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Concept explainers
(a)
Interpretation: The balanced equation for the burning of methyl
Concept introduction:
- Balanced chemical equation of a reaction is written according to law of conservation of mass.
- Stoichiometry of a
chemical reaction is the relation between reactants and products of the reaction and it is represented by the coefficients used for the reactants and products involved in the chemical equation.
(a)
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Answer to Problem 35PS
The balanced equation for the given reaction is,
Explanation of Solution
When methyl
The balanced equation for the combustion of methyl myristate is given as:
(b)
Interpretation: Enthalpy change for the oxidation of methyl myristate should be determined using the given data.
Concept introduction:
Enthalpy of combustion: At standard conditions when one mole of substance is burnt completely in presence of oxygen, the enthalpy change involved is called enthalpy of combustion.
(b)
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Answer to Problem 35PS
Enthalpy change is calculated to be
Explanation of Solution
Given:
Change in enthalpy can be calculated by the equation:
(c)
Interpretation: The fuel which provides more energy (Hexadecane or methyl
Concept introduction:
Enthalpy of combustion: At standard conditions when one mole of substance is burnt completely in presence of oxygen, the enthalpy change involved is called enthalpy of combustion.
(c)
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Answer to Problem 35PS
Hexadecane provide more energy than methyl
Explanation of Solution
For methyl myristate:
Change in enthalpy can be calculated by the equation:
For hexadecane:
Change in enthalpy can be calculated by the equation:
Hexadecane provide more energy than methyl myristate.
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Chapter 20 Solutions
Chemistry & Chemical Reactivity
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- The thermochemical equation for the burning of methane, the main component of natural gas, is CH4(g)+2O2(g)CO2(g)+2H2O(l)H=890kJ (a) Is this reaction endothermic or exothermic? (b) What quantities of reactants and products are assumed if H = 890 kJ? (c) What is the enthalpy change when 1.00 g methane burns in an excess of oxygen?arrow_forwardWhen 2.50 g of methane burns in oxygen, 125 kJ of heat is produced. What is the enthalpy of combustion per mole of methane under these conditions?arrow_forwardGraphite 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?arrow_forward
- The enthalpy change for the reaction of hydrogen gas with fluorine gas (o produce hydrogen fluoride is 542 U for the equation as written: mg src=Images/HTML_99425-10-41QAP_image001.jpg alt="" align="top"/> l type='a'> What is the enthalpy change per mole of hydrogen fluoride produced? Is the reaction exothermic or endothermic as written? What would be the enthalpy change for the reverse of the given equation (that 1%, for the decomposition of HF into its constituent elements)?arrow_forwardChlorine dioxide, ClO2, is a reddish yellow gas used in bleaching paper pulp. The average speed of a ClO2 molecule at 25C is 306 m/s. What is the kinetic energy (in joules) of a ClO2 molecule moving at this speed?arrow_forwardAlthough 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.arrow_forward
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