Why are fractional coefficients permitted in a balanced thermochemical equation? Fractional coefficients are permitted in order to have the smallest possible set of coefficients for a given reaction. Fractional coefficients are permitted because the enthalpy change for the reaction is dependent on the amount of matter present. Fractional coefficients are permitted because the enthalpy change for the reaction is independent of the amount of matter present. In thermochemical reactions, only small amounts of matter are considered. O If fractional coefficients were not used, the scale of the reaction would be excessively large.

Why are fractional coefficients permitted in a balanced thermochemical equation? Fractional coefficients are permitted in order to have the smallest possible set of coefficients for a given reaction. Fractional coefficients are permitted because the enthalpy change for the reaction is dependent on the amount of matter present. Fractional coefficients are permitted because the enthalpy change for the reaction is independent of the amount of matter present. In thermochemical reactions, only small amounts of matter are considered. O If fractional coefficients were not used, the scale of the reaction would be excessively large.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 58QAP: Consider the following reaction in the vessel described in Question 57. A(g)+B(g)C(s)For this...

See similar textbooks

Related questions

Q: A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains…

Q: with 2 mol O2 (g) to produce 1 mol CO2 (g), 2 mol H2O(l), and 890 kJ of heat. Write a…

A: when any substance which burns in presence of oxygen that reaction is called as combustion reaction.…

Q: During a certain chemical reaction 1,395 J of heat is released from the system and 360 J of work is…

A: Given :- work done on surrounding = 360 J heat released from system = 1395 J To be calculated :-…

Q: A metal object with mass of 29.0 g is heated to 97.0 °C and then transferred to an insulated…

A: Since the heat lost by metal + heat gain by water should be = 0 as no heat is lost in surroundings…

Q: A 2.74-g sample of a substance suspected of being pure gold is warmed to 72.1 °C and submerged into…

Q: Answer the problems and show complete solutions. 1. Explain the difference between heat capacity and…

A: The relation between heat energy and specific heat is given by Q = mCΔT Q = heat energy m = mass of…

Q: A 29.8 g sample of water at 4.7 C is mixed with 52.5 g of water at 74.8 C. Calculate the final…

A: Given data,Mass of water(1)=29.8gTemperature(T1)=4.7oCMass of…

Q: A 55.2 g piece of metal has a temperature of 90.4 °C before being placed into 102.5 g of water at…

A: Given details, For metal, Mass (m) = 55.2 g T1 = 90.4°CT2 = 24.7°C ∆T=(T2-T1)=65.7°C For water, Mass…

Q: Specific Heat Capacity A 24.5-g sample of an unknown metal is heated to 97.5°C and is placed in a…

A: Given that: Mass of metal = 24.5 g Initial temperature of metal = 97.5°C Mass of water = 164 g…

Q: A system receives 450 kJ of heat from its surroundings and the surroundings do 50.0 kJ of work on…

A: Given: Heat (q) = +450KJ The sign is positive because it absorbs from the surrounding.…

Q: Ignition wires heat Thermometer A bomb calorimeter, or constant volume calorimeter, is a device…

A: Given: mass of 1,6-hexanediol = 0.520 g mass of water = 1090 g Initial temperature = 24.30 oC Final…

Q: The reaction between sodium metal and chlorine gas produces 822 kJ of heat energy for every chlorine…

Q: An 18.89 g sample of neon gas in a container with a movable wall is initially at a temperature of…

A: GIVEN: Mass of Neon gas = 18.89 g Initial Temperature (T1)= 320 K Final Temperature (T2)= 405 K…

Q: For an exothermic reaction, how is the measured temperature change affected if some of the heat…

A: Consider that an exothermic reaction is taking place inside a calorimeter with water as its…

Q: For a process at constant pressure, 6.20 x 10* calories of heat are released. This quantity of heat…

A: Inorder to convert kilocalorie to joule, multiply the energy value by 4184. So, 1 kcal = 4184 J 1…

Q: A 30.0 g sample of chromium is heated to 100.0 °C in a boiling water bath. The sample is added to a…

Q: The enthalpy change when a strong acid is neutralized by strong base is –56.1 kJ/mol. If 12.0 mL of…

A: Given : concentration of HBr = 6 M and volume of HBr solution = 12 mL = 0.012 L…

Q: How much heat (in kJ) is evolved (under standard conditions) when 97.55 g of copper reacts to form…

A: Mass of copper, Cu = 97.55 g Amount of heat evolved during formation of copper (II) oxide, CuO from…

Q: The ΔH value for the reaction is -90.8 kJ. How much heat is released when 198.1 g Hg is reacted with…

A: Reaction involved :- 2Hg + O2 = 2HgO

Question

Why are fractional coefficients permitted in a balanced thermochemical equation?
Fractional coefficients are permitted in order to have the smallest possible set of coefficients for a given reaction.
Fractional coefficients are permitted because the enthalpy change for the reaction is dependent on the amount of matter present.
Fractional coefficients are permitted because the enthalpy change for the reaction is independent of the amount of matter present.
In thermochemical reactions, only small amounts of matter are considered.
O If fractional coefficients were not used, the scale of the reaction would be excessively large.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

Determine whether the statements given below are true or false. Consider an endothermic process taking place in a beaker at room temperature. (a) Heat flows from the surroundings to the system. (b) The beaker is cold to the touch. (c) The pressure of the system decreases. (d) The value of q for the system is positive.
If a student performs an endothermic reaction in a calorimeter, how does the calculated value of H differ from the actual value if the heat exchanged with the calorimeter is not taken into account?
Graphite 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?
9.58 For the reaction C2H2(g)+2H2(g)C2H6,H=136 kJ. What are the ratios that can be defined between moles of substances and energy?
Explain why the specific heat of the contents of the calorimeter must be known in a calorimetry experiment.
Using the data in Appendix G, calculate the standard enthalpy change for each of the following reactions: (a) Si(s)+2F2(g)SiF4(g) (b) 2C(s)+2H2(g)+O2(g)CH3CO2H(l) (c) CH4(g)+N2(g)HCN(g)+NH3(g) ; (d) CS2(g)+3Cl2(g)CCl4(g)+S2Cl2(g)
In the process of isolating iron from its ores, carbon monoxide reacts with iron(III) oxide, as described by the following equation: Fe2O3(s)+3CO(g)2Fe(s)+3CO2(g)H=24.8kJ The enthalpy change for the combustion of carbon monoxide is 2CO(g)+O2(g)2CO2(g)H=566kJ Use this information to calculate the enthalpy change for the equation 4Fe(s)+3O2(g)2Fe2O3(s)H=?
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)?
What mass of acetylene, C2H2(g), must be burned to produce 3420 kJ of heat, given that its enthalpy of combustion is 1301 kJ/mol? Compare this with the answer to Exercise 5.91 and determine which substance produces more heat per gram.
Differentiate between the enthalpy of formation of H2O(l)andH2O(g) . Why is it necessary to specify thephysical state of water in the following thermochemicalequation CH4(g)+2O2(g)CO2(g)+2H2O(lorg)H=?
A _________ is a device used to determine the heat associated with a chemical reaction.
The combustion of 1.00 mol liquid methyl alcohol (CH3OH) in excess oxygen is exothermic, giving 727 kJ of heat. (a) Write the thermochemical equation for this reaction. (b) Calculate the enthalpy change that accompanies the burning 10.0 g methanol. (c) Compare this with the amount of heat produced by 10.0 g octane, C8H18, a component of gasoline (see Exercise 5.41).

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS