Write the van der Waals equation.
(N/A) The van der Waals equation for $n$ moles of a real gas is given by: $\left(p + \frac{an^2}{V^2}\right)(V - nb) = nRT$,where $p$ is the pressure,$V$ is the volume,$T$ is the temperature,$R$ is the universal gas constant,and $a$ and $b$ are the van der Waals constants.
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Which statement is correct regarding the equation $Z = PV/RT$?
Easy
View SolutionConsider the following gases and their corresponding $ 'a'$ values given in parentheses: $CH_4 (2.25), N_2 (1.35), O_2 (1.36)$,and $CO (1.46)$. Which of these gases will be the most difficult to liquefy?
Medium
View SolutionConsider the van der Waals constants,$a$ and $b,$ for the following gases.
Gas $Ar$ $Ne$ $Kr$ $Xe$ $a \ (atm \ dm^6 \ mol^{-2})$ $1.3$ $0.2$ $5.1$ $4.1$ $b \ (10^{-2} \ dm^3 \ mol^{-1})$ $3.2$ $1.7$ $1.0$ $5.0$
Which gas is expected to have the highest critical temperature?
| Gas | $Ar$ | $Ne$ | $Kr$ | $Xe$ |
| $a \ (atm \ dm^6 \ mol^{-2})$ | $1.3$ | $0.2$ | $5.1$ | $4.1$ |
| $b \ (10^{-2} \ dm^3 \ mol^{-1})$ | $3.2$ | $1.7$ | $1.0$ | $5.0$ |
Which gas is expected to have the highest critical temperature?
Match the Van der Waals constant $a$ (in $L^2 \cdot bar \cdot mol^{-2}$) for the following gases:
Gas $a$ value $1. C_6H_{6(g)}$ $a. 0.217$ $2. C_6H_5CH_{3(g)}$ $b. 5.464$ $3. Ne_{(g)}$ $c. 18.000$ $4. H_2O_{(g)}$ $d. 24.060$
| Gas | $a$ value |
|---|---|
| $1. C_6H_{6(g)}$ | $a. 0.217$ |
| $2. C_6H_5CH_{3(g)}$ | $b. 5.464$ |
| $3. Ne_{(g)}$ | $c. 18.000$ |
| $4. H_2O_{(g)}$ | $d. 24.060$ |
Difficult
View SolutionUnder which conditions will a real gas behave most like an ideal gas?
Medium
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