The equilibrium constant at 25°C for the reaction 2 NO2(g) 2 N,O4(g) is 6.8. At 200°C the equilibrium constant is 1.21 × 10-3. Calculate the enthalpy change (AH) for this reaction, assuming that AH° and AS° of the reaction are constant over the temperature range from 25°C to 200°C.

Determine the equilibrium vapor pressure of germanium metal at 326.0 °C. The standard enthalpy of vaporization of germanium is 376.6 kJ/mol and the vapor pressure at 100.0 °C is 1.6E-32 Pa.

Consider the following reversible reaction at equilibrium: C6H12O6(aq) + 6 O2(g)      6 CO2(g) + 6 H2O(l). Given that this reaction is exothermic, if heat is added to the equilibrium system, how is the stress relieved?

8.B A certain reaction has an equilibrium constant of K = 8.3×10$ at 25°C with a temperature-independent standard enthalpy of reaction of 34.2 kJ/mol. (a) What is the equilibrium constant at 37°C? (b) Use Le Chatelier's principle to defend your answer.

Determine AG° for the reaction 2 SO,(g) + 0,(g) →2 SO3(g) at 25 °C. Thermodynamic Data at 25 °C Species AH? in kJ/mol AG? in kJ/mol S° in J/(mol·K) O2 (g) SO2 (g) SO3 (g) 0. 205.0 -296.8 -300.1 248.2 -395.7 -371.1 256.8

At -8.64 °C the concentration equilibrium constant K = 7.7 for a certain reaction. Here are some facts about the reaction: -1 • The initial rate of the reaction is 5.3 mol·L¯¹·s¯¹. . If the reaction is run at constant pressure, 132. kJ/mol of heat are absorbed. • The constant pressure molar heat capacity C = 2.97 J'mol K¹. Yes. Using these facts, can you calculate K at 16. °C? x10 O No. If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether Kat 16. °C will be bigger or smaller than K at -8.64 °C? C Yes, and K will be bigger. Yes, and K will be smaller. No.

For a certain chemical reaction, the standard Gibbs free energy of reaction at 5.00 °C is -76.7 kJ. Calculate the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 ☐ x10 × Ś

For a certain chemical reaction, the standard Gibbs free energy of reaction at 20.0 °C is 90.2 kJ. Calculate the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = || x10

Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant K at 25.0 °C for the following reaction. 2 NO (g) N2(g) + O2(g) Round your answer to 2 significant digits. K ☐ x10 ค

The steam reforming reaction of methane follows this chemical equation: CHA(g) + H50(g) - CO(g) + 3 H2(g) A H° = +193 kJ/mol At 298 K the reaction lies far to the reactant side with a very small equilibrium constant of 2.35 × 10-23. To obtain a significant amount of the desired hydrogen gas product, the reaction is operated at very high temperatures. What is the equilibrium constant at 1100 K?