For the reaction A(g) + 2B(g) ↔ C(g) ; Kc = 10 Which direction will it proceed if [A] = 0.100, [B]= 0.100 , and [C] = 0.100 is found before equilibrium is established?
A. Left
B. Right
C. No change
Why?
For the reaction A(g) + 2B(g) ↔ C(g) ; Kc = 10 Which direction will it...
A particular reaction is represented as A(g) ↔ 2B(g) + C(g). Initially, the concentration of A was 1.5 M. The reaction was allowed to reach equilibrium and the concentration of product C was found to be 0.45 M. What is the value of the equilibrium constant?
Consider the equilibrium constant Kc for the reaction: N2O4(g) ↔ 2NO2(g) is 0.211 at 100°C. What is the value for the equilibrium constant is the reaction is balanced as ½ N2O4(g) ↔ NO2(g) ? A. 0.106 B. 0.459 C. 0.211 D. 0.422
1)For the reaction AsCl5 --> AsCl3 + Cl2, Kc = 33.7. Which of the following statements describes what will happen when 0.00650 M AsCl5, 1.04 M AsCl3 and 0.0005 M Cl2 are mixed together in a 1.0-L flask? the reaction will proceed to the right the reaction will proceed to the left the reaction will be at equilibrium 2)For the reaction A(s) + 2B(g) --> 2C(g) + 3D(g) + E(g), ∆H = +685 J. If the reaction is at equilibrium,...
Consider the equilibrium constant Kc for the reaction: N2O4(g) ↔ 2NO2(g) is 0.211 at 100°C. What is the value for the equilibrium constant if the reaction is reversed: 2NO2(g) ↔ N2O4(g) ? A. -0.211 B. 0.211 C. 4.74 D. -4.74
Consider the reaction A(g) + 2B(g) ⇌ C(g) at 25 °C. The initial pressures of all the gases are 0.100 atm. Once equilibrium has been established, it is found that Pc = 0.140 atm. What is Kp for this reaction at 25 °C. Please explain and/or show the steps.
5.(3 pt) Kc for the following reaction is 0.212 at 1000C.N2O4(g)→2 NO^2(g)A student running this reaction in the lab measures the concentrations as[N2O4] = 0.33 M and [NO2] = 0.66M. They conclude that the reaction must have reached equilibrium because there is a 2:1 ratio of products to reactants, just like in the balanced chemical equation. Decide if the student is right or wrong and explain your reasoning. If the student is right, prove they are right by verifying their...
Consider the following reaction at 350oC: N2(g) + 3 H2(g) ⇌ 2 NH3(g); Kc=70. If the concentrations in the reaction mixture at some moment of time are: [NH3] = 0.0100 M, [H2] = 0.0415 M and [N2] = 0.0200M , then Group of answer choices the system is at equilibrium and no net change will occur the system is not at equilibrium and the reaction will proceed to the left the system is at equilibrium and the reaction will proceed to...
Question 1 In the reaction: CO2(g) + C(s) --> 2CO(g), how might the concentration of C(s) (graphite) affect the equilibrium concentration of the product CO(g)? a. It does not affect it at all because C(s) is not included in the expression of the equilibrium constant. Thus, whether C(s) is present or not does not affect the reaction. b. It doesn't affect it as long as there is C(s) present during the reaction (i.e. C(s) is in excess so it does...
9. By increasing the pressure on increasing the pressure on the equilibrium system for the reaction 2H S (g) → 2H2(g) + S2(g) The equilibrium position is shifted towards a direction : A) right and the value of K decreases B) right and the value of K is established C) left and increase the value of K D) left and the value of K is established. 10. When adding 0.22 mol of ozone to this reaction: NO(g) +O3(g) NO2(g) +...
QUESTION 2 CO(g) + Cl2(g) = COCI_(a) Kc - 1.2 x 10 at 400 °C Consider the above reaction. If the (CO) = [C12] = [COC12] = 5 x 10-6 M at some point during the reaction, is the reaction at equilibrium? If not, in which direction will the reaction proceed in order to reach equilibrium? Use the Math Editor to show your work or complete on paper and upload in the next quesiton. 1. Calculate 2. Is Q> or...