2) if i have an unknown quantity of gas at a pressure of 4.1 atm, a volume of 31 liters, and a temperature…

2) if i have an unknown quantity of gas at a pressure of 4.1 atm, a volume of 31 liters, and a temperature of 87 ⁰c, how many moles of gas do i have? ____ sig figs in answer.

2) if i have an unknown quantity of gas at a pressure of 4.1 atm, a volume of 31 liters, and a temperature of 87 ⁰c, how many moles of gas do i have? ____ sig figs in answer.

Answer

Explanation:

Step1: Convert temperature to Kelvin

$T = 87 + 273.15=360.15\ K$

Step2: Use the ideal - gas law

The ideal - gas law is $PV = nRT$, where $P = 4.1\ atm$, $V = 31\ L$, $R=0.0821\ L\cdot atm/(mol\cdot K)$, and $T = 360.15\ K$. We need to solve for $n$. Rearranging the ideal - gas law for $n$ gives $n=\frac{PV}{RT}$.

Step3: Substitute values

$n=\frac{4.1\ atm\times31\ L}{0.0821\ L\cdot atm/(mol\cdot K)\times360.15\ K}$ $n=\frac{127.1\ L\cdot atm}{29.568315\ L\cdot atm/mol}\approx4.3\ mol$

Answer:

$4.3$