Calculate the amount of NO_2 required for producing 4 ~g moles of HNO_3 as per the chemical reaction, 3 NO_2+H_2 O longrightarrow 2 HNO_3+NO . Given, the gram molecular weights of di-nitrogen and di-oxygen gases are 28 ~g and 32 ~g respectively.

Correct answer: (A) 276 ~g. 4 ~g mole HNO_3=4 × 63=252 ~g HNO_3 underset(3 × 46=138 ~g)3 NO_2+H_2 O longrightarrow underset(2 × 63=126 ~g)2 HNO_3+NO According to the balance chemical reaction 126 ~g HNO_3 produced by 138 ~g NO_2 ∴ 252 ~g HNO_3 will be produced by 126/138 × 252=276 ~g NO_2 Hence, the correct option is (1).

Q37 / 160 · AP EAMCET 2020 (22 Sep Shift 2) · Chemistry

Calculate the amount of $\mathrm{NO}_2$ required for producing $4 \mathrm{~g}$ moles of $\mathrm{HNO}_3$ as per the chemical reaction, $3 \mathrm{NO}_2+\mathrm{H}_2 \mathrm{O} \longrightarrow 2 \mathrm{HNO}_3+\mathrm{NO}$. Given, the gram molecular weights of di-nitrogen and di-oxygen gases are $28 \mathrm{~g}$ and $32 \mathrm{~g}$ respectively.

Correct answer
A
$276 \mathrm{~g}$
B
$274 \mathrm{~g}$
C
$2 \mathrm{~g}$
D
$275 \mathrm{~g}$

Solution

$4 \mathrm{~g}$ mole $\mathrm{HNO}_3=4 \times 63=252 \mathrm{~g} \mathrm{HNO}_3$ $$ \underset{(3 \times 46=138 \mathrm{~g})}{3 \mathrm{NO}_2+\mathrm{H}_2 \mathrm{O} \longrightarrow} \underset{(2 \times 63=126 \mathrm{~g})}{2} \mathrm{HNO}_3+\mathrm{NO} $$ According to the balance chemical reaction $126 \mathrm{~g} \mathrm{HNO}_3$ produced by $138 \mathrm{~g} \mathrm{NO}_2$ $\therefore 252 \mathrm{~g} \mathrm{HNO}_3$ will be produced by $$ \frac{126}{138} \times 252=276 \mathrm{~g} \mathrm{NO}_2 $$ Hence, the correct option is (1).

Hence, the correct answer is option: 'A'.

Solution

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