Consider the following equilibrium: 2NOCI (g) 2NO(g) + Cl₂ (g) AG = 41. KJ Now suppose a reaction vessel is filled with 9.62 atm of nitrosyl chloride (NOCI) and 4.77 atm of chlorine (C1₂) at 722. °C. Answer the following questions about this system: Under these conditions, will the pressure of Cl₂ tend to rise or fall? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of Cl₂ will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of C1, will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. Orise O fall O yes O no atm 0 x10

Consider the following reaction that takes place at 1200 °C: H, (g) + CI, (g) + 2HCI (g) Kc = 2.5x10 Hydrogen gas and chlorine gas were added to a reaction vessel at partial temperatures of 2.00 atm and 1.00 atm, respectively. Calculate the total pressure in the flask at equilibrium.

Consider the following equilibrium: 2NOC1 (g) → 2NO(g) + Cl₂ (g) AG = 41. kJ Now suppose a reaction vessel is filled with 8.30 atm of nitrosyl chloride (NOC1) and 5.80 atm of chlorine (C1₂) at 878. °C. Answer the following questions about this system: Under these conditions, will the pressure of Cl₂ tend to rise or fall? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of Cl₂ will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of Cl₂ will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. оо rise fall yes no 0 atm x10 X Ś

Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 1.5 L flask with 1.7 atm of ammonia gas and 2.1 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 0.77 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = ☐ P x10

Consider the following equilibrium: N,0, (g) = 2NO, (3) AG' = 5.4 kJ Now suppose a reaction vessel is filled with 0.496 atm of nitrogen dioxide (NO,) at 137. °C. Answer the following questions about this system: O rise Under these conditions, will the pressure of NO, tend to rise or fall? O fall Is it possible to reverse this tendency by adding N,O,? In other words, if you said the pressure of NO, will tend to rise, can that O yes be changed to a tendency to fall by adding N,04? Similarly, if you said O no the pressure of NO, will tend to fall, can that be changed to a tendency to rise by adding N,0,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N,0, needed to reverse it. O atm Round your answer to 2 significant digits.

Sulfuryl chloride, SO2Cl2, is a highly reactive gaseous compound. When heated, it decomposes into sulfur dioxide and chlorine. A sample of 3.509 grams of SO2Cl2 is placed in an evacuated 1.00 L bulb and the temperature is raised to 102.0 °C. When the system has come to equilibrium at 102.0 °C, the total pressure in the bulb is found to be 1.43 atm. What is the Kp? (Use ICE table)

Consider the following equilibrium: 2NH3(g) = N₂ (g) + 3H₂(g) 2 AG = 34. kJ Now suppose a reaction vessel is filled with 7.87 atm of ammonia (NH3) and 1.17 atm of hydrogen (H₂) at 448. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. rise fall yes no atm x10 X 5

For the reaction 2 A(g) = B(g) + 3 C(g), we begin with only pure A(g) and the total pressure is 8.00 atm. We attain equilibrium. At equilibrium, the total pressure is 12.00 atm. What is the value of ∆G◦ for this reaction? The temperature is 25.0 ◦C throughout.

demonstrate an understanding of the concept of dynamic equilibrium and the variables that cause shifts in the equilibrium of chemical systems.

Consider the following equilibrium: 2NO₂(g) → N₂O4 (g) AG = -5.4 kJ Now suppose a reaction vessel is filled with 0.202 atm of nitrogen dioxide (NO₂) at 504. °C. A Under these conditions, will the pressure of NO₂ tend to rise or fall? Is it possible to reverse this tendency by adding N₂O4? In other words, if you said the pressure of NO₂ will tend to rise, can that be changed to a tendency to fall by adding N₂O4? Similarly, if you said the pressure of NO₂ will tend to fall, can that be changed to a tendency to rise by adding N₂O4? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂O needed to reverse it. V Round your answer to 2 significant digits. Orise fall O yes no atm 0