Asample of hydrogen gas at a temperature of 275 k and a pressure of 0.456 atm is allowed to expand to a pressure of 845 mmhg. what is the new temperature of the gas?

P₁/T₁ = P₂/T₂

P₁ = 0.456 atm

T₁ = 275 K

P₂ = 845 mmHg = 1.112 atm

T₂ = ?

By applying the formula,
0.456 atm / 275 K = 1.112 atm / T₂                  

                   T₂  = (1.112 atm / 0.456 atm) x 275 K
                   T₂  = 670.6 K

Hence, the temperature of the hydrogen gas is 670.6 K

- decrease the number of plants and animals living in the water.

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%