Salt compounds are commonly used to melt ice that forms on sidewalks in the winter. A common chemical that is used to melt sidewalk ice is calcium chloride, CaCl2(s). When calcium chloride dissolves into solution is releases thermal energy which aides in melting the ice.

The molar mass of water is 18.02 g/mol

The thermal energy, in kilojoules (kJ) that must be released from the calcium chloride,
CaCl2(s), to melt 10.0 kg of ice, expressed in scientific notation is a. bc x 104 k).
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The values of a, b, c, and d.

The values of a, b, c and d are

a = 3, b = 3, c = 4 and d = 3

Explanation:

The quantity of heat needed to melt the ice is given by Q = mL where m = mass of ice and L = latent heat of fusion of ice = 334 kJ/kg. This quanity of heat is also the thermal energy needed to be released by the calcium chloride, CaCl₂

Now, the mass of ice = 10 kg. So,

Q = mL

Q = 10 kg × 334 kJ/kg

Q = 3340 kJ

In scientific notation,

Q = 3.34 × 10³ kJ

So the thermal energy needed to be released by the calcium chloride is 3.34 × 10³ kJ

Comparing Q = 3.34 × 10³ kJ with a.bc × kJ

So, a = 3, b = 3, c = 4 and d = 3

The values of a, b, c and d are

a = 3, b = 3, c = 4 and d = 3

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