# Problem: When a 6.50-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 21.6°C to 37.8°C. Calculate ΔH (in kJ/mol NaOH) for the solution process NaOH(s) → Na+ (aq) + OH- (aq) Assume that the specific heat of the solution is the same as that of pure water. Express your answer with the appropriate units.

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93% (350 ratings) ###### Problem Details

When a 6.50-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 21.6°C to 37.8°C.

Calculate ΔH (in kJ/mol NaOH) for the solution process

NaOH(s) → Na(aq) + OH- (aq)

Assume that the specific heat of the solution is the same as that of pure water. Express your answer with the appropriate units.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Constant-Pressure Calorimetry concept. You can view video lessons to learn Constant-Pressure Calorimetry. Or if you need more Constant-Pressure Calorimetry practice, you can also practice Constant-Pressure Calorimetry practice problems.

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Our tutors rated the difficulty ofWhen a 6.50-g sample of solid sodium hydroxide dissolves in ...as high difficulty.

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Based on our data, we think this problem is relevant for Professor Atwood's class at UB.