During an experiment, a student adds 1.23 g of cao to 200.0 ml of 0.500 m hcl. the student observes a temperature increase of 5.10 °c. assuming the solution/'s final volume is 200.0 ml, the density if 1.00 g/ml, and the heat capacity is 4.184 j / (g·°c, calculate the heat of the reaction,? hrxn.

Question

Chapman

Chemistry

3 September, 08:34

During an experiment, a student adds 1.23 g of cao to 200.0 ml of 0.500 m hcl. the student observes a temperature increase of 5.10 °c. assuming the solution/'s final volume is 200.0 ml, the density if 1.00 g/ml, and the heat capacity is 4.184 j / (g·°c, calculate the heat of the reaction,? hrxn.

+1

Answers (1)

Know the Answer?

Devan Brooks · Answer 1

Given:

Mass of CaO = 1.23 grams

Volume of HCl = 200 mL

Concentration of HCl = 0.500 M

Termperature increase = 5.10 degrees celcius

Final volume = 200 mL

Density of sol'n = 1 g/mL

Cp = 4.184 J/gC

Balanced Equation:

CaO + 2HCl - - - > CaCl2 + H2O

Mass of HCl = 200 mL/1000 * 0.5 mol/L * 36.46 g/mol

= 3.646 grams

Mass solution = 200mL * 1 g/mL = 200 grams

H = mCpdT

= 200 grams * 4.184 J/gC * 5.10 C

H = 4267.68 Joules