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Given: Q=mc deltaT water (c=4.18 J/gC) A2B has a molar mass of 37.5g/mol A water-based solution of 750ml goes from a temperature is 27 degrees

Given: Q=mc deltaT

water (c=4.18 J/gC)

A2B has a molar mass of 37.5g/mol

A water-based solution of 750ml goes from a temperature is 27 degrees C to 38 degrees C when a reaction produces 13.5g of A2B(s)

a) was the reaction endothermic or exothermic

b) how much energy is released/absorbed per mole of A2B?

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