If 50g of load (of specific heat 0.11 kcal/kg . C degree) at 100 degree C is put

Question

If 50g of load (of specific heat 0.11 kcal/kg . C degree) at 100 degree C is put into 75 g of water (of specific heat 1.0 kcl/kg. C degree) at 0 degree C. what is the final temperature of the mixture? 2.0 degree 6.8 degree C %0 degree Which one of the following quantities is the smallest unit of the heat energy? calorie kilocalorie btu joule How many moles are there in 2.00kg of copper? The atomic weight of copper is 63.5 g/mol and its density is 8.90 g/cm3 15.3 31.5 51.3 53.1 The figure shows a graph of the temperature of a pure substance as a function of time as heat is added to it at a constant rate in a closed container. If LF is the latent heat of fusion of this substance and LV is its latent heat of vaporization, what is the value of the ratio LV/LF?

Explanation / Answer

11)

T = final temperature of the mixture

cw = specific heat of water = 1

cl = specific heat of lead = 0.11

ml = mass of lead = 50 g

mw = mass of water = 75 g

using conservation of energy

Heat lost by lead = heat gained by water

ml cl (100 - T) = mw cw (T - 0)

(50) (0.11) (100 - T) = (75) (1) (T)

T = 6.83 C

2)

Joule

3)

M = atomic mass = 63.5 g/mol

m = given mass = 2 kg = 2000 g

n = number of moles = m/M = 2000/63.5 = 31.5 moles

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