Calculate the change in pressure in atm- when 2 moles of NO and 16 g O2 in a 6-25 litre originally at 27-C react to produce the maximum quantity of NO2 possible according to the equation- 2NOg-O2g- 2NO2g -Take R- 112 L atm K1 mol-1-

The correct option is A 2 2NO(g) #160; #160; #160; #160; #160;+ #160; #160; #160; #160; #160; O_2(g) #160; #160; ...

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Byju's Answer

Standard XII

Chemistry

Rate of Reaction

Calculate the...

Question

Calculate the change in pressure (in atm), when 2 moles of NO and 16 g $O_{2}$ in a 6.25 litre originally at $27^{\circ} C$ react to produce the maximum quantity of $N O_{2}$ possible according to the equation.

$2 N O (g) + O_{2} (g) \to 2 N O_{2} (g)$

$[T a k e R = \frac{1}{12} L a t m K^{1} m o l^{- 1}]$

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Solution

The correct option is A 2
$2 N O (g)$ + $O_{2} (g)$ $\to$ $2 N O_{2} (g)$

2 0.5 0
$2 - 2 \times 0.5$ 0 $2 \times 0.5$

1 0 1

$n_{f} = 1 + 1$ and $n_{i} = 2 + 0.5$

$∴ Δ n = (2.5 - 2) = 0.5$

$∴$ change in pressure, $Δ p = \frac{Δ n R T}{V}$

$= 0.5 \times \frac{1}{12} \times \frac{300}{6.25}$

$= 2 a t m$

Hence, the correct answer is option $A$ .

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Calculate the change in pressure (in atm), when 2 moles of NO and 16 g O2 in a 6.25 litre originally at 27∘C react to produce the maximum quantity of NO2 possible according to the equation.2NO(g)+O2(g)→2NO2(g)[Take R=112 L atm K1 mol−1]

The correct option is A 22NO(g) + O2(g) → 2NO2(g) 2 0.5 02−2×0.5 0 2×0.51 0 1nf=1+1 and ni=2+0.5∴Δn=(2.5−2)=0.5∴ change in pressure, Δp=ΔnRTV =0.5×112×3006.25 =2 atmHence, the correct answer is option A.