If 3.25 g N2 gas is introduced into an evacuated 1.50 L flask at 325 K, what is the pressure inside the flask (in atm)?

2.06 atm

Explanation:

The computation of the pressure inside the flask is shown below;

As per the ideal gas law

we know that

P V = nRT

where

V = 1.50L

T = 325 K

R = 0.0821

Now moles of N_2 is

= 3.25 ÷ 28

= 0.116 mol

Now

P = NRT ÷ V

= 0.116 × 0.0821 × 325 ÷ 1.50

= 2.06 atm

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%

a compound is a molecule made of atoms from different elements.

a. by the combination of an unlimited number of elements