Posted by **Ellen** on Friday, October 22, 2010 at 12:04pm.

A calorimeter contains 21.0 mL of water at 14.0 degreesC. When 1.90 g of X (a substance with a molar mass of 70.0 g/mol) is added, it dissolves via the reaction

X(s)+H_2O(l)reacts to make X(aq)

and the temperature of the solution increases to 28.5degreesC.

Calculate the enthalpy change, Delta H, for this reaction per mole of X.

Assume that the specific heat and density of the resulting solution are equal to those of water [4.18 J/degrees C) and 1.0g/mL] and that no heat is lost to the calorimeter itself, nor to the surroundings.

## Answer This Question

## Related Questions

- Chemistry - A calorimeter contains 22.0 mL of water at 14.0 C. When 2.50 g of X...
- Chemistry Urgent - A calorimeter contains 32.0mL of water at 13.0∘C . When...
- Chemictry - A calorimeter contains 32.0 of water at 11.5. When 1.70 of (a ...
- chemestry - A calorimeter contains 16.0 of water at 15.0. When 1.60 of (a ...
- chem - A calorimeter contains 16.0ml of water at 15.0degrees celsius. When 1.60g...
- Chemistry - A calorimeter contains 30.0 mL of water at 11.0 degrees C. When 1.50...
- Calorimetry - A calorimeter contains 21.0 mL of water at 12.0 degress Celsius. ...
- ap chemistry - A calorimeter contains 20.0 of water at 12.5 . When 2.20 of (a ...
- ap chem - A calorimeter contains 20.0 of water at 12.5 . When 2.20 of (a ...
- Chemistry - Assume that a reaction occurs in which unknown substances R and S ...

More Related Questions