(i) A gas of mass $32 g m s$ has volume of $20$ litres at S.T.P. Calculate the gram molecular weight of the gas.
(ii) How much Calcium oxide is formed when $82 g$ of calcium nitrate is heated? Also find the volume of nitrogendioxide evolved :
$2 C a {(N O_{3})}_{2} ⟶ 2 C a O + 4 N O_{2} + O_{2}$
$(C a = 40, N = 14, O = 16)$

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Solution

(i) The mass of $22.4 l$ of gas at S.T.P. is equal to its gram molecular mass.
$20$ litres of gas at S.T.P. weighs $= 32 g m s$
$∴$ $22.4$ litres of gas will weigh $= \frac{32}{20} \times 22.4$
$= 35.84 g m s$
$≃ 36 g m s$ .
Therefore, Gram molecular weigh of the gas is $36 g m s$ .
(ii) $\begin{matrix} 2 C a {(N O_{3})}_{2} 2 [40 + 2 (14 + 48)] = 328 g m \end{matrix} \begin{matrix} Δ - ------- \to \end{matrix} \begin{matrix} 2 C a O 112 g m \end{matrix} \begin{matrix} + 4 N O_{2} 4 m o l e s = 4 \times 22.4 = 89.6 l \end{matrix} \begin{matrix} + O_{2} \end{matrix}$
1. If $328 g$ of $C a {(N O_{3})}_{2}$ releases $112 g m$ of $C a O$
Then $82 g$ of $C a {(N O_{3})}_{2}$ will releases $= \frac{112}{328} \times 82$
$= 28 g m s$ of $C a O$
2. If $328 g$ of $C a {(N O_{3})}_{2}$ releases $89.6 l$ of $N O_{2}$ at STP
Then $82 g$ of $C a {(N O_{3})}_{2}$ will releases $= \frac{89.6}{328} \times 82$
$= 22.4$ litres of nitrogendioxide.

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(i) A gas of mass 32gms has volume of 20 litres at S.T.P. Calculate the gram molecular weight of the gas.(ii) How much Calcium oxide is formed when 82g of calcium nitrate is heated? Also find the volume of nitrogendioxide evolved : 2Ca(NO3)2⟶2CaO+4NO2+O2 (Ca=40,N=14,O=16)