The molar heat of fusion for water is 6.01 kJ/mol. The heat capacity for water is 75 J/mol deg. Which expression gives the quantity of energy need to change 1.0 mol ice at 0C to liquid water at 25C?

A. 6010/(75x25)
B. 6.01+75
C. 6010+(75x25)
D. 6010/298+(75x25)
E. (6010+(75x25))/298

(mass ice x heat fusion) + (mass H2O x specific heat H2O x delta T) = ?

To calculate the amount of energy needed to change 1.0 mol of ice at 0°C to liquid water at 25°C, you need to consider two processes: the energy required to heat the ice from 0°C to 0°C (melting), and the energy required to heat the liquid water from 0°C to 25°C (heating).

First, let's calculate the energy required for the melting process using the molar heat of fusion. The molar heat of fusion for water is 6.01 kJ/mol. Since you have 1.0 mol of ice, the energy required for the melting process is:

Energy for melting = 6.01 kJ/mol

Next, let's calculate the energy required for the heating process. The heat capacity for water is 75 J/mol·°C. To heat 1.0 mol of water from 0°C to 25°C, the energy required is:

Energy for heating = (75 J/mol·°C) × (25°C - 0°C) = (75 J/mol·°C) × (25°C) = 1875 J/mol

Now, to calculate the total energy required, you need to add the energy for melting and the energy for heating:

Total energy required = Energy for melting + Energy for heating

Plugging in the values:

Total energy required = 6.01 kJ/mol + 1875 J/mol

To make the units consistent, convert kJ to J:

Total energy required = 6010 J/mol + 1875 J/mol

Combining the two terms:

Total energy required = 7885 J/mol

Therefore, the correct expression that gives the quantity of energy needed to change 1.0 mol ice at 0°C to liquid water at 25°C is:

C. 6010 + (75 × 25)