For the reaction - N2O5g - 2NO2g - 0-5O2gThe mole fraction of N2O5g decomposed at constant volume and temperature is 4-10-x-then calculate the value of x- if the initial pressure is 600 mm Hg and the pressure at any time is 960 mm Hg is-Assume ideal behaviour-

nbsp; amp; N_2O_5(g) amp;→ amp;2NO_2(g) nbsp; amp;→ nbsp; amp;1/2 O_2(g) nbsp; amp; nbsp;Initial P amp; P mm Hg nbsp; ...

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Byju's Answer

Standard XII

Chemistry

Characteristics of Chemical Equilibrium

For the react...

Question

For the reaction : $N_{2} O_{5} (g) \to 2 N O_{2} (g) + 0.5 O_{2} (g)$
The mole fraction of $N_{2} O_{5} (g)$ decomposed at constant volume and temperature is $4 \times 10^{- x}$ ,then calculate the value of x. if the initial pressure is 600 mm Hg and the pressure at any time is 960 mm Hg is.
Assume ideal behaviour.

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Solution

$\begin{matrix} N_{2} O_{5} (g) & \to & 2 N O_{2} (g) & \to & \frac{1}{2} O_{2} (g) I n i t i a l P & P m m H g & 0 & 0 F i n a l P a f t e r t i m e t & P - p & 2 p & \frac{1}{2} p \end{matrix}$
Total pressure = $P - p + 2 p + \frac{1}{2} p$
$= P + \frac{3}{2} p$
Thus, $P \propto 240$ mm
Mole fraction of $N_{2} O_{5}$ decomposed = $\frac{P}{P} = \frac{240}{960} = 0.4$

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Q. For the reaction,

N_{2} O_{5} (g) \to 2 N O_{2} (g) + 0.5 O_{2} (g)

, calculate the mole fraction of

N_{2} O_{5} (g)

decomposed at a constant volume and temperature if the initial pressure is 600 mm Hg and the pressure at any time is 960 mm Hg. Assume ideal gas behaviour.
Write the numerical value (upto 2 digit only) after decimal point only as for 0.19, write 19).

Assume ideal gas behaviour. For the reaction, $N_{2} O_{5} (g) ⇌ 2 N O_{2} (g) + 0.5 O_{2} (g)$ , the initial pressure is 600 mmHg and the pressure at any time is 960 mmHg. The fraction of $N_{2} O_{5} (g)$ decomposed at constant volume and temperature is: