# At 27° and 750 mm pressure the volume of a definite mass of gas 3000 ml calculate the volume of the gas at STP ?

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#### Explanation

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#### Explanation:

I want someone to double check my answer

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anor277 Share
Oct 20, 2017

You might have to work on this question.....we have the volume already quoted. We can calculate the molar quantity on the given data....

#### Explanation:

The basic equation is $P V = n R T$

We have a volume, a temperature, and a pressure. And thus we can work on the molar quantity. We know that $1 \cdot a t m$ will support a column of mercury that is $760 \cdot m m$ high....and so.....

$n = \frac{P V}{R T} = \frac{\frac{750 \cdot m m \cdot H g}{760 \cdot m m \cdot H g \cdot a t {m}^{-} 1} \times 3.000 \cdot L}{0.0821 \cdot L \cdot a t m \cdot {K}^{-} 1 \cdot m o {l}^{-} 1 \times 300 \cdot K}$

I make this approx. $0.1 \cdot m o l$ of gas.....

The key to doing these question is to use the correct gas constant, and the correct units. As chemists, we typically deal with litres and atmospheres, and we know how to access $m m \cdot H g$ from atmospheres, and also $1 \cdot L = 1 \cdot {\mathrm{dm}}^{3} = {10}^{-} 3 \cdot {m}^{3}$. In examinations, the gas constant is quoted with a range of units; as a chemist $R = 0.0821 \cdot L \cdot a t m \cdot {K}^{-} 1 \cdot m o {l}^{-} 1$ is probably most appropriate.

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