A mixture of 8.95 g of Cl2 and 18.0 g of NO2 and an undetermined amount of SO2 occupies a volume of 22.4 liters at 760 mm Hg and 0 C. How many moles of SO2 are present? I keep coming up with 62 and that is not right. Someone please help!!
I responded to your note about the 62; if you will post your work I will find the error. I told you that you should come up with n = 1 for total mols.
To calculate the number of moles of SO2 present in the mixture, we first need to find the number of moles of each gas individually.
1. Calculate the number of moles of Cl2:
Given that the molar mass of Cl2 is approximately 70.90 g/mol, we can use the formula:
moles = mass / molar mass = 8.95 g / 70.90 g/mol
2. Calculate the number of moles of NO2:
Given that the molar mass of NO2 is approximately 46.01 g/mol, we can use the formula:
moles = mass / molar mass = 18.0 g / 46.01 g/mol
Next, we need to calculate the moles of SO2. To do this, we will use the ideal gas law equation, PV = nRT, where:
P = pressure (760 mm Hg)
V = volume (22.4 liters)
n = moles of gas
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (0 degrees Celsius + 273.15 = 273.15 K)
3. Calculate the number of moles of SO2 using the ideal gas law:
n = (PV) / (RT) = (760 mm Hg * 22.4 L) / (0.0821 L·atm/mol·K * 273.15 K)
= (760 mm Hg * 22.4 L) / (22.414 L·atm/mol·K)
= 760/22.414 mol
Now, to find the moles of SO2 present in the mixture, we subtract the sum of the moles of Cl2 and NO2 from the total moles calculated above.
4. Calculate the moles of SO2:
moles of SO2 = total moles - moles of Cl2 - moles of NO2
Substituting the values we calculated:
moles of SO2 = 760/22.414 mol - moles of Cl2 - moles of NO2
After calculating the moles of Cl2 and NO2 in steps 1 and 2, we can substitute those values and calculate the final answer.