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Alenkinab [10]
3 years ago
10

How much heat is required to melt 26.0 g of ice at its melting point?

Chemistry
1 answer:
MAXImum [283]3 years ago
8 0

Answer:

Heat required to melt 26.0 g of ice at its melting point is 8.66 kJ.

Explanation:

Number of moles of water in 26 g of water: 26× \frac{1}{18.02} moles

                                                                      =1.44 moles

The enthalpy change for melting ice is called the entlaphy of fusion. Its value is 6.02 kj/mol.

we have relation as:

                                           q = n × ΔH

where:

q  = heat

n  = moles

Δ H  = enthalpy

So calculating we get,

                                        q= 1.44*6.02 kJ

                                        q= 8.66 kJ

We require 8.66 kJ of energy to melt 26g of ice.

                       

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Answer:

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Explanation:

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The unit of mass is 'Kilogram' which is written as 'kg' and volume, v = 10 L.

<h3>Equation :</h3>

To calculate the volume

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volume = mass / density

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<h3>What is density mass?</h3>

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I understand the question you are looking for :

If you have a density of 100 kg/L, and a mass of 1000 units, tell me the following: First what are the mass units? Secondly, what is the volume?

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