What volume is occupied by a $7 \cdot g$ $7g$ mass of dinitrogen gas at a temperature of $300 \cdot K$ $300K$ , and a pressure of $750 \cdot m m \cdot H g$ $750mmHg$ ?

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What volume is occupied by a $7 \cdot g$ $7g$ mass of dinitrogen gas at a temperature of $300 \cdot K$ $300K$ , and a pressure of $750 \cdot m m \cdot H g$ $750mmHg$ ?

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Answer 1 · 2017-07-10T05:29:19

$V ≅ 6 \cdot L$ $V~=6*L$

Explanation:

Given $V = \frac{n R T}{P}$ $V=(nRT)/P$ , we know that nitrogen (LIKE most of the elemental gases) is a DIATOM, i.e. $N_{2}$ $N_2$ . We also know that $760 \cdot m m \cdot H g \equiv 1 \cdot a t m .$ $760*mm*Hg-=1*atm.$ This is a key point, as we can use the height of a mercury column as an accurate representation of pressure.

So $V = \frac{\frac{7.0 \cdot g}{28.0 \cdot g \cdot m o l^{- 1}} \times 0.0821 \cdot \frac{L \cdot a t m}{K \cdot m o l} \times 300 \cdot K}{\frac{750 \cdot m m \cdot H g}{760 \cdot m m \cdot H g \cdot a t m^{- 1}}}$ $V=((7.0*g)/(28.0*g*mol^-1)xx0.0821*(L*atm)/(K*mol)xx300*K)/((750*mm*Hg)/(760*mm*Hg*atm^-1))$

All units EXCEPT $litres$ $"litres"$ cancel, so...........

$~=6*L.......$

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What volume is occupied by a $7 \cdot g$ $7g$ mass of dinitrogen gas at a temperature of $300 \cdot K$ $300K$ , and a pressure of $750 \cdot m m \cdot H g$ $750mmHg$ ?

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Explanation:

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What volume is occupied by a 7*g7⋅g7*g mass of dinitrogen gas at a temperature of 300*K300⋅K300*K, and a pressure of 750*mm*Hg750⋅mm⋅Hg750*mm*Hg?

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Explanation:

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What volume is occupied by a $7 \cdot g$ $7g$ mass of dinitrogen gas at a temperature of $300 \cdot K$ $300K$ , and a pressure of $750 \cdot m m \cdot H g$ $750mmHg$ ?