**Chemical Equilibrium Calculation** **Problem Statement:** Enter your answer in the provided box. For the reaction: \[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \] Given that \( K_c \) is 0.393 at 485°C, calculate \( K_p \) for the reaction at this temperature. \[ K_p = \square \] **Guidance:** For a given reaction at equilibrium, the relationship between the equilibrium constants \( K_c \) and \( K_p \) can be determined using the equation: \[ K_p = K_c(RT)^{\Delta n} \] Where: - \( R \) is the gas constant, typically 0.0821 L·atm/mol·K - \( T \) is the temperature in Kelvin - \( \Delta n \) is the change in moles of gas (\( \text{moles of gaseous products - moles of gaseous reactants} \)) **Steps to follow:** 1. Convert the temperature from Celsius to Kelvin. 2. Calculate \( \Delta n \) for the reaction. 3. Substitute the known values into the \( K_p \) equation to find the answer.

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AutoSave CHEM 212 Final Exam_Fall 2020 Word Search 困 ff steve M SM File Home Insert Draw Design Layout References Mailings Review View Help E Share O Comments 3a) Calculate AGon for this reaction: CH3OH (g) → CO (g) + 2 H2 (g) The equilibrium partial pressures for each component are: CH;OH = 0.620 atm, CO = 0.105 atm, H2 = 0.125 atm b) Is the reaction spontaneous? Briefly explain. 3c) Cells use the hydrolysis of adenosine triphosphate (ATP) as a source of energy. The conversion of ATP to ADP has a standard free energy change of -30.5 kJ/mol. If all the free energy from the metabolism of glucose goes to the conversion of ADP to ATP, how many mole of ATP can be produced for each mole of glucose? Page 3 of 6 492 words D Focus 80%

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