Question

. How much volume would 2.00 moles of gas take up, under standard temperature and pressure conditions?

11.2 L
22.4 L
33.6 L
44.8 L

Answer 1

Use the ideal gas law

Answer 2

what's that?

Answer 3

PV = nRT...you have not seen this equation for gases?

Answer 4

ohh yes i have but idk how to use it

Answer 5

You need to solve for volume , so the first thing to do is rearrange the equation for V....can you do that for me?

Answer 6

V=nRT/P ?

Answer 7

Good

Answer 8

now you need values for n, R ,T and P

n is the number of moles of gas (given in the problem)
R is the ideal gas constant (you probably have the value in your notes)
Now they say..."standard temperature and pressure"...
if you google standard temperature and pressure for gases you can see what those values are.
Then substitute into your equation and solve for V

Answer 9

I'm so confused because I'm looking back in my notes and didn't learn any of this

Answer 10

no problem....see if you can find the values for R, P and T for this problem and include their units

Answer 11

I can't find it anywhere

Answer 12

hang on...
http://en.wikipedia.org/wiki/Gas_constant
http://chemistry.about.com/od/chemistryglossary/a/stpdefinition.htm

Answer 13

Their are different values for R depending on the units in the problem...
you will need R = .0821 l.atm/(mol.K)

Answer 14

1 mole of gas at STP occupies 22.4 liters

Answer 15

22.4 L X 2 = 44.8 L why we need to use ideal gas law for this easy question ?