Chapter 5: Q34E (page 227)
A teaspoon of the carbohydrate sucrose (common sugar) contains 16 calories (16kcal). What is the mass of one teaspoon of sucrose if the average number of calories for carbohydrates is 4.1 Calories/g?
The mass of one teaspoon of sucrose is approximately 3.9 g.
Over 30 million students worldwide already upgrade their learning with Vaia!
All the tools & learning materials you need for study success - in one app.
Get started for free
The decomposition of hydrogen peroxide, \({{\bf{H}}_{\bf{2}}}{{\bf{O}}_{\bf{2}}}\), has been used to provide thrust in the control jets of various space vehicles. Using the data in Appendix G, determine how much heat is produced by the decomposition of exactly 1 mole of \({{\bf{H}}_{\bf{2}}}{{\bf{O}}_{\bf{2}}}\)under standard conditions.
\({\bf{2}}{{\bf{H}}_{\bf{2}}}{{\bf{O}}_{\bf{2}}}\left( {\bf{l}} \right) \to {\bf{2}}{{\bf{H}}_{\bf{2}}}{\bf{O}}\left( {\bf{g}} \right){\bf{ + }}{{\bf{O}}_{\bf{2}}}\left( {\bf{g}} \right)\)
The white pigment \({\bf{Ti}}{{\bf{O}}_{\bf{2}}}\)is prepared by the reaction of titanium tetrachloride, \({\bf{TiC}}{{\bf{l}}_{\bf{4}}}\), with water vapor in the gas phase:
\({\bf{TiC}}{{\bf{l}}_{\bf{4}}}\left( {\bf{g}} \right){\bf{ + 2}}{{\bf{H}}_{\bf{2}}}{\bf{O}}\left( {\bf{g}} \right) \to {\bf{Ti}}{{\bf{O}}_{\bf{2}}}\left( {\bf{s}} \right){\bf{ + 4HCl}}\left( {\bf{g}} \right)\)
How much heat is evolved in the production of exactly 1 mole of \({\bf{Ti}}{{\bf{O}}_{\bf{2}}}\)(s) under standard state conditions?
Ethylene, \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{2}}}\), a byproduct from the fractional distillation of petroleum, is fourth among the 50 chemical compounds produced commercially in the largest quantities. About 80% of synthetic ethanol is manufactured from ethylene by its reaction with water in the presence of a suitable catalyst. \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{2}}}{\bf{(g) + }}{{\bf{H}}_{\bf{2}}}{\bf{O(g)}} \to {{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}{\bf{OH(l)}}\).Using the data in the table inAppendix G, calculate ฮHยฐ for the reaction.
From the data in Table 5.2, determine which of the following fuels produces the greatest amount of heat per gram when burned under standard conditions: CO(g), CH4(g), or C2H2(g).
Aluminum chloride can be formed from its elements:
(i)\({\bf{2Al(s) + 3C}}{{\bf{l}}_{\bf{2}}}{\bf{(g)}} \to {\bf{2AlC}}{{\bf{l}}_{\bf{3}}}{\bf{(s) \Delta H^\circ = ?}}\)
Use the reactions here to determine the ฮHยฐ for reaction(i):
\(\begin{array}{*{20}{l}}{\left( {{\bf{ii}}} \right){\rm{ }}{\bf{HCl(g)}} \to {\bf{HCl(aq) \Delta H^\circ (ii) = - 74}}{\bf{.8 kJ}}}\\{\left( {{\bf{iii}}} \right){\rm{ }}{{\bf{H}}_{\bf{2}}}{\bf{(g) + C}}{{\bf{l}}_{\bf{2}}}{\bf{(g)}} \to {\bf{2HCl(g) \Delta H^\circ (iii) = - 185 kJ}}}\\{\left( {{\bf{iv}}} \right){\rm{ }}{\bf{AlC}}{{\bf{l}}_{\bf{3}}}{\bf{(aq)}} \to {\bf{AlC}}{{\bf{l}}_{\bf{3}}}{\bf{(s) \Delta H^\circ (iv) = + 323 kJ}}}\\{\left( {\bf{v}} \right){\rm{ }}{\bf{2Al(s) + 6HCl(aq)}} \to {\bf{2AlC}}{{\bf{l}}_{\bf{3}}}{\bf{(aq) + 3}}{{\bf{H}}_{\bf{2}}}{\bf{(g) \Delta H^\circ (v) = - 1049 kJ}}}\end{array}\)
What do you think about this solution?
We value your feedback to improve our textbook solutions.
