Suppose you wanted to heat a mug of water (178 mL) from room temperature 10 °C to 52 °C to make a cup of tea. How much energy (in units of joules) would you need from your microwave? (Cwater=4.184 J/g˚C)

Q = 31279.6 j

Explanation:

Given dа ta:

Mass = 178 mL

Initial temperature = 10°C

Final temperature = 52°C

Specific heat capacity = 4.184 j/g.°C

Heat absorbed = ?

Solution:

First of all we will convert the mL to g.

178 mL*1 L/1000 mL = 0.178 L

1 L = 1000 g

0.178 * 1000 = 178 g

Formula:

Q = m. c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

ΔT = T2 - T1

ΔT = 52°C - 10°C

ΔT = 42°C

Q = m. c. ΔT

Q = 178 g * 4.184 J/g.°C * 42°C

Q = 31279.6 j