Use the data below to calculate the value of the equilibrium constant for the following reaction at 298 K. Please give your answer with 2 significant figures. 3 NO2(g) + H2O(e) → 2 HNO3(e) + NO(g) AfG [H2O(l)] = -237.2 kJ mol-1 ; AFG°[HNO3(e)] = -79.9 kJ mol-1 ; AfG [NO(g)] = 86.7 kJ mol-1; AfG°[NO2(g)] = 51.8kJ mol-1

At -13.0 °C the pressure equilibrium constant K, = 5.8 x 10 for a certain reaction. Here are some facts about the reaction: • Some of the reactants are liquids and solids. • If the reaction is run at constant pressure, the volume increases by 14.%. • The constant pressure molar heat capacity C = 2.03 J· mol. K'. - 1 %3D As Yes. 10 Using these facts, can you calculate K, at 0.80 °C? d. No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Yes, and K, will be bigger. If you said no, can you at least decide whether K¸ at Yes, and K. will be 0.80 °C will be bigger or smaller than K̟ at –13.0 °C? smaller. d. No. Continue Submit Assignment 144H TAKING YOU TO A NEW REALITY et unvmedreabiy PREDATOR

Using reaction free energy to predict equilibrium composition Consider the following equilibrium: 2NOCI (g) = 2NO (g) + Cl2 (g) AGº =41. kJ Now suppose a reaction vessel is filled with 7.45 atm of nitrosyl chloride (NOCI) and 6.59 atm of chlorine (Cl₂) at 335. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of C₁₂ tend to rise or fall? ☐ x10 fall Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of C12 will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of C₁₂ 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. yes no atm

Consider the following reaction at 37°C. 2 NOCI(g) = 2 NO(g) + Cl₂(g) AG⁰ = 38.5 kJ If 2.17 atm of NOCI are reacted in a rigid container at 37°C, calculate the equilibrium partial pressure (in atm) of NO. atm