Part A A sample of pure NO2 is heated to 334 °C at which temperature it partially dissociates according to the equation 2 NO2 (g) = 2 NO (g) + O2 (9) At equilibrium the density of the gas mixture is 0.520 g/L at 0.750 atm . Calculate K. for the reaction.

Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) PC13(g) + Cl₂(g) K = 1.80 at 250 °C A 0.4044 mol sample of PCI, (g) is injected into an empty 4.40 L reaction vessel held at 250 °C. Calculate the concentrations of PCI, (g) and PCI, (g) at equilibrium.

Consider the following equilibrium: 2NOCl (g) <--> 2NO (g) + Cl2 (g) With K = 1.6 x 10-5. 1.00 mole of pure NOCl and 0.964 mole of pure Cl2 are placed in a 1.00 L container. Calculate the equilibrium concentration of Cl2 (g).

Steam reforming of methane ( CH, ) 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 5.0 L flask with 0.93 atm of methane gas and 2.7 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of carbon monoxide gas to be 0.47 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. K_ = || x10

Suppose a 250. mL flask is filled with 1.2 mol of Br,, 1.4 mol of OCl, and 1.1 mol of BrCl. The following reaction becomes possible: Br, (g) +OCl, (g) - BrOC1 (g) +BrC1(g) The equilibrium constant K for this reaction is 0.483 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places. OM

The equilibrium constant K. for the reaction H2(g) + Br2(g) == 2HB1(g) is 2.18 × 10° 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.

The equilibrium constant, K, for the following reaction is 6.59×10-2 at 546 K. PCl5 (g)  PCl3 (g) +  Cl2 (g) An equilibrium mixture of the three gases in a 6.59 L container at 546 K contains 0.254 M PCl5,   0.129 M PCl3 and 0.129 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 11.7 L?

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Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) PCI, (g) + CL, (g) K. = 1.80 at 250 °C %3! A 0.3251 mol sample of PCI, (g) is injected into an empty 3.60 L reaction vessel held at 250 "C. Calculate the concentrations of PCI, (g) and PCI, (g) at equilibrium.

6. Hydrogen gas is finding more acceptance as an alternative fuel. It is produced along with carbon dioxide by the reaction of carbon monoxide and gaseous water at 915 K. At this temperature, the equilibrium constant (K.) is 1.56. If this reaction is started in a 4.00 L closed system flask with 0.450 mol of CO, 1.25 mol H2O, 1.15 mol CO2, and 3.50 mol H2, calculate the concentrations of all substances in the flask initially and at equilibrium. Put these values in the ICE table below. (Hint: you will need to use the quadratic formula.) CO Н20 CO2 H2 INITIAL CHANGE EQUILIBRIUM 0.1125 0.3125 0.2875 0.875 -X -X +X +x e these values in the table. d. Calculate the reaction quotient, Q. e. Express the direction of equilibrium shift as an algebraic expression. Complete the change row of the table. f. Substitute the algebraic expressions into the equilibrium expression and solve for the equilibrium concentrations. Place these values in the table.