The reaction A(g)⇌2B(g) has an equilibrium constant of K = 0.010. What is the equilibrium constant for the reaction B(g)⇌12A(g)?
Express your answer using two significant figures.
A(g) <----------> 2B(g)
K1 = [B]^2 / [A] = 0.010
B (g) <-----------> 1/2 A (g)
K = [A]^1/2 / [B]
= sqrt (1 / K1)
= sqrt (1/ 0.010)
K = 10
equilibrium constant = 1.0 x10^1
The reaction A(g)⇌2B(g) has an equilibrium constant of K = 0.010. What is the equilibrium constant...
The reaction A(g)⇌2B(g) has an equilibrium constant of K = 0.040. What is the equilibrium constant for the reaction B(g)⇌12A(g)?
QUESTION 6 The reaction 21Br(g) 리2(g) + Br2(g) Has an equilibrium constant K 0.012 If the initial concentration of IBr is 0.026, what is the equilibrium concentration of 12(g)? Enter your answer with 2 significant figures. QUESTION 7 For the reaction Initially the concentration of A was 0.2M. After reaching equilibrium, it was found that the concentration of A had decreased by 0.09. What is the value of the equilibrium constant K for this reaction? Enter your answer with 2...
The reaction Alg) - 2B (g) has an equilibrium constant of k, = 11.6. What is the total pressure in a closed container at equilibrium if the equilibrium partial pressure of A is 11.0 atm? O(A) 22. 9 atm (B) 22.2 atm (C) 23.8 atm (D) 23, 3 atm (E) 24. 2 atm Submit
The reaction below has an equilibrium constant of Kp = 2.26 x 104 at 298 K. CO(g) + 2H2(g) = CH3OH(9) Part A Calculate Kp for the reaction below. CH3OH(g) = CO(g) + 2H2(g) Express your answer to three significant figures. Ky = 4.42-10-5 Submit Previous Answers Completed Part B Calculate K, for the reaction below. CO(g) + H2(g) = = CH3OH(g) Express your answer to three significant figures. ΟΙ ΑΣΦ ? K = Part C Calculate K, for the...
The equilibrium constant for the reaction 2 NO(g) + Br2 = 2 NOBr(9) is Ke = 2.2 x 10" at certain temperature. K = 45 Previous Answers Correct Correct answer is shown. Your answer 45.45 was either rounded differes significant figures than required for this part. Part 6 Calculate K. for NOBr(g) - NO(g) + Bra(g). Express your answer using two significant figures. A = 0 ?
Consider the following reaction: A(g)⇌2B(g) Find the equilibrium partial pressures of A and B for each of the following different values of Kp. Assume that the initial partial pressure of B in each case is 1.0 atm and that the initial partial pressure of A is 0.0 atm. Make any appropriate simplifying assumptions. Part A: Kp= 1.6 Enter your answers numerically separated by a comma. Express your answers using two significant figures. Part B: Kp= 2.0×10−4 Enter your answers numerically...
The change in enthalpy (AH) for a reaction is -35.7 kJ/mol. The equilibrium constant for the reaction is 1.4x109 at 298 K Part A What is the equilibrium constant for the reaction at 618 K? Express your answer using two significant figures. ΑΣφ ? K-
Consider the following reaction: A(g)⇌2B(g) Find the equilibrium partial pressures of A and B for each of the following different values of Kp. Assume that the initial partial pressure of B in each case is 1.0 atm and that the initial partial pressure of A is 0.0 atm. Make any appropriate simplifying assumptions. Part B: Kp= 1.0×10^−4 Enter your answers numerically separated by a comma. Express your answers using two significant figures. I did my math and ended up with...
The change in enthalpy (ΔrH) for a reaction is -23 kJmol−1 . The equilibrium constant for the reaction is 3.1×103 at 298 K. Part A What is the equilibrium constant for the reaction at 603 K ? Express your answer using two significant figures.
The change in enthalpy (?Horxn) for a reaction is -29.6 kJ/mol . The equilibrium constant for the reaction is 4.3×103 at 298 K. Part A What is the equilibrium constant for the reaction at 686 K ? Express your answer using two significant figures.