Chapter 5, Problem 5.57P

Interpretation Introduction

Interpretation:

Grams of aluminium that reacts with excess hydrochloric acid to form aluminium chloride and $35.8\text{mL}$ of hydrogen gas over water at $27°\text{C}$ and $751\text{mmHg}$ is to be calculated.

Concept introduction:

Ideal gas law equation is as follows:

$PV=nRT$        (1)

Here,

$P$ is the pressure of the gas.

$V$ is the volume occupied by gas.

$n$ is the number of moles of gas.

$T$ is the temperature in Kelvin.

$R$ is the universal gas constant.

Rearrange equation (1) for $n$ as follows:

$n=\frac{PV}{RT}$        (2)

The formula to calculate number of moles is as follows:

$n=\frac{\text{weight}\left(m\right)}{\text{molecular}\text{weight}\left(M\right)}$        (3)

Conversion factor to convert $\text{torr}$ to $\text{atm}$ is as follows:

$\text{760}\text{mmHg}=\text{1}\text{atm}$

Conversion factor to convert $\text{mL}$ to $\text{L}$ is as follows:

$1\text{mL}={10}^{-3}\text{L}$

The conversion factor to convert $°\text{C}$ to Kelvin is as follows:

$T\left(\text{K}\right)=T\left(\text{°C}\right)+273.15$        (4)