Answer :
Answer:
The required heat energy is [tex]\bf{19680~cal}[/tex].
Explanation:
The heat energy 'Q' required to raise the temperature of water is given by
[tex]Q = M~s~\Delta \theta[/tex]
where 'M' is the mass of water, 's' is the specific heat capacity of water and '[tex]\Delta \theta[/tex]' is the change of temperature.
Given, [tex]M = 246 gm, \Delta \theta = (100^{0}~C - 20^{0}~C) = 80^{0}~C[/tex] and we know that the specific heat capacity of water is [tex]s = 1~cal~gm^{-1}~^{0}C^{-1}[/tex].
Substituting the values in the above expression, the required heat energy is
[tex]Q = 246~gm \times 1~cal~gm^{-1}~^{0}C^{-1} \times 80^{0}~C = 19680~Cal[/tex]
The heat required to raise the temperature of water is required.
The heat required is [tex]82380.48\ \text{J}[/tex]
m = Mass of coffee = 246 g
c = Specific heat of water = 4.184 J/g C
[tex]\Delta T[/tex] = Change in temperature = [tex]100-20=80^{\circ}\text{C}[/tex]
Heat is given by
[tex]Q=mc\Delta T\\\Rightarrow Q=246\times 4.186\times 80\\\Rightarrow Q=82380.48\ \text{J}[/tex]
The heat required is [tex]82380.48\ \text{J}[/tex]
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