Two sealed tanks each contains gas at 273 K. Tank A contains 9.00 g of argon gas, and tank B contains 18.7 g of chlorine gas. How many moles of gas are in each tank?
How would I start this problem
Argon is 40 grams / mol
so how many mols is 9 grams ?
Now watch out Chlorine Gas is Cl2
so 35.5*2 = 70 grams / mol
I mean 71 :)
So do I just do 9/40
and then do 18.7/70
Yes, but following the typo pointed out by Anonymous, that would be 71 and not 70 :-)
Got it thanks
To solve this problem, you need to use the ideal gas law, which relates the pressure (P), volume (V), temperature (T), and number of moles (n) of a gas. The ideal gas law is given by the equation PV = nRT, where R is the ideal gas constant.
To find the number of moles of gas in each tank, you need to rearrange the ideal gas law equation to solve for n. The equation becomes n = PV / RT.
First, you need to determine the pressure, volume, and temperature for each tank. The problem doesn't provide this information, so let's assume that both tanks have the same conditions.
Next, you need to convert the given masses of argon gas and chlorine gas into moles. To do this, you divide the mass by the molar mass of each gas.
The molar mass of argon (Ar) is 39.95 g/mol, so to find the number of moles of argon gas in Tank A, you divide the mass of argon gas (9.00 g) by the molar mass of argon gas:
n(Ar) = mass(Ar) / molar mass(Ar)
= 9.00 g / 39.95 g/mol
Similarly, the molar mass of chlorine (Cl) is 35.45 g/mol, so to find the number of moles of chlorine gas in Tank B, you divide the mass of chlorine gas (18.7 g) by the molar mass of chlorine gas:
n(Cl) = mass(Cl) / molar mass(Cl)
= 18.7 g / 35.45 g/mol
After performing these calculations, you will have the number of moles of gas in each tank.