00:01
This question asks us to find the molecular mass of the gas formed by the reaction.
00:07
We are given the conditions of standard temperature and pressure, which is 273 kelvin and 1 atm.
00:17
And then we are told that the gas collected is 1 liter and 1 .52 grams.
00:24
So we are going to use the ideal gas law equation.
00:29
And since we are looking for the molecular mass and not the number of moles, which is n, we're going to call m grams per mole the molecular mass, and that's what we're looking for.
00:46
So when we plug in n into our equation, we're going to call n 1 .52 moles over m.
00:58
So taking everything we have here, we're going to pull.
01:03
I'll get into our equation and it's going to look like this.
01:27
And then remember we're going to use our gas constant in the units of liters times atm, since our pressure is in atm...