Determine the value of K for the following reaction if the equilibrium concentrations are as follows:...
Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 3.5 M, [H2]eq = 4.1 M, [NH3]eq = 0.47 M. N2(g) + 3 H2(g) ⇌ 2 NH3(g) A. A) 9.157 x10-4 B. B) 1.76 x10-4 C. C) 4.76 x10-8 D. D) -6.76 x10-3 E. E) none of these
please help with these two questions QUESTION 2 Consider the following reaction and its equilibrium constant: SO2(g) + NO 2(0) SO 3(g) + NO(g) K c = 0.33 A reaction mixture contains 0.41 M SO 2, 0.13 M NO 2.0.11 M SO 3 and 0.13 M NO. Which of the following statements is TRUE concerning this system? The reaction quotient will decrease The reaction will shift in the direction of reactants. The reaction will shift in the direction of products,...
5) Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [NO2]eq = 0.85 M and [NO]eq=0.38 M. 2 NO2(g) - N2048) A) 2.2 B) 1.9 C) 0.022 D) 0.22 E) 0.53 6) Which of the following statements is true? A) If Q=K, it means the reaction is not at equilibrium. B) If Q<K, it means the forward reaction will proceed to the right) to form more reactants. C) IFO <K, it means the...
1. Write the equilibrium constant expression for the following reaction: H3PO4(aq) + 3 H2O(l) ↔ PO4 3- (aq) + 3 H3O+ (aq) 2. (LeChatlier’s principle) The following reaction has Kc = 4.2 x 102 at 325oC, all gases. PBr3 + Cl2 ↔ PCl3 + Br2 ΔHo = -47 kJ/mol a. For this reaction at equilibrium, [PBr3] = [Cl2] = 0.0273 M, and [PCl3] = [Br2] = 0.560 M. What do you expect to happen to the equilibrium concentrations of each...
15.Calculate K for the following reaction given the following equilibrium concentrations of Ha CO, and H2O: (7p) PCIs(g)_ PCI3(g) + Cl2(g) K-? Equilibrium Concentrations (M): .200 040 080 15.Calculate K for the following reaction given the following equilibrium concentrations of Ha CO, and H2O: (7p) PCIs(g)_ PCI3(g) + Cl2(g) K-? Equilibrium Concentrations (M): .200 040 080
EX2 · Question 10 Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [HCl]eq = 0.13 M; [HI]eq = 5.6 x 10-16M; [Cl2]eq = 0.0019 M. 2 HCl(g) + I2(s) ⇌ 2 HI(g) + Cl2(g) · Question 11 Consider the following reaction at equilibrium. What effect will be on the equilibrium when the pressure of the system rises from 4 atm to 12 atm? N2(g) + 3H2(g)) ⇌ 2NH3(g) · Question 12 What is the overall order of...
not sure if its C or D...??? Determine the value of K for the following reaction if the equilibrium concentrations are as follows: (HCl)eg = 0.13 M, [HI]eg = 5.6' 10-16 M, (Cl2leg = 0.0019 M. 2HI(g) + C12(8) = 2HCl(g) + 12(s) O 1.4' 10-19 8.210-18 2.8 1031 3.5'10-32
What is the equilibrium constant (K) for the following reaction given the equilibrium concentrations of each substance are [HI 0.85 M, [H]-0.27 M, and [L]-0.60 M 22. 2 HI (g) H, (g) I, (g) a. 5.25 b. 0.22c.4.5 d. 0.19 23. Given: 2 SO, (g) +O2(g) 2503 (g) and Ke-4.3 x 102 and that the following concentrations are present: So, 0.10 M Is the mixture at equilibrium, yes or no? If not at equilibrium, in which direction - [OJ-0.10 M...
At equilibrium 12(g) + Br2(g) + 2 IBr(g), K = 1.2 x 102 The following concentrations were determined at a particular time: 12(g) = 0.310 mol/L, Br2(g) = 0.310 mol/L and IBr(g) = 2.00 mol/L Calculate Q, the reaction quotient, and by comparing to the K value state if the system is at equilibrium or which direction it will shift if it is not at equilibrium. [3]
For the reaction N2(g) + 3H2(g) = 2NH3(g) what is the value of Ke at 500°C if the equilibrium concentrations are as follows: [H2] = 0.40 M, (N2) = 0.40 M, and (NH3) = 1.9 M Express the equilibrium constant to two significant figures. V AE OE ? Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining Set up the equilibrium-constant expression for this reaction using the equilibrium concentrations. The product concentrations a the reactant concentrations are...