A 2.375-g sample of impure Mn2(CO3)5 is decomposed with heat. 64.33 mL of CO2 is collected over water at a temperature of 40.00oC. The gas is collected at an atmospheric pressure of 755 torr. Water has a vapor pressure of 37 torr at 40.00oC. What is the % Mn2(CO3)5 in the original impure sample? Mn2(CO3)5 → Mn2O5 + 5 CO2

201cm/s÷5: 18

explanation:

there is no explanation

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%

so she was walking and she stepped on warm jeffy , uh uh uhh dadye i just pooped my pants