A sample containing 4.8 g of O2 gas has a volume of 15.0L. Pressure and temperature remain constant.
What is the volume after 4.00g of He is added to the 4.8g of O2 gas in the container
Why can't you do this the same way you did the "0.5 mol gas added to 4.8 g O2 gas"?
To find the final volume after adding 4.00 g of He to the 4.8 g of O2 gas, we need to use the concept of the ideal gas law. According to the ideal gas law, the relationship between pressure (P), volume (V), number of moles (n), and temperature (T) of a gas is given by the equation PV = nRT, where R is the gas constant.
First, we need to determine the number of moles of O2 gas present in the initial sample.
1. Calculate the number of moles of O2 gas (n1) using the formula:
n1 = mass/molar mass = 4.8 g / (32.00 g/mol) = 0.15 mol
Now, let's calculate the number of moles of He added to the container.
2. Calculate the number of moles of He (n2) using the formula:
n2 = mass/molar mass = 4.00 g / (4.00 g/mol) = 1.00 mol
Next, we will calculate the total number of moles (ntotal) of gas present in the container after adding He.
3. Calculate the total number of moles (ntotal) using the formula:
ntotal = n1 + n2 = 0.15 mol + 1.00 mol = 1.15 mol
Finally, we can use the ideal gas law to find the final volume (V2) with the new quantity of gas:
4. Rearrange the ideal gas law equation to solve for V2:
V2 = (n1 * V1) / ntotal
V2 = (0.15 mol * 15.0 L) / 1.15 mol = 1.957 L
Therefore, the final volume of the gas mixture after adding 4.00 g of He to the 4.8 g of O2 gas is approximately 1.957 L.