If 5400. Joules of energy were supplied to 4.5 grams of ice at - 10 degree Celsius, how many grams of what phases would you have?

The answers to you questions are 3,66 g of liquid water and 0,84 g of vapor.

Solution:1) Q₁ = mxCxΔT = 4,5 g x 2,108 J/°C x g x 10°C.

= 97,86 J heat required to warm the ice to 0°C.

2) = 4,5 g x 334 J/g. = 1503 J heat required to melt the ice to water at 0°C.

3) = 4,5 g x 4,184 J/°C x g x 100°C

= 1882,28 J heat required to warm the water from 0°C to 100°C. = 5400 J - 3483,14 J = 1916,86 J heat left to vaporize the water.

mass of the vapor = 1916,86 J : 2257 J/g

= 0,84 g.

Answer is: 3,66 g of liquid water and 0,84 g of vapor.

1) Q₁ = m·C·ΔT

Q₁ = 4,5 g · 2,108 J/°C·g · 10°C.

Q₁ = 97,86 J heat required to warm the ice to 0°C.

2) Q₂ = 4,5 g · 334 J/g.

Q₂ = 1503 J heat required to melt the ice to water at 0°C.

3) Q₃ = 4,5 g · 4,184 J/°C·g · 100°C

Q₃ = 1882,28 J heat required to warm the water from 0°C to 100°C.

Q₄ = 5400 J - 3483,14 J = 1916,86 J heat left to vapourize the water.

m (vapor) = 1916,86 J : 2257 J/g = 0,84 g.