Question

use the references to access important values if needed for this question.
a 1.24 mol sample of neon gas at a temperature of 14.0 °c is found to occupy a volume of 25.1 liters. the pressure of this gas sample is
mm
hg.
submit answer
try another version
3 item attempts remaining

Explanation:

Step1: Convert temperature to Kelvin

The formula to convert Celsius to Kelvin is \(T(K)=T(^{\circ}C)+273.15\). Given \(T = 14.0^{\circ}C\), then \(T=(14.0 + 273.15)K=287.15K\).

Step2: Use the ideal gas law \(PV = nRT\)

We need to find \(P\). Rearranging the ideal gas law for \(P\) gives \(P=\frac{nRT}{V}\).
The value of \(R\) (gas constant) is \(62.36L\cdot mmHg\cdot mol^{-1}\cdot K^{-1}\), \(n = 1.24mol\), \(V=25.1L\), and \(T = 287.15K\).
Substitute the values into the formula:

$$
LATEXBLOCK0
$$

First, calculate the numerator: \(1.24\times62.36\times287.15=(1.24\times62.36)\times287.15 = 77.3264\times287.15\approx22200\) (approximate intermediate calculation).
Then divide by \(V = 25.1L\): \(P=\frac{22200}{25.1}\approx884mmHg\)

Answer:

\(884mmHg\)