In an experiment to determine the heat of combustion of methanol (CH3OH) a student used a set up like the one shown in the diagram below. Study the set- up and the data below it and answer the questions that follows

Volume of water = 500cm³

Final temperature of water = 27.0⁰C

Initial temperature of water = 20.0⁰C

Final mass of lamp + methanol = 22.11g

Initial mass of lamp + methanol = 22.98g

Density of water = 1.0/ cm³

Heat change = mass x temperature x 4.2j/g/C

(a) Write an equation for the combustion of methanol ( 1 mk)

(b) Calculate

(i) The number of moles of methanol used in the experiment (C=12), (O= 16) (H=1) ( 2 mks)

(ii) Heat change in this experiment

(iii) The heat of combustion per mole of methanol ( 2 mks)

Transcribed Image Text:

Thermometer www.dow beaker water "lamp Methanol Thermometer www.dow beaker water "lamp Methanol

Answer rating: 100% (QA)

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