Question

at what temperature (in kelvin) would 4.0 moles of hydrogen gas in a 100 liter container exert a pressure of 1.00 atmospheres?

Explanation:

Step1: Use the ideal gas law

The ideal gas law is \(PV = nRT\), where \(P\) is pressure (in atm), \(V\) is volume (in liters), \(n\) is the number of moles, \(R\) is the ideal gas constant (\(R=0.0821\space L\cdot atm/(mol\cdot K)\)), and \(T\) is temperature (in Kelvin). We need to solve for \(T\), so we can re - arrange the formula to \(T=\frac{PV}{nR}\).
Given \(n = 4.0\space mol\), \(V=100\space L\), \(P = 1.00\space atm\), and \(R = 0.0821\space L\cdot atm/(mol\cdot K)\).

Step2: Substitute the values into the formula

Substitute the values into \(T=\frac{PV}{nR}\):

$$
LATEXBLOCK0
$$

Answer:

\(304.5\space K\)