The equilibrium constant, K., for the following reaction is 2.25 at 681 K. 2NH3(g)N2(g) + 3H2(g) Calculate K, at this temperature for the following reaction: 1/2N2(g) + 3/2H2(g) NH3(g) Ke

Suppose a 500. mL flask is filled with 1.4 mol of CO, 1.7 mol of H₂O and 0.30 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) + CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 0.935 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. M X

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The equilibrium constant, Ko, for the following reaction is 2.74 at 1150 K. Calculate K, for this reaction at this temperature. 2503(g)=2S02(g) + O2(g) Kc

For the reaction NH3(g) + H2S(g)        NH4HS(s) K = 400. At 35 °C. IF 1.00 mole of each of NH3, H2S, and NH4HS are placed in a 5.00 L vessel, (a) what mass of NH4HS will be present at equilibrium? (b) What is the pressure of H2S at equilibrium?

Suppose a 250. mL flask is filled with 0.60 mol of CHCI,, 0.50 mol of HCl and 1.7 mol of CCI4. The following reaction becomes possible: 3' Cl, (g) + CHCI, (g) – HC1 (g) + CCI4(g) The equilibrium constant K for this reaction is 0.748 at the temperature of the flask. Calculate the equilibrium molarity of CHC1,. Round your answer to two decimal places. M

Steam reforming of methane ( CH4 ) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 1.5L flask with 3.6 atm of methane gas and 5.0 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of carbon monoxide gas to be 2.2 atm .Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits.

Suppose a 500. mL flask is filled with 0.60 mol of Br,, 0.10 mol of OCl, and 1.5 mol of BrOCl. The following reaction becomes possible: Br, (g) +OCl, (g) - - BrOC1(g) +Brci(g) The equilibrium constant K for this reaction is 0.349 at the temperature of the flask. Calculate the equilibrium molarity of BrOCl. Round your answer to two decimal places.

Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures, according to the following reaction. N2(g) + O2(g) = 2 NO(g) The equilibrium constant for the reaction is K = 0.232 at 1230 °C. If a container is charged with 0.301 atm of nitrogen and 0.218 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen? Report your answer to THREE significant figures.

Suppose a 250. mL flask is filled with 0.40 mol of OCl,, 1.6 mol of BrOCl and 1.8 mol of BrCl. The following reaction becomes possible: Br, (g) + OCI, (g) - BROCI (g)+ BrCl (g) The equilibrium constant K for this reaction is 0.756 at the temperature of the flask. Calculate the equilibrium molarity of Br,. Round your answer to two decimal places. OM