You mix 125 mL of 0.220 M CSOH with 50.0 mL of 0.550 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from21.30 °C before mixing to 23.84 °C after the reaction.CsOH(aq) + HF (aq) →→ CsF(aq) + H₂O(l)What is the enthalpy of reaction per mole of CSOH? Assume the densities of the solutions are all 1.00 g/mL, and the specific heat capacities ofthe solutions are 4.2 J/g - K.Enthalpy of reaction -kJ/molYou should use care when dissolving H₂SO4 in water because the process is highly exothermic. To measure the enthalpy change, 5.3 g ofconcentrated H₂SO4() was added (with stirring) to 134 g of water in a coffee-cup calorimeter. This resulted in an increase in temperature from21.6 °C to 30.5 °C. Calculate the enthalpy change for the process H₂SO4 () → H₂SO4 (aq), in kJ/mol. Assume the specific heat capacity of thesolution is 4.2 J/g. K.Enthalpy change =kJ/molYou mix 125 mL of 0.220 M CSOH with 50.0 mL of 0.550 M HF in a coffee-cup calorimeter, and the temperatur21.30 °C before mixing to 23.84 °C after the reaction.CsOH(aq) + HF (aq) → CsF(aq) + H₂O(l)What is the enthalpy of reaction per mole of CSOH? Assume the densities of the solutions are all 1.00 g/mL, andthe solutions are 4.2 J/g. K.Enthalpy of reaction=[kJ/mol

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You mix 125 mL of 0.220 M CsOH with 50.0 mL of 0.550 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from 21.30 °C before mixing to 23.84 °C after the reaction. CsOH(aq) + HF (aq) →→ CsF(aq) + H₂O() What is the enthalpy of reaction per mole of CsOH? Assume the densities of the solutions are all 1.00 g/mL., and the specific heat capacities of the solutions are 4.2 J/g. K. Enthalpy of reaction - kJ/mol

You mix 125 mL of 0.220 M CsOH with 50.0 mL of 0.550 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from 21.30 °C before mixing to 23.84 °C after the reaction. CsOH(aq) + HF (aq) →→ CsF(aq) + H₂O() What is the enthalpy of reaction per mole of CsOH? Assume the densities of the solutions are all 1.00 g/mL., and the specific heat capacities of the solutions are 4.2 J/g. K. Enthalpy of reaction - kJ/mol

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

You mix 125 mL of 0.220 M CSOH with 50.0 mL of 0.550 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from
21.30 °C before mixing to 23.84 °C after the reaction.
CsOH(aq) + HF (aq) →→ CsF(aq) + H₂O(l)
What is the enthalpy of reaction per mole of CSOH? Assume the densities of the solutions are all 1.00 g/mL, and the specific heat capacities of
the solutions are 4.2 J/g - K.
Enthalpy of reaction -
kJ/mol
You should use care when dissolving H₂SO4 in water because the process is highly exothermic. To measure the enthalpy change, 5.3 g of
concentrated H₂SO4() was added (with stirring) to 134 g of water in a coffee-cup calorimeter. This resulted in an increase in temperature from
21.6 °C to 30.5 °C. Calculate the enthalpy change for the process H₂SO4 () → H₂SO4 (aq), in kJ/mol. Assume the specific heat capacity of the
solution is 4.2 J/g. K.
Enthalpy change =
kJ/mol
You mix 125 mL of 0.220 M CSOH with 50.0 mL of 0.550 M HF in a coffee-cup calorimeter, and the temperatur
21.30 °C before mixing to 23.84 °C after the reaction.
CsOH(aq) + HF (aq) → CsF(aq) + H₂O(l)
What is the enthalpy of reaction per mole of CSOH? Assume the densities of the solutions are all 1.00 g/mL, and
the solutions are 4.2 J/g. K.
Enthalpy of reaction=[
kJ/mol

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