19. At elevated temperatures, hydrogen iodide may decompose to form hydrogen gas andiodine gas, as follows:2HI(g) = H2(g) + 12(g)In a particular experiment, the concentrations at equilibrium were measured to be [HI]= 0.85 M, [12] = 0.60 M, and [H2] = 0.27 M. What is K, for this reaction?

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Answered: 19. At elevated temperatures, hydrogen…

Chemistry

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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At room temperature when HI (aq) is added to potassium bisulfite, KHSO3(s), sulfur dioxide is formed and the reaction vessel becomes cold. HI (aq) + KHSO3(s)→ SO2(g) + H2O(l) + K+(aq) + I-(aq). A.)Once the process has reached equilibrium at room temperature, which of the following must be true? choose one....(ΔH<TΔS, ΔH=TΔS, ΔH>TΔS, or need more info). B.) Once the process has reached equilibrium at room temperature, which of the following must be true? choose one....(ΔSuniv<0, ΔSuniv=0, ΔSuniv>0, or need more info).
The equilibrium constant, K, for the following reaction is 1.29x10-2 at 600 K. COC,(g) CO(g) + Cl2(g) + C2(g) Calculate the equilibrium concentrations of reactant and products when 0.262 moles of COCI,(g) are introduced into a 1.00 L vessel at 600 K. [COCI,] = [CO] [Ch] MMM
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 10.1 L container at 698K contains HI at a pressure of 1.21 atm and H2 at a pressure of 0.805 atm, the equilibrium partial pressure of I2 is atm --- Consider the following reaction:2NH3(g) N2(g) + 3H2(g)If 4.60×10-4 moles of NH3, 0.234 moles of N2, and 0.205 moles of H2 are at equilibrium in a 15.6 L container at 814 K, the value of the equilibrium constant, Kp, is .
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19. At elevated temperatures, hydrogen iodide may decompose to form hydrogen gas and iodine gas, as follows: 2HI(g) = H2(g) + 12(g) In a particular experiment, the concentrations at equilibrium were measured to be [HI] = 0.85 M, [12] = 0.60 M, and [H2] = 0.27 M. What is K, for this reaction?