When a 4.25 g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter, the temperature drops from 22.0 degrees C to 16.9 degrees C. Calculate ΔH (kJ/mol) for the solution process. NH4NO3(s) → NH4+(aq) + NO3-(aq) Assume that the specific heat of the solution is the same as that of pure water. Express your answer to two significant figures and include the appropriate units.

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cyanhound711Lv1

11 Dec 2019

When a 4.25 g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter, the temperature drops from 22.0 degrees C to 16.9 degrees C. Calculate ΔH (kJ/mol) for the solution process.

NH₄NO_3(s) → NH₄⁺_(aq) + NO₃^-_(aq)

Assume that the specific heat of the solution is the same as that of pure water. Express your answer to two significant figures and include the appropriate units.

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(a) When a 4.25-g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter (Figure 5.17), the temperature drops from 22.0 to 16.9 °C. Calculate ∆H (in kJ/mol NH₄NO₃) for the solution process:

NH₄NO₃(s) NH₄⁺(aq) + NO₃^–(aq)

Assume that the specific heat of the solution is the same as that of pure water. (b) Is this process endothermic or exothermic?

chocolateminnow755

When a 4.25 g sample of solid ammonium nitrate dissolves in 60.0 gof water in a coffee-cup calorimeter, the temperature drops from22.0 degrees C to 16.9 degrees C.

Calculate Delta H kJ/mol NH4NO3 for the solution process

NH4NO3 ( s) yields NH4 (there is a plus sign above the four)(aq) +^ + NO3(negative sign above the three) (aq)

Assume that the specific heat of the solution is the same as thatof pure water.
Express your answer to two significant figures and include theappropriate units.

roseyak242

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