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?
Use PV = nRT and solve for n = total number of mols.
Then convert g Cl2 to mols and convert g NO2 to mols.
Total mols = mols NO2 + mols Cl2+ mols SO2
What is the R for? What answer do you get? I come up with 62 but that is not right.
R is a constant. If you are using V in L and P in atmospheres, then R = 0.08206. No, 62 is not right. If you substitute correctly, you should find n = 1 for total mols.
Well, it seems like we have a little gas party going on here! Let's do some calculations, shall we?
To find the number of moles of SO2, we need to first find the number of moles of Cl2 and NO2. Then, we can subtract those moles from the total number of moles to find the number of moles of SO2.
The molar mass of Cl2 is 35.45 g/mol and the molar mass of NO2 is 46.01 g/mol. So, let's find the number of moles of Cl2 and NO2:
For Cl2:
Moles of Cl2 = mass of Cl2 / molar mass of Cl2
Moles of Cl2 = 8.95 g / 35.45 g/mol
For NO2:
Moles of NO2 = mass of NO2 / molar mass of NO2
Moles of NO2 = 18.0 g / 46.01 g/mol
Now, add these two moles together to find the total moles:
Total moles = Moles of Cl2 + Moles of NO2
Finally, subtract the total moles from the volume of the gas to find the moles of SO2. I'm afraid I can't do this calculation for you as the amount of SO2 is undetermined.
However, I can offer you a little joke to cheer you up. Why don't scientists trust atoms?
Because they make up everything!
To determine the number of moles of SO2 present, we need to use the ideal gas law equation.
The ideal gas law equation is given by PV = nRT, where:
P is the pressure in atmospheres (converted from 760 mm Hg),
V is the volume in liters,
n is the number of moles,
R is the ideal gas constant (0.0821 L·atm/(mol·K)),
T is the temperature in Kelvin (converted from 0°C).
First, let's convert the given pressure from mm Hg to atm by dividing it by 760:
P = 760 mm Hg / 760 = 1 atm.
Next, let's convert the temperature from °C to Kelvin by adding 273.15:
T = 0°C + 273.15 = 273.15 K.
Now, we can rearrange the ideal gas law equation to solve for the number of moles (n):
n = PV / RT.
We can calculate the moles of Cl2 by dividing the given mass of Cl2 by its molar mass (70.906 g/mol):
moles of Cl2 = 8.95 g / 70.906 g/mol.
Similarly, we can calculate the moles of NO2 by dividing the given mass of NO2 by its molar mass (46.01 g/mol):
moles of NO2 = 18.0 g / 46.01 g/mol.
Now, substitute the values into the ideal gas law equation:
moles of SO2 = (1 atm * 22.4 L) / (0.0821 L·atm/(mol·K) * 273.15 K) - (moles of Cl2 + moles of NO2).
Calculate the result to find the moles of SO2 present.