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A quantity of 1.535 g of methanol (CH3OH) was burned in a constant - volume bomb calorimeter. Consequently the temperature of the water rose from 20.27 degrees Celsius to 26.87 degrees Celsius. If the mass of water surrounding the calorimeter was exactly 1000 g and the heat capacity of the bomb calorimeter without the water was 1.75 kJ/degrees Celsius, calculate the molar heat of the combustion of methanol. The answer is in kJ/mol. I really need someone to explain to me step by step on how to do these types of problems. I'm having a hard time understanding how to do these types of problems.
Show all the steps in the mechanism for the following reaction, When benzene is mixed with deuterated sulfuric acid, deuterium is slowly incorporated onto the ring. Show the mechanism for this reaction and explain how this relates the sulfonation of ..
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