For the reaction H2 S(g) + I2 (s) ⇌ S(s) + 2 HI(g) Kp = 1.33×10–5 at 333 K. What will be the total pressure of the gases above an equilibrium mixture if, at equilibrium, PHI = 0.010 × PH2 S?
The answer is 0.134 atm. Please include work and explanation! Thank you :-)
For the reaction H2 S(g) + I2 (s) ⇌ S(s) + 2 HI(g) Kp = 1.33×10–5...
(1). The equilibrium constant, Kp, for the following reaction is 1.80×10-2 at 698K. 2HI(g) =H2(g) + I2(g) If an equilibrium mixture of the three gases in a 15.5 L container at 698K contains HI at a pressure of 0.399 atm and H2 at a pressure of 0.562 atm, the equilibrium partial pressure of I2 is atm. (2). Consider the following reaction: PCl5(g) =PCl3(g) + Cl2(g) If 1.17×10-3 moles of PCl5, 0.217 moles of PCl3, and 0.351 moles of Cl2 are at...
At 6 oC the equilibrium constant for the reaction: 2 HI(g) H2(g) + I2(g) is KP = 2.66e-11. If the initial pressure of HI is 0.00837 atm, what are the equilibrium partial pressures of HI, H2, and I2? We were unable to transcribe this imageAt 6 °C the equilibrium constant for the reaction: 2 HI(g) = H2(g) + 12(g) is Kp = 2.66e-11. If the initial pressure of HI is 0.00837 atm, what are the equilibrium partial pressures of HI,...
At 49 oC the equilibrium constant for the reaction: 2 HI(g) H2(g) + I2(g) is KP = 4.83e-11. If the initial pressure of HI is 0.00862 atm, what are the equilibrium partial pressures of HI, H2, and I2? p(HI) = p(H2) = . p(I2) = .
Consider this reaction at 298 K: H2 (g) + I2 (g) ⇌ 2 HI(g) Calculate ΔGrxn under the following conditions: PH2 (g) = 0.161 atm PI2 (g) = 0.186 atm PHI(g) = 0.307 atm
Given the reaction at a certain temperature: H2(g) + I2(g) ↔ 2 HI(g). At equilibrium, the partial pressure of HI is 3.8×10–3 atm and the partial pressures of H2 and I2 are 0.20 atm each. The Kp of this reaction is [X]. (Fill in the blank; report with correct number of significant figures.
. Consider the reaction: H2(g) + I2(g) ? 2HI(g) A reaction mixture at equilibrium at 175 K contains PH2 = 0.958 , PI2 = 0.877 , and PHI= 0.020 . A second mixture not equilibrium, but at the same temperature,contains PH2 = PI2 = 0.621 , and PHI = 0.101 . a) For the second mixture, calculate Q. b) Determine whether the reaction in the second mixture will shift right or shift left.c) Construct an ICE table. Keep in mind your...
1. At a given temperature the Kp = 4.76x10-4 for the reaction: H2(g) + 12(g) = 2 HI(g) Calculate the equilibrium partial pressure of Hl if the original reaction mixture contains H2 gas at 0.752 atm, 12 gas at 0.752 atm and Hl gas at 0.134 atm. a) 0.321 atm b) 0.810 atm c) 0.0177 atm d) 0.015 atm e) 0.192 atm
When HI(g) is heated to 700 K, it reversibly decomposes to H2(g) and I2(g). The reaction is- 2 HI(g) ⇌ H2(g) + I2(g). A 15.00-L vessel at 700 K initially contains HI(g) at a pressure of 4.00 atm. When equilibrium is reached, it is found that the partial pressure of H2(g) is 0.387 atm. What is the partial pressure of HI(g) at equilibrium? A) 4.00 atm B) 3.61 atm C) 3.23 atm D) 4.39 atm E) 0.387 atm
The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) 2HI(g) Calculate the equilibrium partial pressures of all species when H2 and I2, each at an intitial partial pressure of 1.65 atm, are introduced into an evacuated vessel at 698 K.
The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K. A mixture of H2, I2 and HI, each at 0.020 M, was introduced into a container at 700 K. Which of the following is true? At equilibrium, [H2] = [I2] = [HI]. No net change occurs because the system is at equilibrium. The reaction proceeds to the left producing more H2(g) and I2(g). The reaction proceeds to the right producing more HI(g). At equilibrium,...