how many moles of oxygen are in a 7.68 l container at 355 k and exerting a pressure of 6,513 mm hg on the…

Explanation:

Step1: Convert pressure to atmospheres

1 atm = 760 mmHg. So, $P=\frac{6513}{760}\text{ atm}=8.57\text{ atm}$

Step2: Identify the ideal - gas constant

The ideal - gas constant $R = 0.0821\frac{\text{L}\cdot\text{atm}}{\text{mol}\cdot\text{K}}$

Step3: Use the ideal gas law $PV = nRT$ to find the number of moles $n$

We know $V = 7.68\text{ L}$, $T=355\text{ K}$, $P = 8.57\text{ atm}$, and $R = 0.0821\frac{\text{L}\cdot\text{atm}}{\text{mol}\cdot\text{K}}$. Rearranging the ideal - gas law for $n$ gives $n=\frac{PV}{RT}$. Substitute the values: $n=\frac{8.57\text{ atm}\times7.68\text{ L}}{0.0821\frac{\text{L}\cdot\text{atm}}{\text{mol}\cdot\text{K}}\times355\text{ K}}$ $n=\frac{65.8176}{29.1455}\text{ mol}\approx2.26\text{ mol}$

Answer:

2.26