Question

a sample of carbon monoxide gas occupies 3.59 l at 125 0c. at what temperature will the gas occupy a volume of 1.25 l if the pressure remains constant? enter answer oc

Explanation:

Step1: Convert temperature to Kelvin

The initial temperature \(T_1 = 125^{\circ}C\). Convert to Kelvin: \(T_1=(125 + 273.15)K=398.15K\).
We use Charles's law \(V_1/T_1 = V_2/T_2\) (since pressure is constant). Given \(V_1 = 3.59L\), \(V_2=1.25L\), and we need to find \(T_2\).
From \(T_2=\frac{V_2T_1}{V_1}\)

Step2: Substitute values

Substitute \(V_1 = 3.59L\), \(T_1 = 398.15K\), \(V_2 = 1.25L\) into the formula:
\(T_2=\frac{1.25\times398.15}{3.59}\)
\(T_2=\frac{497.6875}{3.59}\approx138.63K\)

Step3: Convert back to Celsius

\(t=(T_2 - 273.15)^{\circ}C=(138.63-273.15)^{\circ}C=- 134.52^{\circ}C\)

Answer:

\(-134.5^{\circ}C\) (rounded to one - decimal place)