Question

What volume would 20.0 moles of sulfur dioxide occupy at 75.3 °C
with a pressure of 5.18 atm?

Answer 1

To find the volume occupied by 20.0 moles of sulfur dioxide at 75.3 °C and 5.18 atm, use the Ideal Gas Law. After converting the temperature to Kelvin, the calculated volume is approximately 1110.76 liters.

Step-by-step explanation:

To determine the volume occupied by 20.0 moles of sulfur dioxide at 75.3 °C with a pressure of 5.18 atm, we can use the Ideal Gas Law, which is expressed as PV=nRT. Here, P is the pressure, V is the volume, n is the number of moles of the gas, R is the universal gas constant (0.0821 L·atm/(mol·K)), and T is the temperature in Kelvin.

First, convert the temperature from Celsius to Kelvin: T(K) = 75.3 °C + 273.15 = 348.45 K.

Then, plug in the known values into the Ideal Gas Law equation:

V = \( \frac{nRT}{P} \)

V = \( \frac{20.0 \text{moles} \times 0.0821 \frac{{L\cdot atm}}{{mol\cdot K}} \times 348.45 K}{5.18 atm} \)

Now, we calculate the volume V:

V = \( \frac{20.0 \times 0.0821 \times 348.45}{5.18} \) L

V = 1110.76 L

The volume occupied by 20.0 moles of sulfur dioxide under the given conditions is approximately 1110.76 liters.