if 75 kj of heat is transferred to 1200 g liquid water at 36 C, what would the new temperature of the water be?

θ2 = 50.93°

Explanation:

Given the following :

Quantity of heat = 75kj = 75 × 1000 = 75000J

Mass of liquid water = 1200g

Temperature of water = 36°C

Using the relation :

Q = mc∆T ; where

Q = heat energy (Joules, J)

m = mass of a substance (kg)

c = specific heat (units J/g.°C)

∆T = change in temperature (θ2 - θ1)

(The specific heat capacity of liquid water(c)

is 4.186 J/g.°C

Inputting values:

Q = mc(θ2 - θ1)

75000 = 1200 × 4.186 (θ2 - 36)

75000 = 1200 × 4.186(θ2) - 150.696

75000 = 5023.2(θ2) - 180835.2

75000 + 180835.2 = 5023.2θ2

255835.2 = 5023.2(θ2)

θ2 = 255835.2 / 5023.2

θ2 = 50.93°

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

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