At 1000 K, Kp=2.1×106 and ΔH∘ = -101.7 kJ for the reaction H2(g)+Br2(g)⇌2HBr(g). A 0.950 mol quantity of Br2 is added to a 1.00 L reaction vessel that contains 1.24 mol of H2 gas at 1000 K. What are the partial pressures of H2, Br2, and HBr at equilibrium?
At 1000 K, Kp=2.1×106 and ΔH∘ = -101.7 kJ for the reaction H2(g)+Br2(g)⇌2HBr(g). A 0.950 mol...
For the reaction H2(g) + Br2(g) → 2HBr(g) Kp = 3.6 x 104 at 1494 K. What is the value of Kp for the following reaction at 1494 K? 42 H2(g) + / Br2(g) HBr(g) K". p Submit
The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180 × 106 at 730°C. Starting with 1.20 moles of HBr in a 21.3−L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium.
The equilibrium constant K. for the reaction H2(g) + Brz(g) = 2HBr(g) is 2.18 x 106 at 730°C. Starting with 3.20 moles of HBr in a 12.0-L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium. (10 points) (Reference: Chang 14.43
A sealed 1.5-L container initially holds 0.00623 mol H2, 0.00414 mol Br2, and 0.0244 mol of HBr at 550 K. when equilibrium is established, [H2]= 0.00467M H2(g)+Br2(g) <-> 2HBr(g) A. what are [HBr}eq and [Br2}eq? B. what are Kc and Kp at 550 K? C.A 0.00209 mol sample of Br2 is added to the equilibrium mixture of gases. What are the partial pressures of all species once equilibrium is reestablished?
10. The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180 × 106 at 730°C. Starting with 2.20 moles of HBr in a 13.7−L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium. [H2] = [Br2] = [HBr] =
For the following reaction, Kp = 2.8 ✕ 104 at 1630 K. H2(g) + Br2(g) equilibrium reaction arrow 2 HBr(g) What is the value of Kp for the following reactions at 1630 K? (a) HBr(g) equilibrium reaction arrow 1/2 H2(g) + 1/2 Br2(g) (b) 2HBr(g) equilibrium reaction arrow H2(g) + Br2(g) (c) 1/2H2(g) + 1/2 Br2(g) equilibrium reaction arrow HBr(g)
6. Given the following data: Brig) 2 Brig) ΔΗ'-192.5 kJ/mol H2(g) + Br2(g)-) 2HBr(g) ΔΜ"--72.4 k/mol Calculate ΔΗ' for the reaction below H(g) + Br(g) - HBr(g)
For the reaction H2(g) + Br2(g) ↔ 2HBr(g) Kp = 3.5 x 104 at 1495 K. What is the value of Kp for the following reaction at 1495 K? 4HBr(g) ↔ 2H2(g) + 2Br2(g) please show work
Consider the reaction: CO(g) + H2O(g) -><- CO2(g) + H2(g) Kp = 0.0871 at 1000 K A reaction mixture originally contains a CO partial pressure of 1744 torr and a H2O partial pressure of 766 torr at 1000 K. Caluculate the equilibrium partial pressures of each of the products 6) (10 points) Consider the reaction: CO(g) + H2O(g) = CO2(g) + H2(g) Kp = 0.0871 at 1000 K A reaction mixture initially contains a CO partial pressure of 1 744...
Be sure to answer all parts. The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180 × 106 at 730°C. Starting with 2.20 moles of HBr in a 18.1−L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium. [H2] =___ M Br2] = ___M [HBr] = ____M