What pressure will be exerted by each of the gases in the following mixture if the total pressure of the mixture amounts to 768.8 torr? 0.500 g of hydrogen; 0.245 g of oxygen; 0.335 g of nitrogen.
What do I need to do??
To find the pressure exerted by each gas in the mixture, you need to use the concept of partial pressures.
Here's what you need to do step-by-step:
1. Convert the masses of each gas to moles using their molar masses. The molar mass of hydrogen (H2) is 2 g/mol, oxygen (O2) is 32 g/mol, and nitrogen (N2) is 28 g/mol.
Moles of hydrogen (H2) = 0.500 g / 2 g/mol
Moles of oxygen (O2) = 0.245 g / 32 g/mol
Moles of nitrogen (N2) = 0.335 g / 28 g/mol
2. Use the ideal gas law, PV = nRT, to calculate the partial pressure of each gas. Since all the gases are at the same temperature and volume, we can assume that the moles (n) and the volume (V) are the same for each gas.
Partial pressure of hydrogen (PH2) = Moles of hydrogen (H2) / Total moles of all gases x Total pressure
Partial pressure of oxygen (PO2) = Moles of oxygen (O2) / Total moles of all gases x Total pressure
Partial pressure of nitrogen (PN2) = Moles of nitrogen (N2) / Total moles of all gases x Total pressure
3. Substitute the calculated values and solve for each partial pressure.
Let's proceed with the calculations: