Calculate the approximate enthalpy change, ?Hrxn, for the combustion of one mole of methane a shown in the balanced chemical equation: CH4+2O2?2H2O+CO2 Use the values you calculated in Parts A, B, C, and D, keeping in mind the stoichiometric coefficients.
delta H CH4=1656 kJ/mol
delta H O2=498 kJ/mol
delta H H2O=-928 kJ/mol
delta H CO2=-1598 kJ/mol
Combustion reactions:
The chemical reaction in which an organic compound or hydrocarbon (H and C) burns with oxygen and forms water and carbon dioxide is represented as combustion reaction. The combustion reaction is exothermic reaction in which heat releases in the form of energy.
Bond enthalpy:
Bond enthalpy is one of the thermodynamic quantities that measures the bond strength in the molecules (energy stored in the form of chemical bond). It is defined as the amount of energy that is needed for breaking the chemical bonds in the molecules. It is also known as average bond energy or bond dissociation enthalpy. It is usually expressed in.
The arbitrary reaction is given below:
Here
and are the reactants.
is the product.
The approximate enthalpy change for the gas phase reaction can be estimated by the following formula:
Here
indicates the bond dissociation energy of reactants
indicates the bond dissociation energy of products.
represents the bond dissociation energy.
In the above formula, n and m are the coefficients of reactants and products, respectively.
Stoichiometric coefficients:
A stoichiometric coefficient is a simple whole number that is used to determine the relative number of moles or molecules in a balanced chemical equation.
The given combustion reaction of methane is as follows:
In the above reaction, methane burns with oxygen to form carbon dioxide and water as products.
The given balanced chemical equation is as follows:
Use the following equation to calculate the change in enthalpy for the given combustion reaction of one mole of methane.
Substitute the values of the substances.
Ans:
Hence, the approximate enthalpy change,, for the combustion of one mole of methane is .
Calculate the approximate enthalpy change, ?Hrxn, for the combustion of one mole of methane a shown...
Part ACalculate the bond energy per mole for breaking all the bonds in methane, CH4.Express your answer to four significant figures and include the appropriate units.ΔHCH4 =1656 kJmolCorrectIn CH4, the energy required to break one C−H bond is 414 kJ/mol. Since there are four C−H bonds in CH4, the energy ΔHCH4 for breaking all the bonds is calculated asΔHCH4=4×bond energy of C−H bond=4×414 kJ/mol=1656 kJ/mol CH4 moleculesPart BCalculate the bond energy per mole for breaking all the bonds of oxygen,...
Part E Calculate the approximate enthalpy change , ?H?, for the combustion of methane: CH4+2O2?2H2O+CO2 Use the values you calculated in Parts A to D, keeping in mind the stoichiometric coefficients. Please explain.
3. Calculate the standard enthalpy change (AHº) for the combustion of methane given the following data: AH° = -232.4 kJ CH4(g) + O2(g) → CH2O(g) + H20 (g) CH20 (g) + O2(g) → CO2(g) + H2O(g) AH° = -343.5 kJ 3. Calculate the standard enthalpy change (AHº) for the combustion of methane given the following data: AH° = -232.4 kJ CH4(g) + O2(g) → CH2O(g) + H20 (g) CH20 (g) + O2(g) → CO2(g) + H2O(g) AH° = -343.5 kJ...
How many moles of water vapor are produced for every mole of methane consumed in the combustion reaction: CH4(g) + 2O2(g) --> CO2(g) + 2H2O(g) What is the mole coefficient for NO if its reaction is correctly balanced? NO(g) + O2(g) + H2O(l) --> HNO2(g)
Use the example shown to calculate the reaction enthalpy, delta H, for the following reaction: CH4(g)+2O2(g)->CO2(g)2H2O(l). Use the series of reaction that follows: 1. C(s)+2H2(g)-> CH4(g), delta H= -74.8 kJ 2. C(s)+O2(g)->CO2(g), delta H= -393.5 kJ 3. 2H2(g)+O2(g)-> 2H2O(g), delta H= -484.0 kJ 4. H2O(l)->H2O(g), delta H= 44.0 kJ
The experimentally determined heat of combustion of methane is 50.1 kJ/g. Calculate the heat of combustion of methane in kJ/mol. Molar mass of methane CH4 = 16 g/mol CH4(g) + 2 O2(g) → CO2 (g) + 2 H2O(l)
Calculate the standard enthalpy of reaction for the combustion of propane. NOTE: This equation is not balanced. Round to the nearest whole number. C3H8(g) + O2 --> CO2(g) + H2O(l) kJ/mol Compound Hf (kJ/mole) C3H8(g) -105 CO2(g) -394 H2O(l) -284
Heres the question, show work please! Calculate the enthalpy of combustion per mole for C6H12O6. Assume that the combustion products are CO2(g) and H2O(l). Calculate the enthalpy of combustion per mole for C6H12O6. Assume that the combustion products are CO2(g) and H2O(l). -2816 kJ/mol -5336 kJ/mol -1939 kJ/mol 580.7 kJ/mol Heres the question, show work please! Calculate the enthalpy of combustion per mole for C6H12O6. Assume that the combustion products are CO2(g) and H2O(l).
CH_(g) + 2O2(g) → CO2(g)+ 2H2O(1) AH = -890.4 kJ When 1 mole of CO2(g) is produced, what is the enthalpy change? When 3 mol of O, is reacted with an excess of CH4, what is the enthalpy change? When 1 mole of H,O(l) is produced, what is the enthalpy change?
For the combustion of methane(CH4) CH4 (g) + 2 O2 (g) --> CO2 (g) + 2H2O (g) Δ H = -882 kJ/mol If 250.0 g of CH4 is burned , what is the energy change? ( Answers in scientific notation are entered such as 1.234 e4 )