In experiment, 10.0g of methanol, CH_3OH, was burned in a calorimeter which cont
ID: 476137 • Letter: I
Question
In experiment, 10.0g of methanol, CH_3OH, was burned in a calorimeter which contains 1.50 kg water. What will be the temperature change of the water, in K? specific heat capacity of H_3O: 4.184 J g^-1 K^-1 Specific heat capacity of calorimeter: 925 j k^-1 Standard heat combustion of CH_2OH: -726.4 kJ mol^-1. 31.5 36.2 93.6 245 Isopropanol, C_3H_8O, boils at 82.5 degree C. Calculate the amount of heat energy, in kJ, required to completely convert 100 g of C_3H_8O(e), initially at a temperature of 25 degree C, to vapour at its boiling point Specific Heat Capacity of C_3H_8O(l): 2.68 J g^-1 K^-1 Specific Heat Capacity of C_3H-8O(g): 1.54J g^-1 K^-1 Latent Heat of Fusion of Isopropanol: 5.28 mol^-1 Latent Heat of Vaporization of Isopropanol: 44.0 kJ mol^-1 17.6 24.2 82.0 88.5 97.4Explanation / Answer
Question 15
The isopropanol" in this case is going to do two things
1) It reaches 82.5 0C from 25 0C in liquid state.
2) Then it is converting to vapour
Q = m c T
Q = quantity of heat in joules (J)
m = mass of the substance acting as the environment in
grams (g)
c = specific heat capacity (4.19 for H2O) in J/(g oC)
T = change in temperature = Tfinal - Tinitial in oC
Let us calculate the heat is need for this conversion
Q = 100 x 2.68 x (82.5-25) + 100 x 44 x 103 / 60.1
Q = 15410 + 73211
Q = 88621 Joules or 88.6 KJ ~88.5 Kj
Hence option D is correct answer