(a)
Interpretation:
The value of enthalpy change
Concept introduction:
The change in the enthalpy of a reaction when the reactant is converted into product under standard conditions is called standard enthalpy of reaction.
The expression for standard enthalpy of reaction is,
Here,
(a)
Explanation of Solution
The value of
Given:
Refer to Appendix L for the values of standard enthalpy of formation.
The standard enthalpy of formation of
The standard enthalpy of formation of
The standard enthalpy of formation of
The standard enthalpy of formation of
The reaction involved in photosynthesis is,
The
Substitute the value of
The value of
(b)
Interpretation:
The enthalpy change involved in producing one molecule of glucose by the process of photosynthesis at
Concept introduction:
The relationship between the number of moles and the number of molecules is,
Also,
(b)
Explanation of Solution
The enthalpy change involved in producing one molecule of glucose by the process of photosynthesis at
Given:
The enthalpy change involved in the production of one mole of glucose by the process of photosynthesis at
Since
The enthalpy change involved in producing one molecule of glucose by the process of photosynthesis is
(c)
Interpretation:
The energy of a photon of light having a wavelength
Concept introduction:
The energy of one photon
Here,
Value of
(c)
Explanation of Solution
The energy of a photon of light having wavelength
Given:
The wavelength of light is
The speed of light is
Planks constant is
Substitute the values in equation (2).
The energy of a photon of light having wavelength
(d)
Interpretation:
The absorption of one photon at
Concept introduction: If the energy of one photon is greater than the energy required for the production of one mole of substance then single photon absorption is sufficient for the reaction to proceed else multiple photons must be absorbed.
(d)
Explanation of Solution
The energy of one photon calculated in part(c) is
Therefore multiple photons must be absorbed for the production of one molecule of glucose by photosynthesis reaction.
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Chapter 24 Solutions
Chemistry & Chemical Reactivity
- 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_forwardThe enthalpy change for the following reaction is 393.5 kJ. C(s,graphite)+O2(g)CO2(g) (a) Is energy released from or absorbed by the system in this reaction? (b) What quantities of reactants and products are assumed? (c) Predict the enthalpy change observed when 3.00 g carbon burns in an excess of oxygen.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
- The enthalpy change when 1 mol methane (CH4) is burned is 890 kJ. It takes 44.0 kJ to vaporize 1 mol water. What mass of methane must be burned to provide the heat needed to vaporize 1.00 g water?arrow_forward9.68 What are some features of petroleum that make it such an attractive fuel?arrow_forwardHow much heat is produced by combustion of 125 g of methanol under standard state conditions?arrow_forward
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