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5.75g of SO2Cl2 was placed in a 2.00L flask. What is the molarity of the gas and other questions

4) a quantity of 5.75g of SO2Cl2 was placed in a 2.00L flask. What is the molarity of the gas?

5) how many grams of potassium chlorate decompose to potassium chloride and 587mL of O2 at 128 degrees celsius and 752 torr?

Molarity = moles per liter

To get the moles from grams, you need to use the molar mass.
Which can be achieved by either being given it, using the internet in this case, or a periodic table and adding up the masses of each.

I'll just use the internet, but a professor may want you to use the periodic table he/she gives you. But, I'm lazy and don't feel like adding, but the values will be almost identical either way.

Molar mass of SO2Cl2 = 134.9698 g/mol

So to achieve the moles of SO2Cl2, you need to convert.

you have 5.75 grams of SO2Cl2 so multiply that by the molar mass of it, 134.9698 g/mol. But, since you NEED MOLES, flip it so that the grams will cancel and leave you with moles.

5.75 g x 1mol/134.9698g = 0.043 moles of SO2Cl2

So, now by definition Molarity = moles/L

You have 2.00 L.

So:

0.043 moles/ 2.00 L = 0.0215 M

For the 2nd one, I would say use the Ideal Gas Law

PV=nRT

P = Pressure
V= Volume
n = number of moles
R = Rate Constant
T = Temp.




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