A1.92 mol sample of hydrogen gas occupies 22.2 l. how many mol of hydrogen are needed to fill a 102.1 l container at the same pressure and temperature? enter your answer in the provided box. i mol h2

8.83 moles of Hydrogen

Explanation:

We are told that 1.92 moles of H2 occupies 22.2 L at a certain pressure and temperature, and we are asked to calculate the quantity of moles of H2 are necessary to fill a container of 102.1 L. So, if the pressure and temperature are constant, then the equality expressed before 1.92 H2 moles = 22.2 L maintains. Therefore, we can calculate what is being asked as follows:

22.2 L 1.92 H2 moles

102.1 L x = (102.1 L × 1.92 H2 moles)/22.2 L = 8.83 H2 moles

This means that 8.83 H2 moles are necessary to fill a 102.1 L container at a certain pressure and temperature.

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%