What is the mass of a sample of CO2 if it is held at 24 degrees C, 0.544 atm in a 3.00L flask?

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What is the mass of a sample of CO2 if it is held at 24 degrees C, 0.544 atm in a 3.00L flask?

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Answer 1 · 2015-11-14T01:43:26

2.94g

Explanation:

Use the ideal gas law ( $P V = n R T$ $PV=nRT$ ).

Since the question asks for mass, if we find the number of moles of $C O_{2}$ $CO_2$ , we can multiply that by the molar mass to find the mass of the $C O_{2}$ $CO_2$ gas.

If we want to solve for moles, $n = \frac{P V}{R T}$ $n=(PV)/(RT)$ .

Plug in values: $n = \frac{0.544 \cdot 3.00}{0.08206 \cdot (24 + 273.15)}$ $n=(0.544*3.00)/(0.08206*(24+273.15))$

Remember, the temperature must be in Kelvin, not Celsius.

$n = 0.67$ $n=0.67$

$0.67 m o l$ $0.67mol$ $C O_{2}$ $CO_2$ $\times \frac{44 g}{1 m o l} = 2.94 g$ $xx(44g)/(1mol)=color(blue)(2.94g)$

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What is the mass of a sample of CO2 if it is held at 24 degrees C, 0.544 atm in a 3.00L flask?

1 Answer

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