a 20.0 l tank of co₂ contains 88.0 grams of gas at 500.0 kpa of pressure. what is the temperature of the…

Explanation:

Step1: Calculate the number of moles of CO₂

The molar mass of CO₂ is $M = 12.01+2\times16.00=44.01\ g/mol$. The number of moles $n=\frac{m}{M}$, where $m = 88.0\ g$. So $n=\frac{88.0\ g}{44.01\ g/mol}\approx2.00\ mol$.

Step2: Use the ideal - gas law

The ideal - gas law is $PV = nRT$, where $P = 500.0\ kPa=500000\ Pa$, $V = 20.0\ L = 0.0200\ m^{3}$, $n = 2.00\ mol$, and $R = 8.314\ J/(mol\cdot K)$. We need to solve for $T$. Rearranging the ideal - gas law gives $T=\frac{PV}{nR}$. Substitute the values: $T=\frac{500000\ Pa\times0.0200\ m^{3}}{2.00\ mol\times8.314\ J/(mol\cdot K)}$. $T=\frac{10000\ J}{16.628\ J/K}\approx601\ K$.

Answer:

$601\ K$