Concept explainers
Practice ProblemATTEMPT
Use the following data to calculate
Want to see the full answer?
Check out a sample textbook solutionChapter 5 Solutions
Chemistry
Additional Science Textbook Solutions
Organic Chemistry
Thermodynamics, Statistical Thermodynamics, & Kinetics
Organic Chemistry (9th Edition)
Chemistry: Atoms First
Organic Chemistry As a Second Language: Second Semester Topics
- SIMPLE ALGORITHM. Correct significant figures and rounding off (Conventional). 9. In the reaction 2Al(s) + 3O2(g) → 2Al2O3(s), determine the ΔH0f of Al2O3(s) if the value of ΔH0 is -3351 kJ.arrow_forwardSIMPLE ALGORITHM. Correct significant figures and rounding off (Conventional). 2. Given the following reactions Fe2O3(s) + 3CO(s) → 2Fe(s) + 3CO2(g) ΔH = -28.0 kJ 3Fe(s) + 4CO2(s) → 4CO2(g) + Fe3O4(s) ΔH = +12.5 kJ Determine the enthalpy of the reaction of Fe2O3 with CO: 3Fe2O3(s) + CO(g) → CO3(g) + 2Fe3O4(s).arrow_forwardCompute ΔGo at 200.0 oC for each of the following reactions, which are important in the chemistry of coal. Assume that coal has the same thermodynamic properties as graphite. Substance ΔHo(kJ/mol) So(J/(mol*K)) C(graphite) 0 5.7 H2O(g) -241.83 188.835 CO(g) -110.5 197.7 H2(g) 0 130.680 O2(g) 0 205.152 CO2(g) -393.5 213.8 C(s, coal) + H2O(g) CO(g) + H2(g) C(s, coal) + O2(g) CO2(g) C(s, coal) + 1/2O2(g) CO(g) CO(g) + H2O(g) CO2(g) + H2(g)arrow_forward
- A 115.26 g sample of aluminum is heated from 37 oC to its melting point of 660 oC and then melted completely. How much energy was absorbed by the sample? (Answer in kJ) S=0.91 J/goC Delta Hf = 10.7 kJ/molarrow_forwardProblem 22: Benzene (C6H6) burns in air to produce carbon dioxide and liquid water. How much heat is released per mole of C6H6 burned? The standard enthalpy of formation of C6H6 is 49.04 kJ/mol. Jjjjarrow_forwardSIMPLE ALGORITHM. Correct significant figures and rounding off (Conventional). 8. For the reaction H2(g) + Cl2(g) → 2HCl(g), determine the ΔH0f for HCl(g) in kJ/mol if the ΔH0 is -186 kJ.arrow_forward
- Consider the following reaction: 2 CH3OH(g) → 2 CH4(g) + O2(g) DH = 252.8 kJ (a) Is reaction exothermic or endothermic? ANSWERED (b) Calculate the amount of heat transferred when 24.0 g of CH3OH(g) is decomposed by this reaction at constant pressure. ANSWERED (c) For a given sample of CH3OH, the enthalpy change during the reaction is 82.1 kJ. How many grams of methane gas are produced? ANSWERED (d) How many kilojoules of heat are released when 38.5 g of CH4(g) reacts completely with O2(g) at constant pressure?arrow_forwardSIMPLE ALGORITHM: Correct significant figures and rounding off (Conventional). 3. Given the following reactions N2(g) + 2O2(g) → 2NO2(g) ΔH = 66.4 kJ 2NO(g) + O2(g) → 2NO2(g) ΔH = -114.2 kJ Determine the enthalpy of the reaction of the nitrogen to produce nitric oxide, N2(g) + O2(g) → 2NO(g).arrow_forward4. How much energy is removed from 500.0 g of water when the temperature is lowered by 1.10 o C? Answer: -550. cal (or -2.30 x 103 J) 5. How much energy is required to raise the temperature of 1000.0 g of water from 23.00 o C to 26.00 o C? Answer: 3.00 x 103 cal (or 1.26 x 104 J) 6. The specific heat of copper is (0.0924 cal/go C), how much energy is required to raise the temperature of 10.0 g of copper by 100.0 o C? Answer: 92.4 calarrow_forward
- Simple Algorithm: Solve the following problems. Write your answer on the space provided. Show your complete solutions. For your final answer, report correct significant figures and rounding off (Follow the conventional). 3. The value of ΔH0 for the reaction: 2Ba(s) + O2(g)→ 2BaO(s) is -1107 kJ. What is the amount of energy released when 5.75 g of Ba(s) reacts completely with oxygen to form BaO(s) in kJ?arrow_forward1. How much energy is removed from 500.0 g of water when the temperature is lowered by 1.10 o C? answer: -550. cal (or -2.30 x 103 J) 2. How much energy is required to raise the temperature of 1000.0 g of water from 23.00 o C to 26.00 o C? answer: 3.00 x 103 cal (or 1.26 x 104 J)arrow_forwardSIMPLE ALGORITHM. Correct significant figures and rounding off (Conventional). 5. Given the following reactions: 2S(s) + 3O2(g) → 2SO3(g) ΔH = -790 kJ S(s) + O2(g) → SO2(g) ΔH = -297 kJ Determine the enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide, 2SO2(g) + O2(g) → 2SO3(g).arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning