In a constant-pressure calorimeter, 55.0 mL of 0.350 M Ba(OH), was added to 55.0 mL of 0.700 M HCI. The reaction caused the temperature of the solution to rise from 23.03 °C to 27.80 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g °C,) respectively), what is AH for this reaction (per mole H₂O produced)? Assume that the total volume is the sum of the individual volumes. AH= x10 TOOLS kJ/mol H₂O

In a constant-pressure calorimeter, 55.0 mL of 0.350 M Ba(OH), was added to 55.0 mL of 0.700 M HCI. The reaction caused the temperature of the solution to rise from 23.03 °C to 27.80 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g °C,) respectively), what is AH for this reaction (per mole H₂O produced)? Assume that the total volume is the sum of the individual volumes. AH= x10 TOOLS kJ/mol H₂O

Chemistry

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Chapter6: Thermochemistry

Section: Chapter Questions

Problem 127CWP: In a coffee-cup calorimeter, 150.0 mL of 0.50 M HCI is added to 50.0 mL of 1.00 M NaOH to make 200.0...

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A 29.1-mL sample of 1.05 M KOH is mixed with 20.9 mL of 1.07 M HBr in a coffee-cup calorimeter (see Section 6.6 of your text for a description of a coffee-cup calorimeter). The enthalpy of the reaction, written with the lowest whole-number coefficients, is 55.8 kJ. Both solutions are at 21.8C prior to mixing and reacting. What is the final temperature of the reaction mixture? When solving this problem, assume that no heat is lost from the calorimeter to the surroundings, the density of all solutions is 1.00 g/mL, and volumes are additive.
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