Ideal Gas Law Problem: What is the volume of gas at a specific temperature and pressure?
How can we calculate the volume of gas based on the Ideal Gas Law?
Given that 1.25 moles of gas is held at a temperature of -4.5°C and a pressure of 1.20 atm, what is the volume of the gas?
Calculating the Volume of Gas:
According to the Ideal Gas Law formula, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (8.31 J/mol·K), and T is the temperature in Kelvin.
First, we need to convert the given temperature of -4.5°C to Kelvin:
T = -4.5°C + 273.15 = 268.65 K
Next, we can plug in the values and solve for V:
V = (nRT)/P = (1.25 moles * 8.31 J/mol·K * 268.65 K) / 1.20 atm = 245.84 L
Therefore, the volume of the gas at that specific temperature and pressure is 245.84 liters.
Explanation:
In this problem, we have been provided with the number of moles of gas, the temperature, and the pressure. By utilizing the Ideal Gas Law formula, we can determine the volume of gas. The first step is to always ensure that the temperature is in Kelvin, as the Ideal Gas Law requires the temperature to be in Kelvin units.
Once we have converted the temperature to Kelvin, we can simply substitute the values into the Ideal Gas Law equation and solve for the volume. In this case, the volume of the gas is calculated to be 245.84 liters.
Understanding how to apply the Ideal Gas Law equation is essential when dealing with gas properties and calculations. By following the steps outlined in this solution, you can efficiently solve similar problems involving gas volumes, pressures, temperatures, and moles.