5) if i have 10.92 moles of gas at a temperature of 67.54 ⁰c, and a volume of 88.89 liters, what is the…

5) if i have 10.92 moles of gas at a temperature of 67.54 ⁰c, and a volume of 88.89 liters, what is the pressure of the gas? ____ sig figs in answer. p = nrt / v

5) if i have 10.92 moles of gas at a temperature of 67.54 ⁰c, and a volume of 88.89 liters, what is the pressure of the gas? ____ sig figs in answer. p = nrt / v

Answer

Explanation:

Step1: Convert temperature to Kelvin

$T = 67.54 + 273.15=340.69\ K$

Step2: Identify the gas - constant value

The ideal gas constant $R = 0.0821\ L\cdot atm/(mol\cdot K)$

Step3: Substitute values into the ideal gas law formula

$P=\frac{nRT}{V}$, where $n = 10.92\ mol$, $R = 0.0821\ L\cdot atm/(mol\cdot K)$, $T = 340.69\ K$, and $V = 88.89\ L$ $P=\frac{10.92\times0.0821\times340.69}{88.89}$ $P=\frac{10.92\times28.060649}{88.89}$ $P=\frac{306.422287}{88.89}$ $P = 3.44\ atm$ (3 significant - figures)

Answer:

$3.44\ atm$