EA 0.3423 g sample of pentane, C5H12, was burned in a bomb calorimeter. The temperature of the calorimeter and the 1.000 kg of water contained therein rose from 20.22°C to 22 82°C. The heat capacity of the calorimeter is 221 kJ/^C. The heat capacity of water = 4.184 J/g.°C. What is the heat o combustion, in kilojoules, per gram of pentane? %3D Multiple Choice O 45.6 kJ/g 48 6 kJ/g 476 kJig None of the above 46.6 kJ/g

EA 0.3423 g sample of pentane, C5H12, was burned in a bomb calorimeter. The temperature of the calorimeter and the 1.000 kg of water contained therein rose from 20.22°C to 22 82°C. The heat capacity of the calorimeter is 221 kJ/^C. The heat capacity of water = 4.184 J/g.°C. What is the heat o combustion, in kilojoules, per gram of pentane? %3D Multiple Choice O 45.6 kJ/g 48 6 kJ/g 476 kJig None of the above 46.6 kJ/g

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...

See similar textbooks

Similar questions

THERMODYNAMICS: A 1.39 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/°C, contained 753 g of water. The temperature of the calorimeter and its contents increased from 23.77°C to 27.95°C. What is AH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place) Round your answer to 1 decimal place.
A 6.78 g sample of methanol was combusted in a bomb calorimeter. The temperature of the calorimeter increased by 12.7 °C. If the molar mass of methanol is 32.04 g/mol, and the heat capacity of the calorimeter is 5,104 J/°C, what is the molar AE for this reaction, in kJ/mol? Do not report units in your answer. Report your answer to one decimal place and include the correct sign.
The enthalpy of combustion of isooctane (C8H18), one of the many hydrocarbons in gasoline is 5.45 × 103 kJ/mol. Calculate the enthalpy change per gram of isooctane and per liter of isooctane (d = 0.688 g/mL).
When pure sulfuric acid is dissolved in water, heat is evolved. 10.65 g of pure sulfuric acid at 20.00 °C was added to a calorimeter containing 300 g of water at 20.00 °C. The temperature of the solution increased to 26.35 °C. If the specific heat of the mixture is 4.184 Jg1°C1, the density of water is 1 g/mL, and the heat capacity of the calorimeter is ignored, what is the heat evolved per mole of sulfuric acid? a. -83.2 kJ O b. -73.6 kJ O C. -76.0 kJ d. -80.8 kJ e. -78.4 kJ
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
The sugar arabinose, C5 H10 O5, is burned completely in oxygen in a calorimeter. C5 H10 O5 (8) + 502(g) → 5CO2(g) + 5H2 O(1) Burning a 0.541 g sample caused the temperature to rise from 20.00°C to 20.54°C. The heat capacity of the calorimeter and its contents is 15.2 kJ/°C. Calculate AH for the combustion reaction per mole of arabinose. ΔΗ+ kJ/mol
A chemist carefully measures the amount of heat needed to raise the temperature of a 1.65kg sample of C9H10O2 from 25.9°C to 37.9°C. The experiment shows that 3.09 X 104J of heat are needed. What can the chemist report for the molar heat capacity of C9H10O2? Round your answer to 3 significant digits. = J * mol-1 * K-1
A metal cube with a mass of 68.77 g and a temperature of 86.13°C is placed into 139.32 g of water with a temperature of 23.85°C. The specific heat capacity of the water is 4.184 J/gºC and the specific heat capacity of the metal is 1.659 J/g C. The final temperature of the water is 32.99°C. Calculate the amount of heat released by the metal (in J). Type your answer...
When 9.42 g of methane (CH4) is burned in a bomb calorimeter (heat capacity = 2.677 × 103 J/°C), the temperature rises from 24.00 to 27.08°C. Calculate the enthalpy change for the following reaction. (C= 12.00 amu, H = 1.00 amu) CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) Group of answer choices a. 8.425 kJ b. –14.01 kJ c. –8.425 kJ d. 8245 J e. 14.00 kJ
A calorimeter contained 81.0 g of water at 16.35°C. A 120.-g sample of iron at 66.60°C was placed in it, giving a final temperature of 19.80°C for the system. Calculate the heat capacity of the calorimeter. Specific heats are 4.184 J/g-°C for H20 and 0.444 Jg-°C for Fe. Heat capacity of the calorimeter = J°C
The combustion of toluene has a AErxn of -3.91 x 10³ kJ/mol. When 1.30 g of toluene (C7H8) undergoes combustion in a bomb calorimeter, the temperature rises from 22.80 °C to 36.11 °C. Find the heat capacity of the bomb calorimeter. Express your answer using three significant figures. Ccal = 17| ΑΣΦ ? kJ/°C
when 50.0 mL of 0.200 M NaOH is mixed with 50 mL of 0.200 M HCl in a coffee cup calorimeter, the temperature increases from 23.5 degrees C to 26.5 degrees C. Assuming that the density of the resulting solution is 1.00 g/mL and the specific heat capacity of the solution is 4.18 J/g degrees C, what is qrxn?