In a generic chemical reaction involving reactants A and B and products C and D, aA + bB»cC + dD, the standard enthalpy AHn° of the reaction is given by AHn = CAH¢°(C) + DAH£°(D) -aAH;°(A) – bAH;°(B) Notice that the stoichiometric coefficients, a, b, c, d, are an important part of this equation. This formula is often generalized as follows, where the first sum on the right- hand side of the equation is a sum over the products and the second sum is over the reactants: ΔΗ Στοducis nΔΗ; ' -Σeactants mΔΗ ' where m and n represent the appropriate stoichiometric coefficients for each substance. Part A What is AHrm° for the following chemical reaction? H2O(1) + CCL4 (1)→COCl (g) + 2HCI(g) You can use the following table of standard heats of formation (AHỆ°) to calculate the enthalpy of the given reaction. Standard Heat of Standard Heat of Element/ Compound Element/ Compound Formation (kJ/mol) Formation (kJ/mol) H(g) 218 N(g) 473 H2(g) O2 (g) CCL (1) -139.5 O(g) 249 H2O(1) -285.8 HCI(g) -92.30kJ C(g) 71 COC2 (g) -218.8kJ C(s) HNO3 (aq) -206.6 Express the heat of formation to three significant figures and include the appropriate units. > View Available Hint(s) HA Value Units

In a generic chemical reaction involving reactants A and B and products C and D, aA + bB»cC + dD, the standard enthalpy AHn° of the reaction is given by AHn = CAH¢°(C) + DAH£°(D) -aAH;°(A) – bAH;°(B) Notice that the stoichiometric coefficients, a, b, c, d, are an important part of this equation. This formula is often generalized as follows, where the first sum on the right- hand side of the equation is a sum over the products and the second sum is over the reactants: ΔΗ Στοducis nΔΗ; ' -Σeactants mΔΗ ' where m and n represent the appropriate stoichiometric coefficients for each substance. Part A What is AHrm° for the following chemical reaction? H2O(1) + CCL4 (1)→COCl (g) + 2HCI(g) You can use the following table of standard heats of formation (AHỆ°) to calculate the enthalpy of the given reaction. Standard Heat of Standard Heat of Element/ Compound Element/ Compound Formation (kJ/mol) Formation (kJ/mol) H(g) 218 N(g) 473 H2(g) O2 (g) CCL (1) -139.5 O(g) 249 H2O(1) -285.8 HCI(g) -92.30kJ C(g) 71 COC2 (g) -218.8kJ C(s) HNO3 (aq) -206.6 Express the heat of formation to three significant figures and include the appropriate units. > View Available Hint(s) HA Value Units

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 76E: Write reactions for which the enthalpy change will be a. Hf for solid aluminum oxide. b. the...

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A rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.
The enthalpy of combustion of diamond is -395.4 kJ/mol. C s, dia O2 g CO2 g Determine the fH of C s, dia.
A piece of lead of mass 121.6 g was heated by an electrical coil. From the resistance of the coil, the current, and the Time the current flowed, it was calculated that 235 J of heat was added to the lead. The temperature of the lead rose from 20.4C to 35.5C. What is the specific heat of the lead?
In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.
When one mole of ethylene gas, C2H4, reacts with fluorine gas, hydrogen fluoride and carbon tetrafluoride gases are formed and 2496.7 kJ of heat are given off. What is Hf for CF4(g)?
Although the gas used in an oxyacetylene torch (Figure 5.7) is essentially pure acetylene, the heat produced by combustion of one mole of acetylene in such a torch is likely not equal to the enthalpy of combustion of acetylene listed in Table 5.2. Considering the conditions for which the tabulated data are reported, suggest an explanation.
Natural gas companies in the United States use the therm as a unit of energy. One therm is 1105 BTU. (a) How many joules are in one therm? (1J=9.48104BTU) (b) When propane gas, C3H8, is burned in oxygen, CO2 and steam are produced. How many therms of energy are given off by 1.00 mol of propane gas?
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.)
Write reactions for which the enthalpy change will be a. Hf for solid aluminum oxide. b. the standard enthalpy of combustion of liquid ethanol, C2H5OH(l). c. the standard enthalpy of neutralization of sodium hydroxide solution by hydrochloric acid. d. Hf for gaseous vinyl chloride, C2H3Cl(g). e. the enthalpy of combustion of liquid benzene, C6H6(l). f. the enthalpy of solution of solid ammonium bromide.
Graphite is burned in oxygen to give carbon monoxide and carbon dioxide. If the product mixture is 33% CO and 67% CO2 by mass, what is the heat from the combustion of 1.00 g of graphite?
The complete combustion of acetylene, C2H2(g), produces 1300. kJ of energy per mole of acetylene consumed. How many grams of acetylene must be burned to produce enough heat to raise the temperature of 1.00 gal water by 10.0c if the process is 80.0% efficient? Assume the density of water is 1.00 g/cm3

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