How much heat energy is required to raise the temperature of 4.50L of water from 36.0^ºC to 44.6^ºC? A)162 J B)1620 J C)16200 J D)162000 J

Question

Quizplus · Accepted Answer

The specific heat capacity of water is 4.184 J/g℃. The mass of 4.50L of water is 4500g (density of water is 1g/mL). Thus, the amount of heat energy required to raise the temperature of the water can be calculated using the formula:

q = m × c × ΔT

where q is the heat energy, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.

Substituting the values, we get:

q = 4500g × 4.184 J/g℃ × (44.6℃ - 36.0℃)
q = 4500g × 4.184 J/g℃ × 8.6℃ 
q = 162000 J

Therefore, the answer is D) 162000 J, as it is the only option that matches the calculated value of the required heat energy in Joules.

How Much Heat Energy Is Required to Raise the Temperature