When a 4.25g sample of solid ammonium nitrate dissolves in 60 gof water in a coffee cup calorimeter,the temperature drops from 22^oC to 16.9^oC.Calculate the ÎH(in KJ/mol andalso the ÎH in Kj/g NHÎ₄NO₃) for the solutionprocess.Assume the specific heat of the solution is the same as oftaht of pure wate which isÎH=4.18j/g.K)?

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22 Feb 2019

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When a 5.00-g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter (see figure below), the temperature drops from 23.0Â°C to 16.1Â°C. Calculate ÎH (in kJ/mol NH4NO3) for the solution process shown below. Assume that the specific heat of the solution is the same as that of pure water. Hint: this process occurs at constant pressure. Is this process endothermic or exothermic?

When a 3.88-g sample of solid ammonium nitrate dissolves in 60.0g of water in a coffee-cup calorimeter, the temperature drops from23.0 ÂºC to 18.4 ÂºC.

Calculate Î H (in kJ/mol NH_4NO_3) for the solution process
NH_4NO_3 â NH_4 ^ + (aq) + NO_3 ^ - (aq). Assume that the specificheat of the solution is the same as that of pure water.
Express your answer using two significant figures.

ÎH =______________ kJ/mol

Is this process endothermic or exothermic?

When a 3.88-g sample of solid ammonium nitrate dissolves in 60.0 gof water in a coffee-cup calorimeter, the temperature drops from23.0 degrees Celcius to 18.4 degrees Celcius .

Calculate change in Heat (in kj/mol NH4NO3) for the solutionprocess
NH4NO3(s)-->NH4(aq) + NO3(aq) . Assume that the specific heat ofthe solution is the same as that of pure water. Express your answerin two significant figures.

change in heat= ? kj/mol

Is this process endothermic or exothermic?

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