B. The highly toxic gas phosgene is produced by the reaction CO(g) + Cl2(g) COCl2(g), ΔH = –108 kJ/mol. Use this reaction to answer the following questions.

i. How would increasing the pressure of the system affect the reaction yield? Explain your answer. (2 points)

ii. How would increasing the pressure of the system affect the reaction rate? Explain your answer. (2 points)

iii. How would increasing the temperature of the system affect the reaction yield? Explain your answer. (2 points)

iv. How would increasing the temperature of the system affect the reaction rate? Explain your answer. (2 points)

Question

11-02-2022
Chemistry

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B. The highly toxic gas phosgene is produced by the reaction CO(g) + Cl2(g) COCl2(g), ΔH = –108 kJ/mol. Use this reaction to answer the following questions.

i. How would increasing the pressure of the system affect the reaction yield? Explain your answer. (2 points)

ii. How would increasing the pressure of the system affect the reaction rate? Explain your answer. (2 points)

iii. How would increasing the temperature of the system affect the reaction yield? Explain your answer. (2 points)

iv. How would increasing the temperature of the system affect the reaction rate? Explain your answer. (2 points)

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unicornetfairies unicornetfairies · Answer 1 · 2022-02-13T12:24:56+01:00

Answer:

I. Increasing pressure will allow more frequent successful collision between particles due to the particles being closer together.

II. Rate of reaction increases due to more products being made; as increased pressure favours the exothermic side of the equilibrium.

III. Increasing temperature provides particles lots of (Kinetic) energy, for more frequent successful collision due to the particles moving at a faster rate than before. However, favouring the endothermic side of the equilibrium due to lots of energy required to break and form new bonds.

IV. Rate of reaction increases due to increase temperature favouring both directions of the equilibrium - causing products to form faster.

Hope this helps!

kumaripoojavt kumaripoojavt · Answer 2 · 2022-05-27T13:28:20+02:00

I. Increasing pressure will allow more frequent successful collision between particles due to the particles being closer together.

II. Rate of reaction increases due to more products being made; as increased pressure favours the exothermic side of the equilibrium.

III. Increasing temperature provides particles lots of (Kinetic) energy, for more frequent successful collision.

IV. Rate of reaction increases due to increased temperature favouring both directions of the equilibrium - causing products to form faster.

What is toxic gas phosgene?

Phosgene is extremely toxic by acute (short-term) inhalation exposure. Severe respiratory effects, including pulmonary edema, pulmonary emphysema, and death have been reported in humans.

I. If the pressure of gaseous reactants is increased, there are more reactant particles for a given volume. There will be more collisions and so the reaction rate is increased. The higher the pressure of reactants, the faster the rate of a reaction will be.

II. Increasing the pressure on a gas reaction shifts the position of equilibrium towards the side with fewer moles of gas molecules.

III. Increasing temperature provides particles lots of (Kinetic) energy, for more frequent successful collision due to the particles moving at a faster rate than before. However, favouring the endothermic side of the equilibrium due to lots of energy required to break and form new bonds.

IV. If the temperature is increased, the position of equilibrium moves in the direction of the endothermic reaction. if the temperature is reduced, the position of equilibrium moves in the direction of the exothermic reaction.

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