1,200 cal of heat energy is added to a liquid with a specific heat of 0.57 cal/g°C. If the temperature increases from 20.°C to 33°C, what is the mass of the liquid?

The mass of the liquid = 162 g

Explanation:

As we know ,  

Q = mc (ΔT)

where Q = Heat energy of the liquid

c = specific heat of the liquid

ΔT = change in temperature

m = mass of the liquid

As given , the temperature increases from 20.°C to 33°C,

⇒ ΔT = 33 - 20 = 13°C

Also given , c = 0.57 cal/g°C

                   Q = 1200 cal

∴ we get

1200 = (m)(0.57)(13)

⇒ 1200 = m(7.41)

⇒m = = 161.943 ≈ 162 g

So, we get

The mass of the liquid = 162 g

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.

explanation: