Concept explainers
(a)
Interpretation:
For the given two reactants and the products under given set of conditions the balanced equation, moles, mole fraction of the reactant, the unreacted amount of given reactant, partial pressure of given compounds should be determined.
Concept Introduction:
Balanced Chemical Equation:
The
(a)
Answer to Problem 106IL
C3H8(g)+5O2(g)→3CO2(g)+4H2O(l)
Explanation of Solution
The given reactants C3H8(g) and O2(g) reacts in order to give set of products like CO2(g) and H2O(l). In order to obtain the balanced chemical reaction the number of atoms present in given reactant and products are analyzed and the suitable coefficients are included before them in order to obtain the balanced equation.
Observing given reactant and products 3 should be included before CO2(g) in order to get equal number of carbon atoms on both sides then, 4 should be included before H2O(l) in order to obtain equal number of hydrogen atom on both sides and finally, 5 should be included before O2(g) so that the number of oxygen atoms present are balanced on the both sides of the equation.
Therefore, the balanced chemical equation is C3H8(g)+5O2(g)→3CO2(g)+4H2O(l).
(b)
Interpretation:
For the given two reactants and the products under given set of conditions the moles, of given compounds should be determined.
Concept introduction:
Ideal gas equation:
Any gas is described by using four terms namely pressure, volume, temperature and the amount of gas. Thus combining three laws namely Boyle’s, Charles’s Law and Avogadro’s Hypothesis the following equation could be obtained. It is referred as ideal gas equation.
V ∝ nTP V = RnTPPV = nRTwhere,n = moles of gasP = pressureT = temperatureR = gas constant
Under some conditions gases don not behave like ideal gas that is they deviate from their ideal gas properties. At lower temperature and at high pressures the gas tends to deviate and behave like real gases.
Boyle’s Law:
At given constant temperature conditions the mass of given ideal gas in inversely proportional to its volume.
Charles’s Law:
At given constant pressure conditions the volume of ideal gas is directly proportional to the absolute temperature.
Avogadro’s Hypothesis:
Two equal volumes of gases with same temperature and pressure conditions tend to have same number of molecules with it.
The relationship between partial pressure and Ptotal is
Pi = χi Ptotalwhere, Pi = partial pressure χi = molefraction Ptotal=Totalpressure
(b)
Answer to Problem 106IL
The number of moles of given species is 0.3178moles.
Explanation of Solution
The number of moles present in the given amount of the substance is calculated as follows,
PV = nRT n = PVRT =5.1atm×1.50L0.0821×20oC=5.1atm×1.50L0.0821×(273.15+20) =7.650.0821×293.15=7.6524.07=0.3178moles.Since,Ptotal=Partialpressureof CO2(g)+Partialpressureof H2O(l) = 0.10atm+5.0atm = 5.1atm
(c)
Interpretation:
For the given two reactants and the products under given set of conditions the balanced equation, moles, mole fraction of the reactant, the unreacted amount of given reactant, partial pressure of given compounds should be determined.
Concept introduction:
Mole fraction: The mole fraction of denotes the individual presence of the component present in the given chemical reaction.
Consider general equation that contains reactants X and Y then the mole fraction of X is determined as follows,
Mole fraction of Mole fraction of one component = Moles of that componentTotal moles present in the reactionMole fraction of X = Number of moles of XNumber of moles of X + Number of moles of Y
The relationship between partial pressure and Ptotal is
Pi = χi Ptotalwhere, Pi = partial pressure χi = molefraction Ptotal=Totalpressure
(c)
Answer to Problem 106IL
The mole fraction for the given species is equal to 0.1667
Explanation of Solution
Consider the given chemical reaction and calculate the mole fraction of C3H8(g) as follows,
Before the reaction there are only reactants present in the flask.
Mole fraction of C3H8(g) = Number of moles of C3H8(g)Number of moles of C3H8(g) + Number of moles of O2(g) = 11+5 = 0.1667
(d)
Interpretation:
For the given two reactants and the products under given set of conditions the balanced equation, moles, mole fraction of the reactant, the unreacted amount of given reactant, partial pressure of given compounds should be determined.
Concept introduction:
Mole fraction: The mole fraction of denotes the individual presence of the component present in the given chemical reaction.
Consider general equation that contains reactants X and Y then the mole fraction of X is determined as follows,
Mole fraction of Mole fraction of one component = Moles of that componentTotal moles present in the reactionMole fraction of X = Number of moles of XNumber of moles of X + Number of moles of Y
The relationship between partial pressure and Ptotal is
Pi = χi Ptotalwhere, Pi = partial pressure χi = molefraction Ptotal=Totalpressure
(d)
Answer to Problem 106IL
The amount of unreacted oxygen in the reaction flask is equal to 0.28045 moles.
Explanation of Solution
PV = nRTInitial moles, nO2 = PVRT = 5×1.50L0.0821×293.15K=0.3116moles
Initial moles of oxygen is 0.3116moles
PV = nRTInitial moles, nC3H8 = PVRT = 0.1×1.50L0.0821×293.15K=6.23×10−3moles
From the given conditions it is clear that C3H8(g) acts as limiting reagent hence the unreacted oxygen is calculated by subtracting the amount of available amount of oxygen with the amount needed by the C3H8(g).
Amount of O2 needed by C3H8 = 6.23×10-3×5 = 0.0315molesExcess of O2 = 0.3116-0.03115 = 0.28045 moles of O2
(e)
Interpretation:
For the given two reactants and the products under given set of conditions the of given compounds should be determined.
Concept introduction:
Mole fraction: The mole fraction of denotes the individual presence of the component present in the given chemical reaction.
Consider general equation that contains reactants X and Y then the mole fraction of X is determined as follows,
Mole fraction of Mole fraction of one component = Moles of that componentTotal moles present in the reactionMole fraction of X = Number of moles of XNumber of moles of X + Number of moles of Y
The relationship between partial pressure and Ptotal is
Pi = χi Ptotalwhere, Pi = partial pressure χi = molefraction Ptotal=Totalpressure
(e)
Answer to Problem 106IL
The partial pressure exerted by the given gas in the system is 2.19 atm
Explanation of Solution
The partial pressure for the gas CO2 is calculated as follows,
Pi = χi PtotalPCO2 =Moles of CO2Total moles×Ptotal = 37×5.1 atm = 2.19 atm
(f)
Interpretation:
For the given two reactants and the products under given set of conditions the partial pressure of given compounds should be determined.
Concept introduction:
Mole fraction: The mole fraction of denotes the individual presence exerted by the component present in the given chemical reaction.
Consider general equation that contains reactants X and Y then the mole fraction of X is determined as follows,
Mole fraction of Mole fraction of one component = Moles of that componentTotal moles present in the reactionMole fraction of X = Number of moles of XNumber of moles of X + Number of moles of Y
The relationship between partial pressure and Ptotal is
Pi = χi Ptotalwhere, Pi = partial pressure χi = molefraction Ptotal=Totalpressure
(f)
Answer to Problem 106IL
The partial pressure exerted by the excess of oxygen after the reaction is 0.24 atm.
Explanation of Solution
The partial pressure for the unreacted oxygen is as follows,
Pi = χi PtotalPO2 =Moles of O2Total moles×Ptotal = 0.280456×5.1 atm = 0.24 atm
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Chapter 10 Solutions
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