What is the mass of 50.0 L of O2(g) at STP?
O is 16g/mole, so O2 is 32g/mole. 50/32 = 1.5625 moles. 1 mole of any gas at stp is 22.4 liters.
1.5625 × 22.4 = 35 liters.
At STP => moles O2 = (50L)/(22.4L/mole) = 2.232 moles O2
2.232 moles O2 = (2.232 mole O2)(32 g/mole) = 71.429 grams O2
do your calculations make sense to you?
you divided the volume of gas by the molar mass ... to get what?
you know the volume (50 L) , and the volume a mole occupies (22.4 L)
so you can find the moles , and use the molar mass to find the total mass
if one mole occupies 22.4 L , how many moles can fit in 50.0 L?
what is the mass of these moles?
25.6
32 g/mol / 22.4 =1.42g/mol
Well, if you were hoping for a clown answer, you're in for a treat! The mass of 50.0 L of O2(g) at STP is... drumroll, please... airy-fairy grams! Just kidding, it's actually 32 grams per mole. So grab your funny math goggles, because 50.0 L of O2(g) would weigh in at approximately 80 grams. And no, that doesn't include the weight of any clown wigs.
To determine the mass of 50.0 L of O2(g) at STP (Standard Temperature and Pressure), we need to follow these steps:
1. Understand the molar mass of O2: The molar mass of oxygen (O) is 16 g/mol. Since O2 consists of two oxygen atoms, the molar mass of O2 is twice that, which gives us 32 g/mol.
2. Calculate the number of moles: Dividing the given volume of 50.0 L by the molar volume of any gas at STP, which is 22.4 L/mol, we can find the number of moles.
Moles of O2 = 50.0 L / 22.4 L/mol = 2.2321 moles (rounding to four decimal places for accuracy)
3. Determine the mass: Now that we have the number of moles, we can calculate the mass. Multiply the number of moles by the molar mass of O2.
Mass of O2 = 2.2321 moles * 32 g/mol = 71.4291 grams (rounding to four decimal places for accuracy)
Therefore, the mass of 50.0 L of O2(g) at STP is approximately 71.4291 grams.