Apiece of copper has a temperature of 75.6 0c. when the metal is placed in 100.0 grams of water at 19.1 0c, the temperature rises by 5.5 0c. what is the mass of the metal?

115.58 g ≅ 115.6 g.

Explanation:

Heat lost by copper (Qc) = Heat gained by the water (Qw) ,

- (Qc) = (Qw).

Qw = m.c.ΔT,

where, Qw is the amount of heat released to water (Q = ??? J).

m is the mass of water (m = 100.0 g).

c is the specific heat capacity of solution (c = 4.18 J/g.°C).  

ΔT is the difference in T (ΔT = final temperature - initial temperature = 24.6°C - 19.1°C = 5.5°C).

∴ Q = m.c.ΔT = (100.0 g)(4.18 J/g.°C)(5.5°C) = 2299 J.

(Qc) = m.c.ΔT,

where, Qc is the amount of heat lost by substance (Qc = - 2299 J).

m is the mass of water (m = ??? g).

c is the specific heat capacity of solution (c = 0.39 J/g.°C).

ΔT is the difference in T (ΔT = final temperature - initial temperature = 24.6°C - 75.6°C = - 51.0°C).

∴ (- 2299 J) = (m)(0.39 J/g.°C)(- 51.0°C).  

∴ m of copper = (- 2299 J)/(0.39 J/g.°C)(- 51.0°C) = 115.58 g ≅ 115.6 g.

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water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.