[WilsonXavier]

Consider two containers of equal volumes containing gas subjected to the same conditions of temperature and
pressure. At first, there 30,0g of an "X" gas and the second container, there 3,01x1023 gas molecules "Y".
How many grams of gas "X" in 68,1L measured under normal tempeeratua and pressure?
Data: Vm = 22,7L / mol

[mikasaur]

Hello and welcome to the forums! Before we can help you have to show us your attempts at solving the problem.

What have you done so far? What sort of theories and ideas have you applied to this gas problem?

[WilsonXavier]

the equation of the ideal gas PV = NRT?

[mikasaur]

That's a good one to think about using for gas problems.

Do you know what each of the variables are in the ideal gas law? If we have two containers of equal volumes subject to the same temperature and pressure what can we say about the amount of gas in each container? How do they relate?

[WilsonXavier]

I did not understand the process of solving this problem.

[mikasaur]

Hmm... well...

You have two containers of equal volumes and with the same temperature and pressure. Do you think the amount of gas in each will be different? The same? Let's start with that.

[WilsonXavier]

equal?

[mikasaur]

They would! Because

[itex]PV=nRT[/itex]

[itex]n=\frac{PV}{RT}[/itex]

So if P, V, and T are equal then n would necessarily be the same for both.

Okay, so now you know the "amount" of gas is the same. They've given you a mass of gas in one container and a number of molecules in the second. Where can you go from here?