What is the pressure of 2 , mol of NH_3 at 27 | vedclass

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(B) The van der Waals equation is given by: $\left( P + \frac{n^2 a}{V^2} \right) (V - nb) = nRT$ Given: $n = 2 \, mol$,$V = 5 \, L$,$T = 27 + 273 = 3

Vedclass · Accepted Answer

$9.33$

Vedclass · Answer

(B) The van der Waals equation is given by: $\left( P + \frac{n^2 a}{V^2} ight) (V - nb) = nRT$ Given: $n = 2 \, mol$,$V = 5 \, L$,$T = 27 + 273 = 300 \, K$,$a = 4.17$,$b = 0.03711$,$R = 0.0821 \, L \, atm \, K^{-1} \, mol^{-1}$. Substituting the values: $\left( P + \frac{2^2 	imes 4.17}{5^2} ight) (5 - 2 	imes 0.03711) = 2 	imes 0.0821 	imes 300$ $\left( P + \frac{16.68}{25} ight) (5 - 0.07422) = 49.26$ $(P + 0.6672) 	imes 4.92578 = 49.26$ $P + 0.6672 = \frac{49.26}{4.92578} \approx 10.00$ $P = 10.00 - 0.6672 = 9.3328 \, atm \approx 9.33 \, atm$.

Gas	$a / (kPa \cdot dm^6 \cdot mol^{-2})$	$b / (dm^3 \cdot mol^{-1})$
$A$	$642.32$	$0.05196$
$B$	$155.21$	$0.04136$
$C$	$431.91$	$0.05196$
$D$	$155.21$	$0.4382$

$P \text{ (bar)}$	$\frac{PV}{RT}$
$1$	$1$
$2$	$1$
$3$	$1$
$3.1$	$1.2$
$3.5$	$1.4$
$4.0$	$1.5$

What is the pressure of $2 \, mol$ of $NH_3$ at $27 \, ^oC$ when its volume is $5 \, L$ using the van der Waals equation (in $, atm$)? ($a = 4.17 \, L^2 \, bar \, mol^{-2}$,$b = 0.03711 \, L \, mol^{-1}$)

Similar Questions

Consider the following table:

Gas $a / (kPa \cdot dm^6 \cdot mol^{-2})$ $b / (dm^3 \cdot mol^{-1})$

$A$ $642.32$ $0.05196$

$B$ $155.21$ $0.04136$

$C$ $431.91$ $0.05196$

$D$ $155.21$ $0.4382$

$a$ and $b$ are van der Waals constants. The correct statement about the gases is:

The following data is obtained for one mole of a gas. The gas deviates from ideal behavior in the pressure (in bar) range:
$P \text{ (bar)}$ $\frac{PV}{RT}$
$1$ $1$
$2$ $1$
$3$ $1$
$3.1$ $1.2$
$3.5$ $1.4$
$4.0$ $1.5$

What will the van der Waals equation be at high temperature and low pressure?

Gases deviate from the ideal gas behaviour because their molecules

Which equation shows the correct form of the Berthelot equation?

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