4.) Consider the equilibrium: 4NO2(9) + 6H20(g) = 4NH3(g) + 702(9) If the change in the pressure of NO2 is 50 torr as a mixture of the four gases reaches equilibrium, how much will the pressure of NH3 change? Show your work!

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 200. mL flask with 3.6 atm of carbon monoxide gas and 2.5 atm of water vapor. When the mixture has come t equilibrium she determines that it contains 2.0 atm of carbon monoxide gas, 0.90 atm of water vapor and 1.6 atm of carbon dioxide. The engineer then adds another 1.2 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. atm x10

Phosphorus pentachloride decomposes according to the chemical equation: PCIs(g) → PCl3(g) + Cl₂(g) Kc = 1.80 at 250.0 °C A 45.0 gram sample of PCI-(g) is injected into an empty 5.00-liter reaction vessel held at 250.0 °C. Calculate the pressure, in atm, of the vessel when equilibrium is reached.

A2

(#30) The Equilibrium Constant and the "ICE Chart" Phosphorus pentachloride gas is formed according to the reaction by adding chlorine gas to phosphorus trichloride gas. Then the reaction reaches equilibrium. The equilibrium constant, Kc, equals 49.0 at 230°C. If 0.500 mole each of the reactants are added to a 5-L container, what is the equilibrium composition at 230°C? (30a) In blank #1, type-in our answer for the concentration of phosphorus pentachloride in the product at equilibrium. The unit is Molarity, but enter only the value of your answer with two decimal places. (30b) In blank #2, type in your answer for the concentration of phosphorus trichloride at equilibrium with two decimal places. (30c) In blank #3, type in your answer for the concentration of chlorine gas at equilibrium with two decimal places.

Do 6-10.

As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 200. mL flask with 2.3 atm of carbon monoxide gas and 4.0 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 0.90 atm of carbon monoxide gas, 2.6 atm of water vapor and 1.4 atm of carbon dioxide. The engineer then adds another 1.0 atm of water, and allows the mixture to come to equilibrium again. Calculate the pressure of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. 0 atm x10 X

Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 200. mL flask with 4.6 atm of ammonia gas, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 4.8 atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits.

Consider the chemical reaction shown below with an equilibrium constant (K) of 3.0 at some temperature. You add 3.5 MA and 3.5 MB to a reaction vessel heated to this temperature. What will the reaction do to reach equilibrium? 2 A (g) 2 3 B (g) The reaction will form more reactants to reach equilibrium. O The reaction will form more products to reach equilibrium. O The answer depends on the volume of the reaction vessel. O Cannot be determined because the equilibrium constant changes over time. O The reaction is already at equilibrium.