Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: OpenStax
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Textbook Question
Chapter 7, Problem 66E
Using the bond energies in Table 7.2, determine the approximate enthalpy change for each of the following reactions:
(a)
(b)
(c)
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Using the bond energies as shown, determine the approximate enthalpy change for each of the following reactions:(a) Cl2(g) + 3F2(g) ⟶ 2ClF3(g)(b) H2 C = CH2(g) + H2(g) ⟶ H3 CCH3(g)(c) 2C2 H6(g) + 7O2(g) ⟶ 4CO2(g) + 6H2 O(g)
How do I solve this question?
The average bond enthalpy for C−H is 413 kJ/mol. 413 kJ of energy is required to break a mole of CH into atoms: CH(g)→C(g)+H(g), ΔH=413 kJ Using this information, and your answer from Part A, calculate the enthalpy change of the reaction from Part B. That is, calculate the energy required to break only the carbon-carbon bonds in benzene. PART A ANSWER ΔH∘rxn =
5535.1 kJ.. PART B ANSWER C6H6(g)→6CH(g)
Chapter 7 Solutions
Chemistry by OpenStax (2015-05-04)
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- hat is the enthalpy change for a process? Is enthalpy a state function? In what experimental apparatus are enthalpy changes measured?arrow_forwardA commercial process for preparing ethanol (ethyl alcohol), C2H5OH, consists of passing ethylene gas. C2H4, and steam over an acid catalyst (to speed up the reaction). The gas-phase reaction is Use bond enthalpies (Table 9.5) to estimate the enthalpy change for this reaction when 37.0 g of ethyl alcohol is produced.arrow_forwardUsing the bond dissociation enthalpies in Table 8.8, estimate the enthalpy of combustion of gaseous methane, CH4, to give water vapor and carbon dioxide gas.arrow_forward
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- Enter your answer in the provided box. Use the bond enthalpies given below to estimate the enthalpy of reaction for the combination of carbon monoxide and oxygen to produce carbon dioxide: 2CO(g) + O2(g) → 2CO2(g)arrow_forwardUsing average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: 2co(g) + 2NO(g)→2C02(g) + N2(g) kJarrow_forward5. For the reaction H2(g) + C2H4(g) C2H6(g) (a) Estimate the enthalpy of reaction, using the bond enthalpy values. (b) Calculate the enthalpy of reaction, using standard enthalpies of formation. (AH? for H2, C2H4, and C2H6 are 0 kJ/mol, 52.3 kJ/mol, and -84.7 kJ/mol, respectively.)arrow_forward
- Consider the following compounds: BeCl 2 , MgBr 2 , and SrBr 2 . Answer the following questions based on expected periodic trends: (a) Which is expected to have the shortest ionic bonds? (b) Which is expected to have the highest lattice energy? (c) Which is expected to have the lowest melting point?arrow_forwardConsider the following compounds: CaCl 2 , CaI 2 , and MgCl 2 . Answer the following questions based on expected periodic trends: (a) Which is expected to have t he shortest ionic bonds? (b) Which is expected to have the highest lattice energy? (c) Which is expected to have the lowest melting point?arrow_forwardUse average bond energies together with the standard enthalpy of formation of C( g) (718.4 kJ/mol) to estimate the standard enthalpy of formation of gaseous benzene, C6H6( g). (Remember that average bond energies apply to the gas phase only.) Compare the value you obtain using average bond energies to the actual standard enthalpy of formation of gaseous benzene,82.9 kJ/mol. What does the difference between these two values tell you about the stability of benzene?arrow_forward
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