Question

solve the following problem:
what is the volume of a balloon if it contains 3.2 moles of helium at a temperature of 20°c and 1.2 atm?

Explanation:

Step1: Convert temperature to Kelvin

$$T = 20 + 273=293\space K$$

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

We know \(n = 3.2\space mol\), \(P=1.2\space atm\), \(R = 0.0821\space L\cdot atm/(mol\cdot K)\), \(T = 293\space K\). Rearrange for \(V\):
$$V=\frac{nRT}{P}$$

Step3: Substitute values

$$V=\frac{3.2\times0.0821\times293}{1.2}$$
$$V=\frac{3.2\times24.0553}{1.2}$$
$$V=\frac{76.97696}{1.2}\approx64.15\space L$$

Answer:

64.15 L