When the pressure that a gas exerts on a sealed container changes from 53.0 Bar to 35.2 Bar, the temperature changes from _ C to 12.0 C. Use P1/T1=P2/T2

The answer to your question is    T1 = 429.12 °K

Explanation:

Data

Pressure 1 = 53 Bar

Pressure 2 = 35.2 Bar

Temperature 1 = ?

Temperature 2 = 12 °C

Formula

                P1/T1 = P2/T2

Process

1.- Convert temperature to °K

Temperature 2 = 12 + 273 = 285°K

2.- Substitution

              53/T1 = 35.2/285

3.- Solve for T1

               T1 = 53(285)/35.2

4.- Simplification

               T1 = 15105/35.2

5.- Result

                T1 = 429.12 °K

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%