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Omniscience
Group Title
Consider the gaseous equilibrium
\[2HI(g) \rightleftharpoons
H_2(g) +I_2(g)\]
the addition of more hydrogen will shift the equilibrium to the left right? If yes I don't get why; because there are two volumes in the products?
 2 years ago
 2 years ago
Omniscience Group Title
Consider the gaseous equilibrium \[2HI(g) \rightleftharpoons H_2(g) +I_2(g)\] the addition of more hydrogen will shift the equilibrium to the left right? If yes I don't get why; because there are two volumes in the products?
 2 years ago
 2 years ago

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apoorvk Group TitleBest ResponseYou've already chosen the best response.2
The addition of more hydrogen would shift the reaction towards the reactant side, since you;re adding more 'product'.
 2 years ago

apoorvk Group TitleBest ResponseYou've already chosen the best response.2
Oh you mentioned 'left'  I only noticed the 'right' beside it. My bad lol.
 2 years ago

UnkleRhaukus Group TitleBest ResponseYou've already chosen the best response.1
the gas is at lower energy when there are less moles of gas {ie less pressure the gas pressures are stable when there are as many moles of reactant/products
 2 years ago

Omniscience Group TitleBest ResponseYou've already chosen the best response.0
then it shift to the left or right?
 2 years ago

UnkleRhaukus Group TitleBest ResponseYou've already chosen the best response.1
if you add to the right, some will move to the left
 2 years ago

Omniscience Group TitleBest ResponseYou've already chosen the best response.0
the hydrogen would move to the left( reactants)?
 2 years ago

apoorvk Group TitleBest ResponseYou've already chosen the best response.2
The basic funda is that, since more hydrogen has been added, the collision frequency between hydrogen and iodine molecules would increase, and hence, the reformation of HI would be get a 'push', and hence the equilibrium 'shifts towards left' a bit!
 2 years ago

Omniscience Group TitleBest ResponseYou've already chosen the best response.0
i got it; thanks
 2 years ago
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