Answer :
Answer : The amount of heat required is, [tex]1.004\times 10^6J[/tex]
Explanation :
Formula used :
[tex]q=m\times c\times (T_{final}-T_{initial})[/tex]
where,
q = heat required = ?
m = mass of water = 30.0 kg = 3000 g
c = specific heat of water = [tex]4.184J/g^oC[/tex]
[tex]T_{final}[/tex] = final temperature = [tex]95^oC[/tex]
[tex]T_{initial}[/tex] = initial temperature = [tex]15^oC[/tex]
Now put all the given values in the above formula, we get:
[tex]q=3000g\times 4.184J/g^oC\times (95-15)^oC[/tex]
[tex]q=1004160J=1.004\times 10^6J[/tex]
Thus, the amount of heat required is, [tex]1.004\times 10^6J[/tex]