Question c4095

Apr 4, 2015

You have $\text{1.3 moles}$ of gas in that volume, under those conditions of pressure and temperature.

To solve this problem, all you have to do is apply the ideal gas law equation, $P V = n R T$, and solve for $n$, the number of moles of gas.

One thing to keep in mind is that you must convert the temperature from degrees Celsius to Kelvin in order to get the correct result.

So, plug in your values into the equation and solve for $n$

$P V = n R T \implies n = \frac{P V}{R T}$

n_("gas") = (1.2cancel("atm") * 31cancel("L"))/(0.082(cancel("atm") * cancel("L"))/("mol" * cancel("K")) * (273.15 + 87)cancel("K")) = "1.2596 moles"#

Rounded to two sig figs, the number of sig figs given for all your values, the answer will be

${n}_{\text{gas") = color(green)("1.3 moles}}$