this reaction is 0.10 (K = 0.10 @ 420°C). Assume that you place enough H2 and CO2 in a flask so that their initial concentrations are both 0.050 mol/L. You heat the mixture to 420° C and wait for equilibrium to be achieved. What are the concentrations of reactants and products at equilibrium?
1) At 298 K, an equilibrium mixture contains P H2=0.958 atm, P I2= 0.877 atm and...
1) At 298 K, an equilibrium
mixture contains P H2=0.958 atm, P I2= 0.877 atm and P HI=0.020
atm. Please try and answer all!
You must show all your work to receive credit. Watch sig figs! Consider the reaction: 1) At 298 K, an equilibrium mixture contains P H2-0.958 atm, P ½=0.877 atm, and P HI-0.020 atm. Calculate the value of the equilibrium constant Kp? a) (o, o2) 0.938x o.87? b) And what is the value of the equilibrium constant...
At a given temperature, the equilibrium constant for a certain reaction is 1 X 1014. Does...
At a given temperature, the equilibrium constant for a certain reaction is 1 X 1014. Does this equilibrium favor products or reactants? Why? Select the single best answer. A very high value for the equilbrium constant favors product formation. O O Significant concentrations of both products and reactants are present at equilibrium. A very high value for the equilbrium constant favors reactant formation. A very low value for the equilibrium constant favors reactant formation. A very low value for the...
For a chemical system that is in dynamic equilibrium with Kc = 0.50, which of the...
For a chemical system that is in dynamic equilibrium with Kc = 0.50, which of the following statements is FALSE? The rate of conversion of reactants to products is the same as the rate of conversion of products to reactants From the perspective of the forward reaction, the reaction mixture at equilibrium lies in favor of the products Both reactants and products are present in the reaction mixture The composition of the reaction mixture does not change with time The...
3 attempts left Check my work At a given temperature, the equilibrium constant for a certain reaction is 1 x 1026....
3 attempts left Check my work At a given temperature, the equilibrium constant for a certain reaction is 1 x 1026. Does this equilibrium favor products or reactants? Why? Select the single best answer. A large value for the equilibrium constant favors reactant formation. A small value for the equilbrium constant favors product formation. Significant concentrations of both products and reactants are present at equilibrium. A large value for the equilibrium constant favors product formation. A small value for the...
8. According to Le Chatelier, adding heat to an endothermic equilibrium reaction will cause: (A) No...
8. According to Le Chatelier, adding heat to an endothermic equilibrium reaction will cause: (A) No change (B) Products to form (C) Reactants to form 9. At a given temperature, Kc = 3.0 for the hypothetical reaction, A(g) +B(g) = C(g) If [A] = 2.0 M, [B] = 1.5 M, and [C]=9.0 M, is the reaction at equilibrium? If not, which way will it go? (A) No, to the left (B) No, to the right (C) It is at equilibrium...
5. Consider the (unbalanced) endothermic system: q(heat) + P41s) + NO + P,0615) + N2(e) with equilibrium concentrations of 0.350 M for both nitrogen monoxide and nitrogen at a certain temperature. a. Determine the equilibrium constant K. b. At this temperature, the system is said to favor reactants/products/neither (circle one).
Use K and initial concentrations to calculate equilibrium concentrations. Consider the equilibrium system involving the decomposition of nitrogen monoxide. 2NO(g) N2(g) + O2(g) [N2] [02] K=— = 3.62x10-2 at 286 K [NO] A flask originally contains 0.239 M nitrogen monoxide. Calculate the equilibrium concentrations of the three gases. [NO] = [N2] = [02] =
Q(22) Kp=Kc when? A) The reaction is at equilibrium B) The reaction is exothermic C) The reaction is endothermic D) all of the gasses present are at the same temperature E) the number of moles of gas on both sides of the balanced equation is the same. Q(23) HAH +A at the equilibrium (HA) = 1.65* 10-2 M and [H") = (A-) = 5.44*10-4 M at equilibrium. Kc = A) 1.7 X 10-1 C) 1.7 X 103 D) 1.7 X...
8. Consider the reduction of carbon dioxide by hydrogen to water vapor and carbon monoxide at 420°C. The equilibrium constant for this reaction is 0.10 (K = 0.10 @ 420°C). Assume that you place enough H2 and CO2 in a flask so that their initial concentrations are both 0.050 mol/L. You heat the mixture to 420° C and wait for equilibrium to be achieved. What are the concentrations of reactants and products at equilibrium?
1) At 298 K, an equilibrium
mixture contains P H2=0.958 atm, P I2= 0.877 atm and P HI=0.020
atm. Please try and answer all!
You must show all your work to receive credit. Watch sig figs! Consider the reaction: 1) At 298 K, an equilibrium mixture contains P H2-0.958 atm, P ½=0.877 atm, and P HI-0.020 atm. Calculate the value of the equilibrium constant Kp? a) (o, o2) 0.938x o.87? b) And what is the value of the equilibrium constant...
At a given temperature, the equilibrium constant for a certain reaction is 1 X 1014. Does this equilibrium favor products or reactants? Why? Select the single best answer. A very high value for the equilbrium constant favors product formation. O O Significant concentrations of both products and reactants are present at equilibrium. A very high value for the equilbrium constant favors reactant formation. A very low value for the equilibrium constant favors reactant formation. A very low value for the...
For a chemical system that is in dynamic equilibrium with Kc = 0.50, which of the following statements is FALSE? The rate of conversion of reactants to products is the same as the rate of conversion of products to reactants From the perspective of the forward reaction, the reaction mixture at equilibrium lies in favor of the products Both reactants and products are present in the reaction mixture The composition of the reaction mixture does not change with time The...
3 attempts left Check my work At a given temperature, the equilibrium constant for a certain reaction is 1 x 1026. Does this equilibrium favor products or reactants? Why? Select the single best answer. A large value for the equilibrium constant favors reactant formation. A small value for the equilbrium constant favors product formation. Significant concentrations of both products and reactants are present at equilibrium. A large value for the equilibrium constant favors product formation. A small value for the...
8. According to Le Chatelier, adding heat to an endothermic equilibrium reaction will cause: (A) No change (B) Products to form (C) Reactants to form 9. At a given temperature, Kc = 3.0 for the hypothetical reaction, A(g) +B(g) = C(g) If [A] = 2.0 M, [B] = 1.5 M, and [C]=9.0 M, is the reaction at equilibrium? If not, which way will it go? (A) No, to the left (B) No, to the right (C) It is at equilibrium...
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