how many miles of water could be heated from 40 to how many

Q2 3. At a certain elevation, the boiling point of water is 78.5°C. Which of the following (in kJ) is heat to boil 30.0 mL of water at this elevation, if the water was initially at 13.4°C? (Cp 75.38 J/K mol, d 1.00 g/mL)

Solution

Volume of water= 30 ml, density of water = 1 g/ml, mass of water= volume* density= 30*1= 30 gm

This water need to be heated from 13.4 deg.c to 78.5 deg,c by supplying sensible heat and this sensible heat= mass of water* speciic heat* temperature difference

Since specific heat is given in J/mol.K, the mass of water need to be converted to moles, moles of water= mass/molar mass= 30/18= 1.67 moles

Sensible heat= 1.67*75.38*(78.5-13.4)=8195 joules= 8195/1000Kj= 8.195 KJ