What is the volume occupied by a $91.8 \cdot g$ $91.8g$ mass of carbon dioxide that is heated to $517.2 \cdot K$ $517.2K$ , and subjected to a pressure of $287 \cdot Torr$ $287*"Torr"$ ?

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What is the volume occupied by a $91.8 \cdot g$ $91.8g$ mass of carbon dioxide that is heated to $517.2 \cdot K$ $517.2K$ , and subjected to a pressure of $287 \cdot Torr$ $287*"Torr"$ ?

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Answer 1 · 2017-06-20T07:38:38

$V ≅ 235 \cdot L$ $V~=235*L$

Explanation:

Given the Ideal Gas equation..... $P V = n R T$ $PV=nRT$

So $V = \frac{n R T}{P}$ $V=(nRT)/P$ , and we know that $760 \cdot m m \cdot H g \equiv 1 \cdot a t m$ $760*mm*Hg-=1*atm$

$V = \frac{\frac{91.8 \cdot g}{44.01 \cdot g \cdot m o l^{- 1}} \times 0.0821 \cdot \frac{L \cdot a t m}{K \cdot m o l} \times 517.2 \cdot K}{\frac{287 \cdot Torr}{760 \cdot Torr \cdot a t m^{- 1}}} = ? ? L .$ $V=((91.8*g)/(44.01*g*mol^-1)xx0.0821*(L*atm)/(K*mol)xx517.2*K)/((287*"Torr")/(760*"Torr"*atm^-1))=??L.$

The gas constant conveniently gives us the volume in $litres$ $"litres"$ .

Note here that I have (i) converted the pressure in $Torr$ $"Torr"$ , and (ii) converted the temperature to $degrees Kelvin$ $"degrees Kelvin"$ , which are typically used in these reactions.

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What is the volume occupied by a $91.8 \cdot g$ $91.8g$ mass of carbon dioxide that is heated to $517.2 \cdot K$ $517.2K$ , and subjected to a pressure of $287 \cdot Torr$ $287*"Torr"$ ?

1 Answer

Explanation:

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Science

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Humanities

... and beyond

What is the volume occupied by a 91.8⋅g91.8*g mass of carbon dioxide that is heated to 517.2⋅K517.2*K, and subjected to a pressure of 287⋅Torr287*"Torr"?

1 Answer

Explanation:

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What is the volume occupied by a $91.8 \cdot g$ $91.8g$ mass of carbon dioxide that is heated to $517.2 \cdot K$ $517.2K$ , and subjected to a pressure of $287 \cdot Torr$ $287*"Torr"$ ?