In the chamber below, the volume is 20.5 L. What would the volume be if the temperature is increased to 500 K, the moles are reduced to 0.5, and the pressure is increased to 2.0 atm? A.) 10.25 L
B.) 20.5 L
C.) 41.0 L
D.) 61.5 L

C. bc I ssid

Explanation:

0+0+0+0+0+0=00

10.25L

Explanation:

Doubling the temperature would double the volume while halving the number of moles would decrease the volume by half, so the changes produced by these two variables cancel each other out. Since pressure and volume are inversely proportional, doubling the pressure will cut the volume in half, reducing it from 20.5 to 10.25 L.

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%