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Which statement describes how a basic coffee cup calorimeter works? |
It uses the mass and specific heat of water along with a thermometer to measure the gain or loss of energy when a substance is added. |
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Which statement defines calorimetry? |
the measurement of energy that is given off or absorbed in a physical or chemical process |
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Which statement defines the heat capacity of a sample? |
the quantity of heat that is required to raise the sample’s temperature by 1°C (or Kelvin) |
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A 1.20-g sample of propane (C3H8) is burned in a bomb calorimeter. The temperature of the calorimeter rises from 20.0°C to 30.0°C. The calorimeter has a mass of 2.000 kg and a specific heat of 2.95 J/(g • °C). If the molar mass of propane is 44.0 g/mol, what is the molar heat of combustion of propane? |
2,160 kJ/mol |
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When complete combustion of a 0.260-mol sample of a compound occurs in a bomb calorimeter, the temperature of the calorimeter increases from 20.0°C to 52.0°C. The mass of the calorimeter is 1.50 kg, and its specific heat is 3.410 J/(gi°C). What amount of heat would be produced by burning 1 mol of the compound? |
630 kJ |
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A sample of octane (C8H18) that has a mass of 0.750 g is burned in a bomb calorimeter. As a result, the temperature of the calorimeter increases from 21.0°C to 41.0°C. The specific heat of the calorimeter is 1.50 J/(g • °C), and its mass is 1.00 kg. How much heat is released during the combustion of this sample? |
30.0 kJ |
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A sample of an unknown substance has a mass of 0.465 kg. If 3,000.0 J of heat is required to heat the substance from 50.0°C to 100.0°C, what is the specific heat of the substance? |
0.129 J/(gi°C) |
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Which statement defines calorimeter? |
a device that measures the heat that is gained or lost in a chemical change |
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Which diagram is a bomb calorimeter? |
b. |
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A copper rod that has a mass of 200.0 g has an initial temperature of 20.0°C and is heated to 40.0°C. If 1,540 J of heat are needed to heat the rod, what is the specific heat of copper? |
0.385 J/(gi°C) |
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Which units express heat capacity? |
J/°C, J/K, cal/°C, cal/K |
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Which statement defines specific heat capacity for a given sample? |
the quantity of heat that is required to raise 1 g of the sample by 1°C (Kelvin) at a constant pressure |
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Complete combustion of a 0.600-g sample of a compound in a bomb calorimeter releases 24.0 kJ of heat. The bomb calorimeter has a mass of 1.30 kg and a specific heat of 3.41 J/(gi°C). If the initial temperature of the calorimeter is 25.5°C, what is its final temperature? |
30.9°C |
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During an endothermic phase change, what happens to the potential energy and the kinetic energy? |
Potential energy increases, and kinetic energy stays the same. |
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Which phase change is most likely taking place in this graph? |
a solid to a liquid |
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The molar heat of fusion for water is 6.01 kJ/mol. How much energy must be added to a 75.0-g block of ice at 0°C to change it to 75.0 g of liquid water at 0°C? |
25.04 kJ |
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Which substance releases 4.58 kJ of energy when 6.37 mol freeze? |
nitrogen |
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The molar heat of fusion of lead (Pb) is 1.140 kcal/mol. How much heat must be added to 97.0 g of solid lead at its melting point in order for it to completely melt? |
0.534 kcal |
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Which explanation correctly describes the phase change in the graph? |
This is an exothermic reaction that involves freezing. |
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The heat of vaporization for water is 40.7 kJ/mol. How much heat is released when 755.5 g of water vapor at 100°C condenses to liquid water at 100°C? |
-1,708.27 kJ |
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The heat of vaporization of methanol (CH3OH) is 1076 J/g. How much energy is absorbed by 2.35 mol of methanol when it vaporizes at its boiling point? |
81.02 kJ |
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These data apply to the specific heat and molar enthalpy of H2O: Cp,ice = 2.09 J/g•°C If a 50.0 g sample of ice at -11.5°C is heated to water vapor at 110°C, how much heat is required for this process? |
152.9 kJ |
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The information below shows properties of aluminum (Al). mc023-1.jpgHfus = 10.07 kJ/mol Which quantity of heat is required to melt a 342.9-g sample of Al? |
127.98 kJ |
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An engineer wants to determine an efficient method for condensing large amounts of steam into liquid water. Which constant should she use? |
b. -Hvap |
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What does the symbol (-mc004-1.jpgHfus) indicate in a phase change? |
A solid is being formed. |
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NaCl has a mc020-1.jpgHfus = 30.2 kJ/mol. What is the mass of a sample of NaCl that needs 732.6 kJ of heat to melt completely? |
82.7 g |
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Consider Ca(OH)2 mc025-1.jpg mc025-2.jpg + 2mc025-3.jpg and the following information. mc025-4.jpgHlat = -2,506 kJ/mol What is the mc025-8.jpgHhydr of mc025-9.jpg? |
-533 kJ/mol |
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Consider KF mc022-1.jpg mc022-2.jpg and the following information. mc022-3.jpgHlat = -784 kJ/mol What is the DHhydr of mc022-7.jpg? |
-431 kJ/mol |
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mc009-1.jpg Which answer accurately describes the diagram? |
The temperature decreases, and the process is endothermic. |
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What is the mc012-1.jpgHsol for LiF mc012-2.jpg mc012-3.jpg + mc012-4.jpg? The lattice energy is -1,036 kJ/mol, the enthalpy of hydration for mc012-5.jpg is -499 kJ/mol, and the enthalpy of hydration for mc012-6.jpg is -431 kJ/mol. |
106 kJ/mol |
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Which statement defines the enthalpy of hydration? |
the change in enthalpy when 1 mol of a gaseous ion becomes fully hydrated |
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Consider NaI mc021-1.jpg mc021-2.jpg and the following information. mc021-3.jpgHlat = -704 kJ/mol What is the mc021-8.jpgHsol of this compound? |
47 kJ/mol |
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Which formula can be used to calculate the enthalpy of solution? |
c |
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Which energy changes in the enthalpy of solution are endothermic, and which are exothermic? |
a |
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Which statement accurately describes the diagram? |
a. The temperature increases after dissolution, and the process is exothermic. |
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The mc017-1.jpgHsol for CaCl2 is 41 kJ/mol, and the lattice energy is mc017-2.jpg2,258 kJ/mol. If the hydration enthalpy for chloride ions is -313 kJ/mol, what is the hydration enthalpy for calcium ions? |
b -1,591 kJ/mol |
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What is the mc016-1.jpgHsol for MgF2 mc016-2.jpg Mg2+ + 2mc016-3.jpg? The lattice energy is -2,957 kJ/mol, the enthalpy of hydration for Mg2+ is -1,903 kJ/mol, and the enthalpy of hydration for mc016-4.jpg is -431 kJ/mol. |
b. 192 kJ/mol |
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What is the mc010-1.jpgHsol for mc010-2.jpg? The lattice energy is -788 kJ/mol, the enthalpy of hydration for mc010-3.jpg is -410 kJ/mol, and the enthalpy of hydration for mc010-4.jpg is -313 kJ/mol. |
65 kJ/mol |
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Consider RbOH mc020-1.jpg mc020-2.jpg and the following information. mc020-3.jpgHlat = -765.01 kJ/mol What is the mc020-8.jpgHsol rounded to the correct number of significant figures? |
-82.9 kJ/mol |
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Consider the following intermediate chemical equations. mc015-1.jpg What is the enthalpy of the overall chemical equation NO(g) + O(g) mc015-2.jpg NOmc015-3.jpg(g)? |
-304.1 kJ |
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What is enthalpy? |
the total heat content of the system |
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Consider the following intermediate chemical equations. mc007-1.jpg When you form the final chemical equation, what should you do with CO? |
Cancel out CO because it appears as a reactant in one intermediate reaction and a product in the other intermediate reaction. |
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Consider these intermediate chemical equations: mc005-1.jpg What is an overall chemical equation that has only HCN and CH4 as products, and NHmc005-2.jpg and C as reactants? |
d. mc005-6.jpg |
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What is the overall enthalpy change DHrxn for the system? |
300 kJ |
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According to the enthalpy diagram below, which of the following statements is true? |
Arrow C indicates that the third intermediate reaction is exothermic. |
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What is the overall chemical equation for smog after the above intermediate reactions are combined? |
d. mc003-6.jpg |
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Which of the following statements is true? |
a. The overall chemical reaction is exothermic. |
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Which overall chemical equation is obtained by combining these intermediate equations? |
a. ch4(g) +20.. |
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What is the enthalpy of the overall chemical reaction mc014-2.jpg? |
-1,300 kJ |
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What is the overall enthalpy change DHrxn for the system? |
300 kJ |
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What is the correct enthalpy diagram using the Hess law for this system? |
a. When you combine the intermediate chemical equations, which substance do you cancel out? |
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What is the enthalpy of the overall chemical equation NO(g) + O(g) mc015-2.jpg NOmc015-3.jpg(g)? |
-304.1 kJ |
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According to the enthalpy diagram below, which of the following statements is true? |
Arrow C indicates that the third intermediate reaction is exothermic. |
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According to the Hess law, which of the following depicts the enthalpy diagram summarizing the above intermediate reactions and their overall chemical reaction? |
d |
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