The enthalpy of solution (dissolving) of sodium hydroxide is given below. Determine the change in temperature of a coffee cup calorimeter containing 150 ml of water when 5.00 g NaOH (40.00 g/mol) is added to the container. You may assume that the solution has the same specific heat and density as water.

NaOH(s) → NaOH(aq) ΔH =-44.51 KJ

a. +8.87°C

b. +2.70 C

c. 2.70°C

d. 8.87°C

The change in temperature of a coffee cup calorimeter is 8.87°C.

Explanation:

Volume of the water = V = 150 g

Density of the water , d =1.0 g/mL

Mass of the water = M

Mass of solution = m = M = 150.0 g

Moles of NaOH =

Energy released when 0.125 moles of NaOH added in water = Q

1 kJ = 1000 J

Heat gained by water = Q' = -Q ( conservation of energy)

Specific heat of solution = c = 4.184 J/g°C

Change in temperature of the solution =

The change in temperature of a coffee cup calorimeter is 8.87°C.

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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: