(a)
Interpretation: In the given system,
Concept introduction:
Calorimetry is a technique used to measure how much heat is produced or absorbed during a
Here,
(a)
Answer to Problem 1ASA
Explanation of Solution
The initial temperature is
Final temperature is
Expression for
Thus,
(b)
Interpretation: In the given system,
Concept introduction:
Calorimetry is a technique used to measure how much heat is produced or absorbed during a chemical reaction. It is used to determine the specific heat of the metal. The expression for heat evolved or absorbed is as follows:
Here,
(b)
Answer to Problem 1ASA
Explanation of Solution
The initial temperature of metal is
Final temperature is
Expression for
Thus,
(c)
Interpretation: The amount of heat flowed into the water is to be determined.
Concept introduction:
Calorimetry is a technique used to measure how much heat is produced or absorbed during a chemical reaction. It is used to determine the specific heat of the metal. The expression for heat evolved or absorbed is as follows:
Here,
(c)
Answer to Problem 1ASA
Explanation of Solution
Amount of water is
Specific heat of water is
Now, calculate heat flowing in water as follows:
Thus, heat flowed to water is
(d)
Interpretation: The specific heat of metal is to be determined.
Concept introduction:
Calorimetry is a technique used to measure how much heat is produced or absorbed during a chemical reaction. It is used to determine the specific heat of the metal. The expression for heat evolved or absorbed is as follows:
Here,
(d)
Answer to Problem 1ASA
Explanation of Solution
Amount of metal is
Heat given by metal is absorbed by water. Thus, heat given by metal is
Now, calculate heat flowing in water as follows:
Thus, the specific heat of metal is
(e)
Interpretation: The specific heat of metal is to be determined.
Concept introduction:
The relation between molecular mass and specific metal is as follows:
Here,
(e)
Answer to Problem 1ASA
Explanation of Solution
Substitute values in the above formula
Thus, the approximate molecular formula of metal is
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Chapter 14 Solutions
CHEMICAL PRIN.IN THE LAB-LM>CUSTOM<
- For the reaction TiCl2(s) + Cl2(g) TiCl4(), rG = 272.8 kj/mol-txn. Using this value and other data available in Appendix L, calculate the value of fG for TiCl2(s).arrow_forwardThe decomposition of ozone, O3, to oxygen, O2, is an exothermic reaction. What is the sign of q? If you were to touch a flask in which ozone is decomposing to oxygen, would you expect the flask to feel warm or cool?arrow_forwardThe formation of aluminum oxide from its elements is highly exothermic. If 2.70 g Al metal is burned in pure O2 to give A12O3, calculate how much thermal energy is evolved in the process (at constant pressure).arrow_forward
- For the reaction BaCO3(s) BaO(s) + CO2(g), rG = +219.7 kJ/mol-rxn. Using this value and other data available in Appendix L, calculate the value of fG for BaCO3(s).arrow_forwardSodium reacts violently with water according to the equation Na(s) + H2O() NaOH(aq) + H2(g) Without doing calculations, predict the signs of rH and rS for the reaction. Verify your prediction with a calculation.arrow_forwardThe bombardier beetle uses an explosive discharge as a defensive measure. The chemical reaction involved is the oxidation of hydroquinone by hydrogen peroxide to produce quinone and water: C6H4(OH)2(aq) + H2O2(aq) C6H4O2(aq) + 2H2O(l) Calculate H for this reaction from the following data: C6H4(OH)2(aq) C6H4O2(aq) + H2(g)H = 177.4 kJ H2(g) + O2(g) H2O2(aq)H = 191.2 kJ H2(g) + 12O2(g) H2O(g)H = 241.8 kJ H2O(g) H2O(l)H = 43.8 kJarrow_forward
- The normal melting point of benzene, C6H6, is 5.5 C. For the process of melting, what is the sign of each of the following? (a) rH (b) rS (c) rG at 5.5 C (d) rSG at 0.0 C (e) rG at 25.0 Carrow_forwardA student performing a calorimetry experiment combined 100.0 ml. of 0.50 M HCI and 100.0 ml. of 0.50 M NaOH in a StyrofoamTM cup calorimeter. Both solutions were initially at 20.0 C, but when the two were mixed, the temperature rose to 23.2 C (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 ml of 0.50 M NaOH. WIII the AT observed be greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCI and 100.0 ml. of 1.00 M NaOH. Will the T observed be greater than, less than, or equal to that in the first experiment, and why?arrow_forwardFor each of the following processes, predict the algebraic sign of rH, rS, and rG. No calculations are necessary; use your common sense. (a) The decomposition of liquid water to give gaseous oxygen and hydrogen, a process that requires a considerable amount of energy. (b) Dynamite is a mixture of nitroglycerin, C3H5N3O9, and diatomaceous earth. The explosive decomposition of nitroglycerin gives gaseous products such as water, CO2, and others; much heat is evolved. (c) The combustion of gasoline in the engine of your car, as exemplified by the combustion of octane. 2 C8H18(g) + 25 O2(g) 16 CO2(g) + 18 H2O(g)arrow_forward
- Consider the reaction 2HCl(aq)+Ba(OH)2(aq)BaCl2(aq)+2H2O(l)H=118KJ Calculate the heat when 100.0 rnL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M Ba(OH)2 Assuming that the temperature of both solutions was initially 25.0C and that the final mixture has a mass of 400.0 g and a specific heat capacity of 4.18 J/C g, calculate the final temperature of the mixture.arrow_forwardWhen calculating rSfromSvalues, it is necessary to look up all substances, including elements in their standard state, such as O2(g), H2(g), and N2(g). When calculating rHfrom rHvalues, however, elements in theirstandard state can be ignored. Why is the situation different forSvalues?arrow_forwardThe combustion of methane can be represented as follows: a. Use the information given above to determine the value of H for the combustion of methane to form CO2(g) and 2H2O(l). b. What is Hf for an element in its standard state? Why is this? Use the figure above to support your answer. c. How does H for the reaction CO2(g) + 2H2O (1) CH4(g) + O2(g) compare to that of the combustion of methane? Why is this?arrow_forward
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