What is the ammount if heat in joules required to increase the temperature of a 49.5 gram sample of water from 22c to 66c

9.1KJ

Explanation:

From

H = mcθ

m = mass of the water = 49.5g

c = heat capacity of water = 4.2 Jg-1

θ = temperature change = (66°C - 22°C) = 44°C

H = 49.5*4.2*44 = 9.1KJ

What is the amount of heat, in joules, required to increase the temperature of a 49.5-gram sample of water from 22°C to 66°C?

(1) 9100 J (2) 4600 J (3) 1400 J (4) 2300 J

Answer:

9100 J is the amount of heat, in joules, required to increase the temperature of a 49.5-gram sample of water from 22°C to 66°C.

Explanation:

Given: Q = ? J

mass = 49.5 g = 0.0495 kg

T1 = 22°C

T2 = 66°C

Cp = 4.18 J/Kg°C

Q = mCpΔT

Q = (4.95) (4.18) (66 - 22)

Q = 9104 J

So 9100 J is the amount of heat, in joules, required to increase the temperature of a 49.5-gram sample of water from 22°C to 66°C.