The equilibrium constant for a reaction is 0.599 at 25C. What is the value of delta G for this reaction in kJ/mol? Include correct units and sig fig

10. Use data from your textbook’s appendix to determine ΔG° for the following reaction at 549 K and standard conditions:CH2O(g) + 2 H2(g) ⇌ CH4(g) + H2O(g).(a) 193.7 kJ (b) ‒193.7 kJ (c) 5.749×104 kJ (d) ‒150.1 kJ 11. Determine the equilibrium constant (K) for the reaction in the problem above. CH2O(g) + 2 H2(g) ⇌ CH4(g) + H2O(g).(a) 481 (b) 1.07×109 (c) 2.08×10‒3 (d) 1.87×1014                        CH2O(g) + 2 H2(g) ⇌ CH4(g) + H2O(g). H(kJ/mol)       -108.6        0             -74.6         -241.8 S (J.mol k)       218.8         130.7       186.3          188.8

Consider the following system at equilibrium where ΔΗ° 108 kJ, and Kc = 1.29 × 10-2, at 600 K: = COC1₂ (g) ⇒ CO(g) + Cl₂ (9) If the temperature on the equilibrium system is suddenly decreased: The value of Ke increases decreases remains the same ccess The value of Qc Ois less than Ke Dis greater than K Ois equal to Ke The reaction must Orun in the forward direction to reestablish equilibrium run in the reverse direction to reestablish equilibrium Oremain in the current position, since it is already at equilibrium The concentration of Cl₂ will Oincrease decrease Oremain the same values I needed TON

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According to LeChatelier's principle, when the reaction quotient is less than the equilibrium constant of a reaction, the reaction: A must shift toward products to reach equilibrium. B must shift toward reactants to reach equilibrium. (c) results in an increase in standard enthalpy of formation of reactants. results in an increase in standard enthalpy of formation of products.

ment/takeCovalentActivity.do?locator3Dassignment-take Review Topical Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° =-87.9 kJ, and K. = 83.3 , at 500 K: PCI3 (g) + Cl2 (g) PCI5 (g) If the TEMPERATURE on the equilibrium system is suddenly increased: The value ofK. A. Increases B. Decreases C. Remains the same The value of Qe A. Is greater than K. B. Is equal to K. C. Is less than K. The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of Cl, will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Retry Entire Group 8 more group attempts remaining Pre 50 hp

Consider the following equilibrium: N2 g) +3H, (g) =2NH3 (g) AG" = - 34. kJ Now suppose a reaction vessel is filled with 4.68 atm of nitrogen (N, and 2.51 atm of ammonia (NH,) at 260. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NH, tend to rise or fall? fall Is it possible to reverse this tendency by adding H,? In other words, if you said the pressure of NH, will tend to rise, can that yes be changed to a tendency to fall by adding H,? Similarly, if you said the no pressure of NH, 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 H, needed to reverse it. || atm Round your answer to 2 significant digits. O O

Q4. (a) What is Eell for the following unbalanced reaction? Fe (s) + O2 (g) + 2H20 (4) Fe3 (aq) + 40H (aq) (b) Balance the reaction. (c) What is A,G° for the reaction? (d) What are the conditions of the above process?

FaceboOK [Review Topics] [References) Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° 268 kJ, and K. 5.10x106, at 548 K. %3D NH,CI(s) NH3(g) + HCI(g) When some moles of NH,CI(s) are removed from the equilibrium system at constant temperature: The value of K The value of Q. The reaction must O run in the forward direction to restablish equilibrium. O run in the reverse direction to restablish equilibrium. O remain the same. It is already at cquilibrium. The concentration of NH, will Retry Entire Group 1 more group attempt remaining Submit Answer

Consider the following reaction at 25 °C: 3 NiO(s) + 2 NH,(g) → 3 Ni(s) + N,(g) + 3 H,O(g) If AG° = -18.1 kJ/mol, determine the value of the equilibrium | %3D constant at 25 °C. 3 4 C 7 8. 9. +/- x 100 2. 5