(a)
Interpretation: The heat evolved for the production of 1.00 moles of
Concept Introduction:
(a)
Answer to Problem 34E
Energy released =
Explanation of Solution
Given reaction:
According to given reaction; 2 moles of
Hence the energy required for 1.00 moles of
(b)
Interpretation: The heat evolved during the reaction of 4.03 g hydrogen gas with excess of oxygen for the given reaction needs to be determined.
Concept Introduction: Thermodynamic is a branch of chemistry that deals with the energy change with the system and surroundings. It indicates the energy conversion and transfer between system and surroundings. At constant volume the change in heat for a system to change the internal energy is represented as ΔE or qV. At constant pressure the change in heat for a system to change the enthalpy is represented as ΔH or qp. The relation between
(b)
Answer to Problem 34E
Energy released =
Explanation of Solution
Given reaction:
Mass of
Molar mass of
Calculate moles of
According to given reaction; 2 moles of
Hence the energy required for 2.00 moles of
(c)
Interpretation: The heat evolved during the reaction of 186 g
Concept Introduction: Thermodynamic is a branch of chemistry that deals with the energy change with the system and surroundings. It indicates the energy conversion and transfer between system and surroundings. At constant volume the change in heat for a system to change the internal energy is represented as ΔE or qV. At constant pressure the change in heat for a system to change the enthalpy is represented as ΔH or qp. The relation between
(c)
Answer to Problem 34E
Energy released =
Explanation of Solution
Given reaction:
Mass of
Molar mass of
Calculate moles of
According to given reaction; 1 moles of
(d)
Interpretation: The heat evolved during the explosion of Hindenburg explosion which contains
Concept Introduction: Thermodynamic is a branch of chemistry that deals with the energy change with the system and surroundings. It indicates the energy conversion and transfer between system and surroundings. At constant volume the change in heat for a system to change the internal energy is represented as ΔE or qV. At constant pressure the change in heat for a system to change the enthalpy is represented as ΔH or qp. The relation between
(d)
Answer to Problem 34E
Energy released =
Explanation of Solution
Given reaction:
Volume of
Pressure = 1.0 atm
Temperature =
Molar mass of
Calculate moles of
According to given reaction; 2 moles of
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Chapter 9 Solutions
Chemical Principles
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- In a calorimetric experiment, 6.48 g of lithium hydroxide, LiOH, was dissolved in water. The temperature of the calorimeter rose from 25.00C to 36.66C. What is H for the solution process? LiOH(s)Li(aq)+OH(aq) The heat capacity of the calorimeter and its contents is 547 J/C.arrow_forwardGraphite is burned in oxygen to give carbon monoxide and carbon dioxide. If the product mixture is 33% CO and 67% CO2 by mass, what is the heat from the combustion of 1.00 g of graphite?arrow_forwardHow much would the temperature of 275 g of water increase if 36.5 U of heat were added?arrow_forward
- Enthalpy a A 100.-g sample of water is placed in an insulated container and allowed to come to room temperature at 21C. To heat the water sample to 41C, how much heat must you add to it? b Consider the hypothetical reaction,2X(aq)+Y(l)X2Y(aq)being run in an insulated container that contains 100. g of solution. If the temperature of the solution changes from 21C to 31C, how much heat does the chemical reaction produce? How does this answer compare with that in part a? (You can assume that this solution is so dilute that it has the same heat capacity as pure water.) c If you wanted the temperature of 100. g of this solution to increase from 21C to 51C, how much heat would you have to add to it? (Try to answer this question without using a formula.) d If you had added 0.02 mol of X and 0.01 mol of Y to form the solution in part b, how many moles of X and Y would you need to bring about the temperature change described in part c. e Judging on the basis of your answers so far, what is the enthalpy of the reaction 2X(aq) + Y(l) X2Y(aq)?arrow_forwardPropane, C3H8, is a common fuel gas. Use the following to calculate the grams of propane you would need to provide 369 kJ of heat. C3H8(g)+5O2(g)3CO2(g)+4H2O(g);H=2043kJarrow_forwardConsider the following reaction in the vessel described in Question 57. A(g)+B(g)C(s)For this reaction, E=286 J, the piston moves up and the system absorbs 388 J of heat from its surroundings. (a) Is work done by the system? (b) How much work?arrow_forward
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