SO2 (5.00g) and CO2 (5.00g) are places in a 750.9ml container at 50.0 the partial pressure of SO2 in a container was...?

I assume 50.0 means 50.0celsius temeprature.

mols SO2 = grams/molar mass = ?
mols CO2 = grams/molar mass = ?
pressure SO2 use pv = nRT with T = 273+50 = ?
pressure CO2 use pv = nRT as above.
Total pressure = pSO2 + pCO2 = ?

Post your work if you get stuck.

To find the partial pressure of SO2 in the container, we first need to calculate the moles of SO2 and CO2 present in the container. Then, we can use the Ideal Gas Law to find the partial pressure.

Step 1: Calculate the moles of SO2 and CO2.
To calculate the moles, we need to divide the given mass of each gas by its molar mass.

The molar mass of SO2 (sulfur dioxide) is:
S = 32.07 g/mol
O = 16.00 g/mol
So, the molar mass of SO2 = 32.07 + (2 x 16.00) = 64.07 g/mol

Moles of SO2 = Mass of SO2 / Molar mass of SO2
Moles of SO2 = 5.00 g / 64.07 g/mol

Similarly, we can calculate the moles of CO2.

The molar mass of CO2 (carbon dioxide) is:
C = 12.01 g/mol
O = 16.00 g/mol
So, the molar mass of CO2 = 12.01 + (2 x 16.00) = 44.01 g/mol

Moles of CO2 = Mass of CO2 / Molar mass of CO2
Moles of CO2 = 5.00 g / 44.01 g/mol

Step 2: Calculate the total moles of gas.
To find the total moles of gas, we add the moles of SO2 and CO2 together.

Total moles of gas = Moles of SO2 + Moles of CO2

Step 3: Calculate the partial pressure of SO2.
The Ideal Gas Law equation is:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/(mol·K)), and T is the temperature in Kelvin.

In this case, we are interested in the partial pressure of SO2, so we can rearrange the equation to solve for P:

P(SO2) = (n(SO2) / n(total)) * P(total)

where P(SO2) is the partial pressure of SO2, n(SO2) is the moles of SO2, n(total) is the total moles of gas, and P(total) is the total pressure.

Since the problem does not provide the total pressure, we cannot directly calculate the partial pressure of SO2.

Please provide the total pressure in atm.