A constant-volume calorimeter was calibrated by carrying out a reaction known to release 0.704 kJ of heat in 0.600 L of solution in the calorimeter (q = -0.704 kJ), resulting in a temperature rise of 2.76 °C. In a subsequent experiment, 300.0 mL of 0.40 M HCI0, (aq) and 300.0 mL of 0.40 M NAOH(aq) were mixed in the same calorimeter and the temperature rose by 5.90 °C. What is the change in the internal energy of the reaction mixture as a result of the neutralization reaction? AU= kJ TOOLS x10

A constant-volume calorimeter was calibrated by carrying out a reaction known to release 0.704 kJ of heat in 0.600 L of solution in the calorimeter (q = -0.704 kJ), resulting in a temperature rise of 2.76 °C. In a subsequent experiment, 300.0 mL of 0.40 M HCI0, (aq) and 300.0 mL of 0.40 M NAOH(aq) were mixed in the same calorimeter and the temperature rose by 5.90 °C. What is the change in the internal energy of the reaction mixture as a result of the neutralization reaction? AU= kJ TOOLS x10

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

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 68E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of...

See similar textbooks

Similar questions

When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of neutralization.) At 23.7C, 25.0 mL of 0.475 M H2SO4 is neutralized by 0.613 M KOH in a coffee-cup calorimeter. Assume that the specific heat of all solutions is 4.18J/gC, that the density of all solutions is 1.00 g/mL, and that volumes are additive. (a) How many mL of KOH is required to neutralize H2SO4? (b) What is the final temperature of the solution?
A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of 25.00C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.34C. Assuming the solution has a heat capacity of 4.18 J/C g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
How many moles of isooctane must be burned to produce loo U of heat under standard state conditions?
For the reaction BaCO3(s) BaO(s) + CO2(g), rG = +219.7 kJ/mol-rxn. Using this value and other data available in Appendix L, calculate the value of fG for BaCO3(s).
When 1.000 g of gaseous butane, C4H10, is burned at 25C and 1.00 atm pressure, H2O(l) and CO2(g) are formed with the evolution of 49.50 kJ of heat. a Calculate the molar enthalpy of formation of butane. (Use enthalpy of formation data for H2O and CO2.) b Gf of butane is 17.2 kJ/mol. What is G for the combustion of 1 mol butane? c From a and b, calculate S for the combustion of 1 mol butane.