(a)
Interpretation:
The given reaction is endothermic or exothermic has to be discussed.
Concept Introduction
Endothermic Reactions:
The
Examples for endothermic reactions:
- Melting ice cubes.
- Evaporation of water.
- Producing sugar from photosynthesis.
(b)
Interpretation:
The given reaction is endothermic or exothermic has to be discussed.
Concept Introduction:
Exothermic Reactions:
The chemical reaction in which heat energy is released known as exothermic reaction. The
Examples for exothermic reaction:
- Making ice cubes.
- Formation of snow in clouds.
- Condensation of rain from water vapour.
- Rusting iron.
- Burning sugar.
(c)
Interpretation:
The given reaction is endothermic or exothermic has to be discussed.
Concept Introduction:
Endothermic Reactions:
The chemical reaction in which heat energy is absorbed known as endothermic reaction. If the energy required to break the bond is greater than the energy released, then it is said to be endothermic reaction.
Examples for endothermic reactions:
- Melting ice cubes.
- Evaporation of water.
- Producing sugar from photosynthesis.
(d)
Interpretation:
The given reaction is endothermic or exothermic has to be discussed.
Concept Introduction:
Endothermic Reactions:
The chemical reaction in which heat energy is absorbed known as endothermic reaction. If the energy required to break the bond is greater than the energy released, then it is said to be endothermic reaction.
Examples for endothermic reactions:
- Melting ice cubes.
- Evaporation of water.
- Producing sugar from photosynthesis.
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Chapter 9 Solutions
General, Organic, and Biological Chemistry
- Classify each of the reactions according to one of the four reaction types summarized in Table 18.1. (a) C6H12O6(s) + 6 O2(g) 6 CO2(g) + 6 H2O() rH = 673 kj/mol-rxn rS = 60.4 j/K mol-rxn (b) MgO(s) + C(graphite) Mg(s) + CO(g) rH = 490.7 kJ/mol-rxn rS = 197.9 J/K mol-rxn TABLE 18.1 Predicting Whether a Reaction Will Be Spontaneous Under Standard Conditionsarrow_forwardClassify each of the reactions according to one of the four reaction types summarized in Table 18.1. (a) Fe2O3(s) + 2 Al(s) 2 Fe(s) + Al2O3(s) rH = 851.5 kj/mol-rxn rS = 375.2 J/K mol-rxn (b) N2(g) + 2 O2(g) 2 NO2(g) rH = 66.2 kJ/mol-rxn rS = 121.6 J/K mol-rxn TABLE 18.1 Predicting Whether a Reaction Will Be Spontaneous Under Standard Conditionsarrow_forwardHydrogen chloride gas dissolves in water to form hydrochloric acid (an ionic solution). HCl(g)H2OH+(aq)+Cl(aq) Find H for the above reaction. The data are given in Table 6.2.arrow_forward
- Should heat be added as a reactant or as a product to each of the following equations for chemical reactions based on the given thermicity for the reaction? a. H2 + Cl2 2HCl (exothermic) b. 4NO + 6H2O 4NH3 + 5O2 (endothermic) c. 2H2O + 2Cl2 4HCl + O2 (endothermic) d. 2H2O 2H2 + O2 (exothermic)arrow_forward. A(n) _______ speeds up a reaction without being consumed.arrow_forwardShould heat be added as a reactant or as a product to each of the following equations for chemical reactions based on the given thermicity for the reaction? a. 2SO2 + O2 2SO3 (exothermic) b. N2 + O2 2NO (endothermic) c. CH4 + 2O2 CO2 + 2H2O (exothermic) d. 2H2O + 2Cl2 4HCl + O2 (endothermic)arrow_forward
- A student set up an experiment for six different trials of the reaction between 1.00-M aqueous acetic acid, CH3COOH, and solid sodium hydrogen carbonate, NaHCO3. CH3COOH(aq) + NaHCO3(s) NaCH3CO2(aq) + CO2(g) + H2O() The volume of acetic acid was kept constant, but the mass of sodium bicarbonate increased with each trial. The results of the tests are shown in the figure. (a) In which trial(s) is the acetic acid the limiting reactant? (b) In which trial(s) is sodium bicarbonate the limiting reactant? (c) Explain your reasoning in parts (a) and (b).arrow_forward. For the reaction N2(g)+3H2(g)2NH3(g), list the types of bonds that must be broken and the type of bonds that must form for the chemical reaction to take place.arrow_forwardA novel process for obtaining magnesium from sea water involves several reactions. Write a balanced chemical equation for each step of the process. (a) The first step is the decomposition of solid calcium carbonate from seashells to form solid calcium oxide and gaseous carbon dioxide. (b) The second step is the formation of solid calcium hydroxide as the only product from the reaction of the solid calcium oxide with liquid water. (c) Solid calcium hydroxide is then added to the seawater, reacting with dissolved magnesium chloride to yield solid magnesium hydroxide and aqueous calcium chloride. (d) The solid magnesium hydroxide is added to a hydrochloric acid solution, producing dissolved magnesium chloride and liquid water. (e) Finally, the magnesium chloride is melted and electrolyzed to yield liquid magnesium metal and diatomic chlorine gas.arrow_forward
- xplain why aluminum cans make good storage containers for soft drinks. Styrofoam cups can be used to keep coffee hot and cola cold. How can this be?arrow_forwardWhat is G for the following reaction? 2Br(aq)+Cl2(g)Br2(l)+2Cl(aq) Use data given in Table 19.1.arrow_forward4.60 Why are fuel additives used?arrow_forward
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