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anonymous
 3 years ago
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?
anonymous
 3 years ago
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?

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anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0The addition of more hydrogen would shift the reaction towards the reactant side, since you;re adding more 'product'.

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0Oh you mentioned 'left'  I only noticed the 'right' beside it. My bad lol.

UnkleRhaukus
 3 years ago
Best ResponseYou've already chosen the best response.1the 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

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0then it shift to the left or right?

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

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0the hydrogen would move to the left( reactants)?

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0The 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!
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