Final answer:
The volume occupied by 0.75 mol of gas at 35 °C and 2.0 atm pressure is 9.5 L. This is calculated using the Ideal Gas Law, with the temperature converted to Kelvin and the ideal gas constant R = 0.0821 L·atm/mol·K.
Step-by-step explanation:
The student is asking to find the volume that 0.75 mol of an ideal gas occupies at a temperature of 35 °C and a pressure of 2.0 atm. To solve this, we can use the Ideal Gas Law, which is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin.
To begin, we need to convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature. Therefore, 35 °C + 273.15 = 308.15 K.
Next, we will use the ideal gas constant in the units that match the pressure unit atm, which is R = 0.0821 L·atm/mol·K. We can now rearrange the Ideal Gas Law to solve for V: V = nRT/P.
Plugging the values into the equation, we get:
V = (0.75 mol) × (0.0821 L·atm/mol·K) × (308.15 K) / (2.0 atm)
When we calculate this, V = 9.5 L. So the volume occupied by 0.75 mol of gas at 35 °C and 2.0 atm pressure is 9.5 L.