Answer: The amount of heat required is 371.72 kJ
Explanation:
To calculate the mass of water, we use the equation:
[tex]\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}[/tex]
Density of water = 1 g/mL
Volume of water = 1.20 L = 1200 mL (Conversion factor: 1 L = 1000 mL)
Putting values in above equation, we get:
[tex]1g/mL=\frac{\text{Mass of water}}{1200mL}\\\\\text{Mass of water}=(1g/mL\times 1200mL)=1200g[/tex]
To calculate the amount of heat absorbed or released, we use the equation:
[tex]Q= m\times c\times \Delta T[/tex]
Q = heat absorbed = ?
m = mass of water = 1200 g
c = specific heat capacity of water = 4.186 J/g °C
[tex]\Delta T={\text{Change in temperature}}=(100-26)^oC=74^oC[/tex]
Putting values in above equation, we get:
[tex]Q=1200g\times 4.186J/g^oC\times 74^oC=371716.8J=371.72kJ[/tex]
Conversion factor used: 1 kJ = 1000 J
Hence, the amount of heat required is 371.72 kJ
