Question

How many Jolie’s are required for melting 12.8 g of ice at 0 degree Celsius

Answer 1

Answer: The amount of heat required for melting of ice is 4277 J

Step-by-step explanation:

The chemical equation for the phase change of ice follows:

`H_2O(s)(0^oC)\rightleftharpoons H_2O(l)(0^oC)`

To calculate the amount of heat required to melt the ice at its melting point, we use the equation:

`q=m* \Delta H_(fusion)`

where,

`q` = amount of heat absorbed = ?

m = mass of ice = 12.8 g

`\Delta H_(fusion)` = enthalpy change for fusion = 334.16 J/g

Putting all the values in above equation, we get:

`q=12.8g* 334.16J/g=4277J`

Hence, the amount of heat required for melting of ice is 4277 J

Answer 2

It takes 4,270 Joules of energy to melt 12.8 grams of ice at 0 °C.

Explanation

The enthalpy change for melting ice is called the enthalpy of fusion. Its value is 6.02 kJ/mol. This means for every mole of melting ice, we must apply 6.02 kJ of heat. We can calculate the heat needed with the following equation:

`q = n * ΔH`

`Δ` = Δ

where:

q = heat

n = moles (0.71 mole = 12.8 g water)

ΔH = enthalpy (for water at 0 temperature is 6.02)

This problem can be broken into three steps:

1. Calculate moles of water

2. Multiply by the enthalpy of fusion

3. Convert kJ to J

`q = 0.71 * 6.02`

`q = 4.27 kJ`

`IkJ = 1000J`

`q = 4270J`