4) how much volume would you need in order to store 4.0 kg of ar gas at 298 k and 1.15 atm of pressure?
4) how much volume would you need in order to store 4.0 kg of ar gas at 298 k and 1.15 atm of pressure?
Answer
Answer:
$854.5\ L$
Explanation:
Step1: Calculate the number of moles of Ar
The molar - mass of Ar is $M = 39.95\ g/mol$. First, convert the mass of Ar from kg to g: $m=4.0\ kg = 4000\ g$. Then, use the formula $n=\frac{m}{M}$, so $n=\frac{4000\ g}{39.95\ g/mol}\approx100.125\ mol$.
Step2: Use the ideal - gas law
The ideal - gas law is $PV = nRT$, where $P = 1.15\ atm$, $n = 100.125\ mol$, $R=0.0821\ L\cdot atm/(mol\cdot K)$, and $T = 298\ K$. We want to solve for $V$, so $V=\frac{nRT}{P}$. Substitute the values: $V=\frac{100.125\ mol\times0.0821\ L\cdot atm/(mol\cdot K)\times298\ K}{1.15\ atm}$. $V=\frac{100.125\times0.0821\times298}{1.15}\ L\approx854.5\ L$.