1.78
Answer:
A few useful bits of Argon data:
Rule to remember: One mole of any ideal gas in standard temperature and pressure conditions will occupy 22.4 L. We will need this number for conversion. Work:(1.954 moles Ar) * (22.4 L / 1 moles Ar) = 43.7696 = 43.8 L
1 mole of anything is 22.42 L in volume.
1 mole occupies 22.414 litres at STP
43.8L
This volume is 79,79 litres.
The volume is approx. 15,35 litres.
Molarity = moles of solute/Liters of solutionOr, for our purposes....,Liters of solution (volume) = moles of solute/MolarityVolume (liters) = 0.150 moles HCl/4.00 M HCl= 0.0375 liters = 37.5 milliliters======================
Moles/Liters=Molarity (M) therefore: Molarity*Liters=moles Since you were given milliliters, you must first convert your volume to liters for the equation to be accurate. 2.2M*.065L=moles=.143 moles NaOH
The volume of one mole of gas at a standard temperature and pressure is 22.4 liters. Multiply 22.4 liters by 0.25 moles to get a volume of 5.6 liters.
At STP, 1 mole of gas occupies a volume of 22.4 liters. Thus, 4/5 moles of gas will occupy .8*22.4 liters.
1 mole occupies 22.4 liters. 0.5 moles occupies 11.2 liters at STP.
At standard temperature and pressure, 1 mole of any gas will occupy 22.4 liters. Set up a direct proportion of 22.4 liters/1 mole = 1 liter/x moles and solve for x. You get 0.045 moles.
1 mole occupies 22.414 liters So, 1.84 moles will occupy 41.242 liters
0.25 moles, approx.
1 mole occupies 22.414 liters So, 3.30 moles will occupy 73.966 liters.
1 mole of any gas at STP occupies 22.4 liters. Thus, 2 moles propane will occupy 2 x 22.4 L = 44.8 liters.
This volume is 79,79 litres.
The volume is approx. 15,35 litres.
Number of Moles = concentration * volume (in litres)
First convert the number of grams of CO2 into moles, then use the Ideal Gas Law. For how to solve this problem, see the two Related Questions links to the left of this answer.
Approx. 774 litres.