For the exothermic reaction 3H2(g) + N2(g) ↔ 2NH3(g) + HEAT, which of the following changes could be carried out to cause the reaction to shift to the right? Adding H2 Adding NH3 Increasing the temp...

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For the exothermic reaction 3H2(g) + N2(g) ↔ 2NH3(g) + HEAT, which of the following changes could be carried out to cause the reaction to shift to the right? Adding H2 Adding NH3 Increasing the temp...

For the exothermic reaction 3H2(g) + N2(g) ↔ 2NH3(g) + HEAT, which of the following changes could be carried out to cause the reaction to shift to the right?
1. Adding H2
2. Adding NH3
3. Increasing the temperature
4. Removing N2

science chemistry

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Answer 1

Answer #1

Answer

a) Adding H2

Explanation

According to Le chatlier principle , if a change such as change in concentration, change in pressure , change in volume or change in temperature is applied to an equillibrium the equillibrium adjust itself to counteract to the applied change.

a) Addding H2 shift the equillibrium to the right so that the added H2 will be consumed

b) Adding NH3 shift the equillibrium to the left so that the added NH3 will be consumed

c) Reverse reaction is endothermic reaction ,so increasing temperature shift the equillibrium to left so that the applied heat will be consumed

d) Removing N2 shift the equillibrium to left so that removed N2 will be compensated.

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Answer 2

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For the exothermic reaction 3H2(g) + N2(g) ↔ 2NH3(g) + HEAT, which of the following changes could be carried out to cause the reaction to shift to the right? Adding H2 Adding NH3 Increasing the temp...

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Homework Answers

Add Answer to: For the exothermic reaction 3H2(g) + N2(g) ↔ 2NH3(g) + HEAT, which of the following changes could be carried out to cause the reaction to shift to the right? Adding H2 Adding NH3 Increasing the temp...

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Add Answer to:
For the exothermic reaction 3H2(g) + N2(g) ↔ 2NH3(g) + HEAT, which of the following changes could be carried out to cause the reaction to shift to the right? Adding H2 Adding NH3 Increasing the temp...