Consider the following reaction at 298 K:N2 O4(g) ⇌ 2NO2(g)              KP = 0.142What is the standard free energy change at this temperature? Describe what happens to the initial system, where the reactants and products are in standard states, as it approaches 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

In a particular experiment 1.0 mole of H2O (g) and 1.0 mole of CO (g) are put into a flask and heated to 350 oC.  In another experiment 1.0 mol of H2 (g) and 1.0 mole of CO2 (g) are put into a different flask with the same volume as the first.  This mixture is also heated to 350 oC.  After equilibrium is reached, will there be any difference in the composition of the mixture in the two flasks?

Consider the reactions and their respective equilbrium constants: NO(g) + 1/2BR(g) > NOBR(g)   KP = 5.3 2NO(g) > N2(g) + O2(g)             KP = 2.1 x 1030 Use these reactions and their equilbrium constants to predict the equlibrium constant for the following reaction: N2(g) + O2(g) + Br2(g) > 2NOBR(g)

At 487 K, this reaction has a Ke value of 0.0463. 2 X(g) + 3 Y(g) = 2Z(g) Calculate Kp at 487 K. Note that the pressure is in units of atmosphere (atm). Kp =

For the following reaction: NH4Cl(s) ↔ NH3(g) + HCl(g) ΔH = +42.1 kilocalories Suppose the substances in the reaction above are at equilibrium at 600K in volume V and at pressure P. State whether the partial pressure of NH3(g) will have increased, decreased, or remained the same when equilibrium is reestablished after each of the following disturbances of the original system. Some solid NH4Cl remains in the flask at all times. Justify each answer with a one-or-two sentence explanation. (e) A quantity of gaseous NH3 is added. The answer for e states that the partial pressure of NH3 is increase, which is a bit confusing. The explanation is that some of the the added NH3 reacts with HCl to relieve stress but only part of NH3 reacts. Can you explain how and where this is implied in the reaction or question. Would appreciate a lot of clarification

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

Consider the following equilibrium: 2NH3(g) → N₂(g) + 3H₂(g) AG = 34. kJ Now suppose a reaction vessel is filled with 6.39 atm of ammonia (NH3) and 0.200 atm of hydrogen (H₂) at 206. °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. OO U rise fall yes no atm x10 X Ś

Consider the following equilibrium: N₂ (g) + 3H₂(g) → 2NH3(g) AG = -34. KJ Now suppose a reaction vessel is filled with 3.40 atm of nitrogen (N₂) and 4.50 atm of ammonia (NH3) at 250. °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 H₂? 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 H₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H₂ needed to reverse it. Round your answer to 2 significant digits. OO rise fall yes no atm ☐x10 X Ś