Question

missed this? watch kcv: simple gas laws and the ideal gas law, iwe: avogadro’s law; read section 11.7. you can click on the a 0.670-mol sample of helium gas occupies a volume of 10.7 l. part a what is the volume of 0.975 mol of helium gas under the same conditions? express your answer in liters to three significant figures. v = l

Explanation:

Step1: Recall Avogadro's Law

Avogadro's Law states that at constant temperature and pressure, the volume of a gas is directly proportional to the number of moles of the gas, i.e., $\frac{V_1}{n_1}=\frac{V_2}{n_2}$.
Here, $n_1 = 0.670\space mol$, $V_1 = 10.7\space L$, $n_2 = 0.975\space mol$, and we need to find $V_2$.

Step2: Rearrange the formula to solve for $V_2$

From $\frac{V_1}{n_1}=\frac{V_2}{n_2}$, we can rearrange it to $V_2=\frac{V_1\times n_2}{n_1}$.

Step3: Substitute the values into the formula

Substitute $V_1 = 10.7\space L$, $n_1 = 0.670\space mol$, and $n_2 = 0.975\space mol$ into the formula:
$V_2=\frac{10.7\space L\times0.975\space mol}{0.670\space mol}$

Step4: Calculate the value

First, calculate the numerator: $10.7\times0.975 = 10.4225$
Then, divide by the denominator: $\frac{10.4225}{0.670}\approx15.55597$
Round to three significant figures: $15.6\space L$

Answer:

$15.6$