The total energy required is 47016 J.
It is defined as the heat required to raise the one degree temperature of the unit mass of a given substance.
Given by q = mcΔT
It is defined as the amount of heat required to convert a solid into a liquid or vapor, or a liquid into a vapor, without the change of temperature.
(1.) Energy required to convert -10°C to 0°C = q = mcΔT
q = (15 g)x(2.09 J/g·°C)(10°C)
q = (15 g)x(2.09 J/g·°C)x(10 °C)
q1 = 313.5 J
(2.) Energy required to convert 0°C ice to 0°C water = q = m·ΔHf
q = (15 g)x(334 J/g)
q2 = 5010 J
(3.) Energy required to raise the temperature 0°C water 100°C = q = mcΔT
q = (15 g)x(4.18 J/g·°C)(100 °C)
q3 = 6270 J
(4.) Energy required to convert 100 °C water to 100 °C steam = q = m·ΔHv
q = (15 g)x(2257 J/g)
q4 = 33855 J
(5.) Energy required to convert 100 °C steam to 150 °C steam = q = mcΔT
q = (15 g)x(2.09 J/g·°C)[(150 °C - 100 °C)]
q = (15 g)x(2.09 J/g·°C)x(50 °C)
q5 = 1567.5 J
Total heat energy = q1 + q2 + q3 + q4 + q5
Total heat energy = (313.5 + 5010 + 6270 + 33855 + 1567.5) = 47016 J
The total energy required is 47016 J.
To know more about specific heat, check out:
https://brainly.com/question/14646878
#SPJ4
