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Solved: When a 6.50-g sample of solid sodium hydroxide

Chapter , Problem 5.55

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QUESTION:

When a 6.50-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter (Figure 5.17), the temperature rises from 21.6 to 37.8 °C.

(a) Calculate the quantity of heat (in kJ) released in the reaction.

(b) Using your result from part (a), calculate \(\Delta H\) (in kJ/mol NaOH) for the solution process. Assume that the specific heat of the solution is the same as that of pure water.

Questions & Answers

QUESTION:

When a 6.50-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter (Figure 5.17), the temperature rises from 21.6 to 37.8 °C.

(a) Calculate the quantity of heat (in kJ) released in the reaction.

(b) Using your result from part (a), calculate \(\Delta H\) (in kJ/mol NaOH) for the solution process. Assume that the specific heat of the solution is the same as that of pure water.

ANSWER:

Q:When a 6.50-g sample of solid sodium hydroxide(NaOH) dissolves in 100.0 g of water in acoffee-cup calorimeter (Figure 5.17), the temperature rises from 21.6C to 37.8 C.(a) Calculate the quantity of heat (in kJ) released in the reaction.(b) Using your result from part (a), calculate change in Enthalpy (in kJ/mol NaOH) for thesolution process. Assume that the specific heat of the solution is the same as that of pure water Step By Step Solution:Step 1 of 3:Data for computation:Mass of Sodium Hydroxide sample:6.5 gramsMass of water used: 100gInitial temperature:Final Temperature:Specific heat capacity of water:Molecular mass of NaOH=39.996 g/mol

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