Reaction Represented Chapter 6 Quiz Test
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4 NH3 (g) + 3 O2 (g) --> 2 N2 (g) + 6 H2O (g)If the standard molar heats of formation of ammonia, NH3 (g), and gaseous water, H2O (g), are -46 kJ/mol and -242 kJ/mol, respectively, what is the value of for the reaction represented above?
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-190 kJ/mol
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-290 kJ/mol
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-580 kJ/mol
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-1270 kJ/mol
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-1640 kJ/mol
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This quiz, titled 'Reaction Represented Chapter 6', assesses understanding of thermochemical calculations, including heats of formation, enthalpy changes, and specific heat. It is designed for learners to apply concepts to solve real-world chemical reaction problems, enhancing their practical and analytical skills in chemistry.
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- 2.
Based on the information above, what is the enthalpy change for the sublimation of iodine, represented below?
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15 kJ/mol
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21 kJ/mol
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31 kJ/mol
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42 kJ/mol
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62 kJ/mol
Correct Answer
A. 62 kJ/molExplanation
The given answer of 62 kJ/mol suggests that the enthalpy change for the sublimation of iodine is 62 kilojoules per mole.Rate this question:
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- 3.
What is the standard enthalpy change, , for the reaction represented above? ( for is 230 kJ/mol; of is 83 kJ/mol.)
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-607 kJ
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-147 kJ
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-19 kJ
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+19 kJ
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+773 kJ
Correct Answer
A. -607 kJExplanation
The standard enthalpy change for the reaction represented above is -607 kJ. This value is obtained by subtracting the enthalpy of the reactants (230 kJ/mol) from the enthalpy of the products (83 kJ/mol). The negative sign indicates that the reaction is exothermic, meaning it releases heat to the surroundings.Rate this question:
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- 4.
A 6.22-kg piece of copper metal is heated from 20.5 degrees celsius to 324.3 degrees celsius. Calculate the heat absorbed (in kJ) by the metal. The specific heat of copper is 0.385 J/g*C
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49.1 kJ
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728 kJ
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0.728 kJ
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0.0491 kJ
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777 kJ
Correct Answer
A. 728 kJExplanation
The heat absorbed by an object can be calculated using the formula: Q = mcΔT, where Q is the heat absorbed, m is the mass of the object, c is the specific heat capacity of the material, and ΔT is the change in temperature. In this case, the mass of the copper is given as 6.22 kg, the specific heat capacity of copper is given as 0.385 J/g*C, and the change in temperature is (324.3 - 20.5) = 303.8 degrees Celsius. Converting the mass to grams, we get 6220 g. Plugging these values into the formula, we get Q = (6220 g)(0.385 J/g*C)(303.8 C) = 728 kJ. Therefore, the heat absorbed by the metal is 728 kJ.Rate this question:
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- 5.
A 0.1375 g sample of solid magnesium is burned in a calorimeter that has a heat capacity of 3024 J/*C. If temperature increases by 1.126*C, calculate the enthalpy of the combustion of magnesium.
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73.51 kJ/mol
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602.0 J/mol
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27.76 J/mol
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602.0 kJ/mol
Correct Answer
A. 602.0 kJ/molExplanation
The enthalpy of the combustion of magnesium can be calculated using the formula:
Enthalpy change = (heat capacity of calorimeter * temperature change) / mass of magnesium
In this case, the heat capacity of the calorimeter is given as 3024 J/°C, the temperature change is given as 1.126°C, and the mass of magnesium is 0.1375 g. Plugging these values into the formula, we get:
Enthalpy change = (3024 J/°C * 1.126°C) / 0.1375 g
Simplifying the equation, we find:
Enthalpy change = 602.0 J/mol
Therefore, the enthalpy of the combustion of magnesium is 602.0 J/mol.Rate this question:
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Current Version
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Mar 21, 2023Quiz Edited by
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Sep 10, 2014Quiz Created by
Ashley Vickers
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