es/378413/quizzes/2118546/take/questions/46121239 e sure I can read the writing and numbers legibly. Number your solutions accordingly. Question 12 3 pts The Haber-Bosch process is the main industrial route to production of ammonia and is written as: \( \mathrm{N}_{2(\mathrm{~g})}+3 \mathrm{H}_{2(\mathrm{~g})} \leftrightarrow \) \( 2 \mathrm{NH}_{3(\mathrm{~g})} \) with a \( \Delta \mathrm{H}^{\circ} \) for the reaction being \( -92.4 \mathrm{~kJ} / \mathrm{mol} \). How would addition of a catalyst affect the equilibrium? Which direction, if any, will the reaction go to re-establish the equilibrium? Ask StudyBuddy cannot be determined no effect or no change forward reverse Previous Next Search
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A catalyst speeds up the rate of a reaction by lowering the activation energy but does not affect the position of the equilibrium. Show more…
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The Haber-Bosch process has been used since 1913 to produce ammonia, which is used to make fertilizers. This has allowed food production to keep up with rapid population growth (1.8 billion in 1913, nearly 8 billion today). The reaction is given below: 3H2 (g) + N2 (g) ⇌ 2NH3 (g) ΔH° = -91.8 kJ Assuming the system is at equilibrium, which of the following changes would shift the equilibrium right to make more NH3? Select all that apply adding a catalyst to the reaction mixture increasing the volume of the container decreasing the temperature of the reaction adding more H2 to the reaction mixture
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For the following reaction, determine the effect of each of the following changes on both the rate of reaction and the equilibrium position. Include a brief explanation of your reasoning: N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) + 22.1 kcal/mol increase in temperature: RATE OF REACTION - EQUILIBRIUM SHIFT - increase in pressure/decrease in volume: RATE OF REACTION - EQUILIBRIUM SHIFT - increase in [H2]: RATE OF REACTION - EQUILIBRIUM SHIFT - increase in [NH3]: RATE OF REACTION - EQUILIBRIUM SHIFT - addition of a catalyst: RATE OF REACTION - EQUILIBRIUM SHIFT -
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