References Use the References to access important values if needed for this question. A student ran the following reaction in the laboratory at 688 K: 2HI(g) H2(g) + I½(g) When he introduced HI(g) at a pressure of 4.87 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of I2(g) to be 0.510 atm. Calculate the equilibrium constant, K,, he obtained for this reaction. %3D Submit Answer

Please don't provide handwritten solution....

1. Consider the following equilibrium for which AH < 0 2SO2(g) + O2(g) =2SO3(g) How will each of the following changes affect an equilibrium mixture of the three gases. (a) 02 (g) is added to the system. (b) the reaction mixture is heated. (c) the volume of the reaction vessel is doubled (d) a catalyst is added to the mixture. (e) the total pressure of the system is increased by adding a noble gas. (f) SO:(g)is removed from the system?

A chemical engineer is studying the following reaction: 2 NO(g)+2H2(g) → N,(9)+2H2O(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.0038. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction compound pressure expected change in pressure vessel NO 7.58 atm f increase I decrease (no change) H2 8.02 atm f increase I decrease (no change) A N, 4.16 atm f increase I decrease (no change) H,0 2.79 atm f increase I decrease O (no change) NO 8.89 atm ↑ increase I decrease (no change) H2 9.33 atm f increase I decrease (no change) В N2 3.51 atm f increase I decrease (no change) H,0 1.48 atm f increase I decrease (no change) NO…

3. Please provide the correct answer choices for all parts to this chemistry problem. 

A student ran the following reaction in the laboratory at 295 K:2NO(g) + Br2(g) 2NOBr(g)When she introduced NO(g) and Br2(g) into a 1.00 L evacuated container, so that the initial partial pressure of NO was 1.26 atm and the initial partial pressure of Br2 was 0.587 atm, she found that the equilibrium partial pressure of NOBr was 0.701 atm.Calculate the equilibrium constant, Kp, she obtained for this reaction.Kp =

The equilibrium constant, Ke, for the following reaction is 10.5 at 350. K. 2CH₂Cl₂ (9) CH₂(g) + CCL4 (9) Calculate the equilibrium concentrations of reactant and products when 0.359 moles of CH₂Cl₂ (g) are introduced into a 1.00 L vessel at 350. K [CH₂Cl₂]-[ [CH]-[ [CCL]-[ M M M 3

4. For the equilibrium CH₂(g) + 2H₂S(g) = CS₂(g) + 4H₂(g), the concentrations at equilibrium are [CH4] = 0.0804 M, [H₂S] = 0.0608 M, [CS₂] = 0.0196 M, and [H₂] = 0.0784 M at 1400.0 K. Using the equilibrium constant expression from before, calculate Kc.

The equilibrium constant, Kc, for the following reaction is 0.0129 at 600 K. COC12 (g) CO(g) + Cl₂ (g) If an equilibrium mixture of the three gases in a 16.3 L container at 600 K contains 0.497 mol of COC1₂(g) and 0.339 mol of CO, the equilibrium concentration of Cl2 is || M.

The equilibrium constant Kp = (9.180x10^-1) for the following reaction in the gas phase at a given temperature T: H2O(g) + Cl2O(g) = 2 HOCI(g) Calculate the equilibrium pressure (in bar) of HOCI(g) in the reaction vessel at temperature T if the initial pressures of H2O(g) and Cl₂O(g) are both equal to (3.06x10^-1) bar.