1. Tardigrade
  2. Question
  3. Chemistry
  4. H2(g) + I2(g) leftharpoons 2HI(g) When 46 g of I2 and 1 g of H2 gas heated at equilibrium at 450°C, the equilibrium mixture contained 1.9 g of I2. How many moles of I2 and HI are present at equilibrium?

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Q. $H_{2}(g) + I_{2}(g) \rightleftharpoons 2HI(g)$
When $46$ g of $I_{2}$ and $1\, g$ of $H_{2}$ gas heated at equilibrium at $450°C,$ the equilibrium mixture contained $1.9\, g$ of $I_2$. How many moles of $I_{2}$ and $HI$ are present at equilibrium?

Equilibrium

Solution:

Moles of $I_{2}$, taken $=\frac{46}{254}= 0.181$
Moles of $H_{2}$ taken $= \frac{1}{2}= 0.5$
Moles of $I_{2}$ remaining$ = \frac{1.9}{254} =0.0075$
Moles of $I_{2}$ used $= 0.181 - 0.0075 = 0.1735$
Moles of $H_{2}$ used $= 0.1735$
Moles of $H_{2}$ remaining $= 0.5 - 0.1735 = 0.3265$
Moles of HI formed $= 0.1735 \times 2 = 0.347$
At equilibrium, moles of $I_{2} = 0.0075$ moles
Moles of $HI = 0.347$ moles