7. if i have 24.0 g of co2 at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature (in…

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 $m = 24.0\ g$. So $n=\frac{24.0\ g}{44.01\ g/mol}\approx0.545\ mol$.

Step2: Use the ideal gas law

The ideal - gas law is $PV = nRT$, where $P = 5.6\ atm$, $V = 12\ L$, $n = 0.545\ mol$, and $R=0.0821\ L\cdot atm/(mol\cdot K)$. We need to solve for $T$. Rearranging the ideal - gas law for $T$ gives $T=\frac{PV}{nR}$. Substitute the values: $T=\frac{5.6\ atm\times12\ L}{0.545\ mol\times0.0821\ L\cdot atm/(mol\cdot K)}$. First, calculate the numerator: $5.6\ atm\times12\ L = 67.2\ L\cdot atm$. Then, calculate the denominator: $0.545\ mol\times0.0821\ L\cdot atm/(mol\cdot K)\approx0.0447\ L\cdot atm/K$. Finally, $T=\frac{67.2\ L\cdot atm}{0.0447\ L\cdot atm/K}\approx1503\ K$.

Answer:

$1503\ K$