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 data:

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

frequency, z, and the collision density, z, in carbon dioxide (co2), r 180 pm at 30 °c and 120 kpa

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