Question

1. if a gas in an expandable container is pressurized from 15.0 atmospheres to 16.0 atmospheres and its original moles was 1.55, how many moles would there be after the container is pressurized? n1 = 1.55 p1 = 15 n2 =? p2 = 16.0

Explanation:

Step1: Identify the relevant gas law

We use Avogadro's - Gay - Lussac's law in the form $\frac{P_1}{n_1}=\frac{P_2}{n_2}$ for a gas at constant volume and temperature.

Step2: Rearrange the formula to solve for $n_2$

From $\frac{P_1}{n_1}=\frac{P_2}{n_2}$, we can get $n_2=\frac{P_2n_1}{P_1}$.

Step3: Substitute the given values

Given $P_1 = 15.0$ atm, $n_1=1.55$ mol, $P_2 = 16.0$ atm. Then $n_2=\frac{16.0\times1.55}{15.0}$.

Step4: Calculate the result

$n_2=\frac{24.8}{15.0}\approx1.65$ mol.

Answer:

$1.65$ mol