Question

A glass container was initially charged with 1.60 moles of a gas sample at 4.75 atm and 21.7 °C. Some of the gas was released as the temperature was increased to 32.1 °C, so the final pressure in the container was reduced to 1.40 atm. How many moles of the gas sample are present at the end?

Answer 1

The number of moles of a gas sample after a pressure and temperature change can be determined using the combined gas law, rearranging the equation for the final number of moles, and making sure to convert temperatures to Kelvin.

Step-by-step explanation:

To determine how many moles of a gas sample are present at the end after adjusting the pressure and temperature, we use the ideal gas law given by 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.

We know the initial conditions (P1, n1, T1) and the final conditions (P2, T2), but the volume does not change. Instead, some of the gas is released, and we need to find the final number of moles (n2). Since the volume and R are constant, we use the combined gas law, which is (P1 * n1)/T1 = (P2 * n2)/T2.

We already know P1, n1, T1, P2, and T2, so we can solve for n2. Remember to convert temperatures to Kelvin by adding 273.15 to the Celsius temperatures. Using these steps, we can calculate the final amount of moles of gas left in the container.