7. Determining the Sign of AHIndicate the sign of the enthalpy change, AH, in these processes carried out underatmospheric pressure and indicate whether each process is endothermic or exothermic:a. an ice cube meltsb. 1 g of butane (C4H10) is combusted in sufficient oxygen to give completecombustion to CO2 and H2O.

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Answered: 7. Determining the Sign of AH Indicate…

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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The specific heat capacity of silver is 0.24 J/°C.g. a. Calculate the energy required to raise the temperature of 143.0 g Ag from 268 K to 292 K. Energy = b. Calculate the energy required to raise the temperature of 1.0 mole of Ag by 1.0°C (called the molar heat capacity of silver). Molar Heat Capacity= J/°C-mol c. It takes 1.18 kJ of energy to heat a sample of pure silver from 12.4°C to 15.4°C. Calculate the mass of the sample of silver. g Mass=
Calculate the enthalpy change of the exothermic reaction of 5.20 g of CaCl2(s) dissolved in 0.32 kg of water inside a coffee-cup calorimeter. The combined initial and final temperatures were 20.8°C and 29.4°C, respectively. * a. -12 KJ b. -62 KJ c. 92 KJ d. 48 KJ
II. Rapid walking through a distance of 2.2 km for 30 minutes per day requires 41 J while swimming for the Same penod of time through the same distance requires 226 J. Will these forms of exercise allow you to lose weight equivalent to ig of glucose (MW = 180 g/mol) in 1 week? The standard enthalpy of combustion of glucose is -2806 kJ.
5. When 1.00g of NaCl (MM 58.44 g/mol) is dissolved in 50.00g of water, the temperature drops by 0.319°C. This temperature change is only detectable by the most sensitive thermometers. If this process takes place in a very well insulated calorimeter, no calorimeter constant is needed. a. Calculate the enthalpy change per gram of NaCl. b. Calculate the enthalpy change per mole of NaCl.
To calibrate a calorimeter, 10.0 ml of 1.0 M NaOH and 5.0 ml of 1.0 M HCl was used in a calorimetry experiment. Which of the following will have NO EFFECT on the calculated heat capacity of the calorimeter, Ccal? a. Accidentally adding HNO3 instead of HCl. b.Adding a smaller volume of 1.0 M HCl. c.Using a bigger styrofoam ball for calibration. d.Using a wet test tube for calibration.
What is the enthalpy change, Delta Hrxn, for the following reaction? 2 RbI (s) + Cl2 (g) --> 2 RbCl (s) + I2 (s) a. 1.33 x 103 kJ b. 656 kJ c. – 215 kJ d. 107 kJ e. 763 kJ f. none of these g. – 1.33 x 103 kJ h. 871 kJ
pt pt pt pt pt pt pt pt pt pt pt pt pt pt You should use care when dissolving H₂SO4 in water because the process is highly exothermic. To measure the enthalpy change, 5.8 g of concentrated H₂SO4() was added (with stirring) to 140. g of water in a coffee-cup calorimeter. This resulted in an increase in temperature from 21.0 °C to 30.3 °C. Calculate the enthalpy change for the process H₂SO4(l) → H₂SO4 (aq), in kJ/mol. Assume the specific heat capacity of the solution is 4.2 J/g. K. Enthalpy change = kJ/mol ?
The complete combustion of salicylic acid releases 21.90 kJ of energy per gram of salicylic acid.In a particular bomb calorimeter (initially at room temperature), the combustion of 0.2745 g of salicylic acid, in the presence of excess oxygen, causes the temperature of the calorimeter to rise by 1.85 °C.When a 0.2999-g sample of an unknown organic substance is similarly burned in the same calorimeter, the temperature rises by 3.59 °C.What is the energy of combustion per unit mass of the unknown substance?
D. All of the statements are false. 2NO + 0₂ → NO, A, H° = 90.25 kJ/mol NO₂, AH° = 33.18 kJ/mol → 2NO₂ For numbers 3-4: Consider the data given. 3. What is the value of the standard enthalpy of reaction (kJ/mol)? A. 57.07 C. 114.14 B. -57.07 D. -114.14 4. What is the value of the standard enthalpy of reaction (kJ/mol) of the decomposition of NO2? A. 57.07 C. 114.14 D. -114.14 B. -57.07
10. Bacteria sour wines and beers by converting ethanol, C₂H5OH, into acetic acid, CH₂COOH. Assume that the reaction is C₂H5OH(1) + O₂(g) → CH₂COOH() + H₂O(1) The standard molar enthalpies of combustion of ethanol and acetic acid to produce liquid water are, respectively, - 1367 kJ/mol and -875 kJ/mol. Write chemical equations for the combustions, and use Hess' law to determine the standard enthalpy change for the conversion of ethanol to acetic acid.
2) The combustion of 0.25 g sucrose, C1HO11, in a bomb calorimeter causes the temperature to rise from 24.9 to 28.3 °C. If the heat capacity of the calorimeter is 4.90 kJ/°C, calculate the heat of combustion of sucrose in kJ/g.
19. A peice of titanium metal with a mass of 20.8 g is heated in boiling water to 99.5°C and the dropped into a coffee cup calorimeter containing 75.0 g water at 21.7°C. When the thermal equilibrium is reached, the final temperature is 24.3°C. Calculate the specific heat capacity of titanium. 15. The enthalphy of fusion (melting) of water is 6.0 kJ/mol. CAlculate the quantity of energy that must be transffered to melt 25.0 g H2O at 0°C. ps. pls answer the number 19 if you will just answer one question. But if you can answer two questions pls answer it. Im begging youu :<

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