How much heat is required to raise the temperature of 90 g of water from `30^(@)C` to `100^(@)C`? [Molar heat capacity of water at constant pressure `=75.3J*mol^(-1)*K^(-1)`]

Explanation

The specific heat of water at constant pressure,
`c_(P)=(C_(P,m))/(M)=(75.3)/(18)=4.18J*g^(-1)*K^(-1)`
Where `C_(P,m)`=molar heat capacity at constant pressure,
M=Molar mass of the substance
Mass of water, m=909g and `DeltaT=(373-303)K=70K`
`therefore q=mxxc_(P)xxDeltaT=90xx4.18xx70=26334J=26.33kJ`
`therefore 26.33kJ` of heat is required to raise the temperature of 90g of water from `30^(@)C` to `100^(@)C`.