Consider the problem below: (Equation 1) H2(g) + F2(g) ---> 2 HF(e) AH = -542.2 kJ/mol %3D (Equation 2) 2 H2(g) + O2(g)---> 2 H2O1) AH = -571.6 kJ/mol (Equation 3) 2 F2(g) + 2 H2O(1) 4 HF(g) O2lg) ΔΗ ??????? ---> + The AH for equation 3 is:_ _(express in kJ) Screen Reader Version Consider the problem below: (Equation 1) H2(g) + F2(g) arrow 2 HF(g) AH = minus 542.2 kJ/mol (Equation 2) 2 H2(g) + O2(g) arrow 2 H2O1) AH = minus 571.6 kJ/mol %3D (Equation 3) 2 F2(g) + 2 H20) arrow 4 HF(g) + O2lg) AH = ??????? The AH for equation 3 is:_ _(express in kJ)

Consider the problem below: (Equation 1) H2(g) + F2(g) ---> 2 HF(e) AH = -542.2 kJ/mol %3D (Equation 2) 2 H2(g) + O2(g)---> 2 H2O1) AH = -571.6 kJ/mol (Equation 3) 2 F2(g) + 2 H2O(1) 4 HF(g) O2lg) ΔΗ ??????? ---> + The AH for equation 3 is:_ _(express in kJ) Screen Reader Version Consider the problem below: (Equation 1) H2(g) + F2(g) arrow 2 HF(g) AH = minus 542.2 kJ/mol (Equation 2) 2 H2(g) + O2(g) arrow 2 H2O1) AH = minus 571.6 kJ/mol %3D (Equation 3) 2 F2(g) + 2 H20) arrow 4 HF(g) + O2lg) AH = ??????? The AH for equation 3 is:_ _(express in kJ)

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 47E: Consider the combustion of propane: C3H8(g)+5O2(g)3CO2(g)+4H2O(l)H=2221KJ Assume that all the heat...

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In earlier times, ethyl ether was commonly used as an anesthetic. It is, however, highly flammable. When five milliliters of ethyl ether, C4H10O(l)(d=0.714g/mL), are burned in a bomb calorimeter, the temperature rises from 23.5C to 39.7C. The calorimeter contains 1.200 kg of water and has a heat capacity of 5.32 kJ/C. (a) What is qH2o? (b) What is qcal? (c) What is q for the combustion of 5.00 mL of ethyl ether? (d) What is q for the combustion of one mole of ethyl ether?
Ethanol, C2H5OH, is used as a fuel for motor vehicles, particularly in Brazil. (a) Write the balanced equation for the combustion of ethanol to CO2(g) and H2O(g), and, using the data in Appendix G, calculate the enthalpy of combustion of 1 mole of ethanol. (b) The density of ethanol is 0.7893 g/mL. Calculate the enthalpy of combustion of exactly 1 L of ethanol. (c) Assuming that an automobile’s mileage is directly proportional to the heat of combustion of the fuel, calculate how much farther an automobile could be expected to travel on 1 L of gasoline than on 1 L of ethanol. Assume that gasoline has the heat of combustion and the density of n—octane, C8H18(Hf=208.4kJ/mol;density=0.7025g/mL).
Peanuts and peanut oil are organic materials and bum in air. How many burning peanuts does it take to provide the energy to boil a cup of water (250 mL of water)? To solve this problem, we assume each peanut, with an average mass of 0.73 g, is 49% peanut oil and 21% starch; the remainder is noncombustible We further assume peanut oil is palmitic acid, C16H32O2, with an enthalpy of formation of 848.4 kJ/mol. Starch is a long chain of C6H10O5 units, each unit having an enthalpy of formation of 960 kJ.
Consider the combustion of propane: C3H8(g)+5O2(g)3CO2(g)+4H2O(l)H=2221KJ Assume that all the heat in Example 7-3 comes from the combustion of propane. What mass of propane must be burned to furnish this amount of energy assuming the heat transfer process is 60.% efficient?
A cubic piece of uranium metal (specific heat capacity = 0.117 J/C g) at 200.0C is dropped into 1.00 L deuterium oxide ("heavy water;" specific heat capacity = 4.21 I J/C g) at 25.5C. The final temperature of the uranium and deuterium oxide mixture is 28.5C. Given the densities of uranium (19.05 g/cm3) and deuterium oxide (1.11 g/mL). what is the edge length of the cube of uranium?
Microwave ovens convert radiation to energy. A microwave oven uses radiation with a wavelength of 12.5 cm. Assuming that all the energy from the radiation is converted to heat without loss, how many moles of photons are required to raise the temperature of a cup of water (350.0 g, specific heat =4.18J/gC) from 23.0C to 99.0C?
Assume 200. mL of 0.400 M HCl is mixed with 200. mL of 0.400 M NaOH in a coffee-cup calorimeter The temperature of the solutions before mixing was 25.10 C; after mixing and allowing the reaction to occur, the temperature is 27.78 C. What is the enthalpy change when one mole of acid is neutralized? (Assume that the densities of all solutions are 1.00 g/mL and their specific heat capacities are 4.20 J/g K.)
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)
Some automobiles and buses have been equipped to bum propane (C3H8). Compare the amounts of energy that can be obtained per gram of C3H8(g) and per gram of gasoline, assuming that gasoline is pure octane, C8H18(l). (See Example 7-11.) Look up the boiling point of propane. What disadvantages are there to using propane instead of gasoline as a fuel?
Principles of Heat Flow Titanium is a metal used in jet engines. Its specific heat is 0.523 J/g C. If S.SS g of titanium absorb 4.78 J, what is the change in temperature?
Fructose is a sugar commonly found in fruit. A sample of fructose, C6H12O6, weighing 4.50 g is burned in a bomb calorimeter that contains 1.00 L of water (d=1.00g/mL). The heat capacity of the calorimeter is 16.97 kJ/PC. The temperature of the calorimeter and water rise from 23.49C to 27.72C. (a) What is q for the calorimeter? (b) What is q for water in the calorimeter? (c) What is q when 4.50 g of fructose are burned in the calorimeter? (d) What is q for the combustion of one mole of fructose?

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