what pressure (in atm) does 3.54 moles of chlorine gas at 376 k exert on the walls of its 51.2 l container…

Explanation:

Step1: Identify the ideal - gas law formula

The ideal - gas law is $PV = nRT$, where $P$ is pressure, $V$ is volume, $n$ is the number of moles, $R$ is the ideal - gas constant ($R=0.0821\ \frac{L\cdot atm}{mol\cdot K}$), and $T$ is temperature in Kelvin. We need to solve for $P$, so we can rewrite the formula as $P=\frac{nRT}{V}$.

Step2: Substitute the given values

We are given $n = 3.54\ mol$, $T = 376\ K$, $V=51.2\ L$, and $R = 0.0821\ \frac{L\cdot atm}{mol\cdot K}$. $P=\frac{3.54\ mol\times0.0821\ \frac{L\cdot atm}{mol\cdot K}\times376\ K}{51.2\ L}$

Step3: Calculate the pressure

First, calculate the numerator: $3.54\times0.0821\times376 = 3.54\times30.8696=109.278384$. Then, divide by the volume: $P=\frac{109.278384}{51.2}\ atm\approx2.13\ atm$.

Answer:

$2.13$