equal masses of so2 and o2 are kept in a vessel at 27 degrees celcius. the total pressure of the mixture is 2.1atm. the partial pressure of so2 is
0.7 atm
Make up masses--any convenient number will work.
mols SO2 = grams/molar mass = ?
mols O2 = grams/molar mass = ?
Total mols = ?
XSO2 = mols SO2/total mols.
Then pSO2 = XSO2*Ptotal
To find the partial pressure of SO2 in the mixture, we need to use the concept of Dalton's law of partial pressures. According to Dalton's law, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of each gas present.
In this case, the total pressure of the mixture is given as 2.1 atm. Since the masses of SO2 and O2 are equal, we can assume that they have the same number of moles. Therefore, the partial pressure of SO2 (P_SO2) will be half of the total pressure.
Step 1: Find the partial pressure of SO2.
P_SO2 = (Total Pressure) / 2
P_SO2 = 2.1 atm / 2
P_SO2 = 1.05 atm
Therefore, the partial pressure of SO2 in the mixture is 1.05 atm.
How 0.7
Pso2=xsomultiply ptotal
Ptotal=2.1atmwso2=wo2xso2=nso2di