Builders and dentists must store plaster of Paris, CaSO4 x 1/2 H2O, in airtight containers to prevent it from
absorbing water vapor from the air and changing to
gypsum, CaSO4 x 2H2O How many liters of water
vapor evolve when 2.00 kg of gypsum are heated at
110°C to produce plaster of Paris? At 110°C, the
density of water vapor is 0.574 g/L.

547 L of water vapour

Explanation:

Equation of reaction: 2[CaSO4.2H20] + Heat ---> 2[CaSO4.½H2O] + 3H20

From the equation of reaction above, 2 moles of gypsum when heated produces 2 moles of plaster of Paris and 3 moles of water vapour.

Molar mass of gypsum = 172 g/mol

Molar mass of H2O = 18 g/mol

Therefore, 2 * 172 g of gypsum produces 3 * 18 g of water vapour

i.e. 344 g of gypsum produces 54 g of H2O

2 Kg(2000 g) of gypsum will produce (54 * 2000)/344 g of water vapour = 313.95 of water vapour.

Volume of water vapour produced = mass/density

Volume of water vapour = 313.95 g/ 0.574 g/L = 547 L of water vapour

Therefore 547 L of water vapour are produced

1. a)c-14 has two more protons

2. d)they have different numbers of protons, neutrons, and valence electrons; they are all gases at room temperature.

3. c) iron and nickel.