Which numerical setup can be used to calculate the heat energy required to completely melt 100. grams of h2o(s) at 0°c?

1.(100. g)(334 j/g)

The heat required to melt 100g of ice is 33.4 KJ.

The latent heat is the heat required to break the inter-molecular interactions in a substance as it is converted from one phase to another. Latent heat does not lead to rise in temperature. The temperature of the substance remains steady during phase transition. The latent heat of fusion of ice is the heat required to convert 1 g of solid ice to liquid.

Given that we have;

Mass of ice = 100g

Latent heat of fusion of ice = 334 Joules/g

H = mL

Where;

m = mass of ice

L = latent heat of fusion of ice

Substituting the values we have;

H = 100g × 334 J/g

H = 33400 J or 33.4 KJ

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1.(100. g)(334 J/g)

We are given;

We are required to identify the numerical setup that will give the energy required to melt 100 g of ice at 0°

Q = mass × latent heat of fusion

In this case;

The latent heat of fusion of water is 334 Joules/g

Therefore;

Heat absorbed, Q = 100 g × 334 J/g

                              = (100 g)(334J/g)

Thus, the appropriate numerical setup to calculate the heat absorbed is (100 g)(334J/g)

the formula mass of a molecule or a compound is the sum of the atomic weights of the atoms in its empirical formula

(that's what i know about formula mass)