Question

What is the mass of 22.4L of H2 at stp

Answer 1

The mass of 22.4 L of H2 at STP is 2 g.

Step-by-step explanation:

The mass of 22.4 L of H2 at STP can be calculated by using the molar mass of H2 and the molar volume at STP.

First, we determine the moles of H2 by using the molar volume of gas at STP, which is 22.4 L/mol. Since 22.4 L is equal to 1 mol, we can say:

1 mol H2 = 22.4 L H2

Then, we can use the molar mass of H2, which is 2 g/mol, to convert moles of H2 to mass:

1 mol H2 = 2 g H2

Therefore, the mass of 22.4 L of H2 at STP is 2 g.

Answer 2

2.02 g H₂

General Formulas and Concepts:

Chemistry - Atomic Structure

• Reading a Periodic Table
• Using Dimensional Analysis
• STP (Standard Conditions for Temperature and Pressure) = 22.4 L per mole at 1 atm, 273 K

Step-by-step explanation:

Step 1: Define

22.4 L H₂ at STP

Step 2: Identify Conversions

STP - 22.4 L / mol

Molar Mass of H - 1.01 g/mol

Molar Mass of H₂ - 2(1.01) = 2.02 g/mol

Step 3: Convert

`22.4 \ L \ H_2((1 \ mol \ H_2)/(22.4 \ L \ H_2) )((2.02 \ g \ H_2)/(1 \ mol \ H_2) )` = 2.02 g H₂