How much heat energy is required to melt 75g of ice at 0°c? a. 4.45jb. 30.13jc. 169, 500jd. 25, 050j

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

Q = N x ΔH

where:

Q  = heat

N  = moles  

ΔH  = enthalpy

In this problem we would like to calculate the heat needed to melt 35 grams of ice at 0 °C. 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.

Step 1 : Calculate moles of water

Step 2 : Multiply by enthalpy of fusion

Q = N × ΔH  =  [ Step 1 Answer ] ×  6.02 =

Step 3 : Convert kJ to J

Finally rounding to 2 sig figs (since 34°C has two sig figs) we get

Q Would Equal ____

a small container that holds a source of energy a solar cell that captures light energy and converts it into electricity a voltaic cell that uses the oxidation of a fuel to produce electricity

explanation: