## question from module

josephyim1L
Posts: 61
Joined: Fri Sep 28, 2018 12:15 am

### question from module

13. State whether the equilibrium shifts towards products, reactants, or neither when the given change occurs.
2 HI(g) + Cl2(g) ⇌ 2 HCl(g) + I2(s) delta H° = -238.0 kJ.mol-1
i. The volume of the system is compressed.
ii. The temperature of the system is decreased.

Can someone explain the answer to this question?

Rimsha Hussaini 1A
Posts: 31
Joined: Fri Sep 28, 2018 12:20 am

### Re: question from module

When the volume of a system is compressed, the effect on the system depends on how many moles are on each side of the equation. If the moles of the reactants equal the moles of the products, like in this situation, the change in volume has an equal effect on the reactants and the products. Thus, the system remains in equilibrium and does not shift in either direction.

Given that the delta H is negative, we know that this reaction is an exothermic one. Lowering the temperature favors the forward reaction and the reaction shifts towards the products.

805087225
Posts: 30
Joined: Thu Jun 07, 2018 3:00 am

### Re: question from module

Same number of moles, so no change in direction of equilibrium!
And temperature is as explained above.

Sophia Ding 1B
Posts: 62
Joined: Fri Sep 28, 2018 12:16 am

### Re: question from module

Something that helps me with temperature shift is that when it's a negative delta h, you can think of there being a product of heat (+heat on the product side) and when delta h is positive then there is +heat on the reactant side. Thus, if temperature is decreased, then equilibrium would shift to where heat is in the equation: the products.

Saman Andalib 1H
Posts: 73
Joined: Fri Sep 28, 2018 12:16 am

### Re: question from module

When the volume of the container is decreased, the pressure in the container is therefore increased. This increase in the pressure will cause the reaction to shift towards the side of the chemical equation with fewer moles of gas. Therefore, the equation will shift towards the products. When the temperature of the system is decreased, the equation will shift towards the side which requires the temperature input to proceed. Therefore, the reaction will again shift to the products.

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