Answer : The amount of heat is required is, 1672 J
Solution :
Formula used :
\(Q= m\times c\times \Delta T\)
\(Q= m\times c\times (T_{final}-T_{initial})\)
Q= heat gained
m= mass of the substance = 20 g
c = heat capacity of water = 4.18 J/g ° C
\(T_{final}\) = final temperature = \(30^oC\)
\(T_{initial}\) = initial temperature = \(10^oC\)
Now put all the given values in the above formula, we get the heat required.
\(Q= (20g)\times (4.18 J/g^oC)\times (30-10)^oC\)
Q = 1672 Joules
Therefore, the amount of heat is required is, 1672 J
