Using the standard molar heat of combustion of hydrogen, methane, and ethane (given below), find the...
Homework Answers
Given reactions are :
H2 + ½ O2 → H2O ΔHo = -285.8 kJ......(1)
CH4 + 2O2 → CO2 + 2H2O ΔHo = -890.4 kJ . .....]*2
2CH4 + 4O2 → 2CO2 + 4H2O ΔHo = -1780.8 kJ.....(2)
C2H6 + (7/2)O2 → 2CO2 + 3H2O ΔHo = -1559.9 kJ....(3)
Subtracting (1) and (3) from (2) , we get
2CH4 + 4O2 - H2 - ½ O2 - C2H6 - (7/2)O2 → 2CO2 + 4H2O - 2CO2 - 3H2O - H2O ΔHo = -1780.8 kJ +285.8 + 1559.9 kJ
2CH4 → H2 + C2H6 ΔHo = 64.9 kJ
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Using the standard molar heat of combustion of hydrogen,
methane, and ethane (given below), find the...
Calculate the change in enthalpy (ΔH) for the heat of formation of ethane, C2H6, using Hess' Law and the following reactions:
Calculate the change in enthalpy (ΔH) for the heat of formation of ethane, C2H6, using Hess' Law and the following reactions:a) 2C(S) + 2O2(g) → 2CO2(g), ΔH = -188 kcalb) C2H6(g) + (7/2)O2(g) → 2CO2(g) + 3H2O(l), ΔH = -373 kcalc) H2(g) + (1/2)O2(g) → H2O(l), ΔH = -68.3 kcal
Part 1) Use the following equations to calculate the heat of the reaction for the formation...
Part 1) Use the following equations to calculate the heat of the reaction for the formation of ethane (C2H6). C2H6(g) + 7/2 O2(g) → 2CO2(g) + 3 H2O(l) ∆ Ho = -1560 kJ C(gr) + O2(g) → CO2(g) ∆ Ho = -394 kJ H2(g) + 1/2 O2(g) → H2O(l) ∆ Ho = -286 kJ Calculate ∆Ho for the following reaction: 2 C(gr) + 3H2(g) → C2H6(g) ethane Use kJ for your answer. ΔHo = Part 2) Find the heat of...
3. Calculate the standard enthalpy change (AHº) for the combustion of methane given the following data:...
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...
please explain each step in clear writing. Chloroform (CHCI3) is formed from methane and chlorine in...
please explain each step in clear writing.
Chloroform (CHCI3) is formed from methane and chlorine in the following reaction: CH4 (g)3C12 (g)3HC1(g)+CHCI3 (g) Calculate A, Ho, the enthalpy change for this reaction, using the standard molar enthalpy change of formation of CHCI3 (g), AfH° = -103.1 kJ mol1, and the standard enthalpy changes for the following reactions: CH4 (g)202 (g)2H2O (e) CO2 (g) AH°=-890.4 kJ mol-1 2HC1(g) H2 (g)Cl2 (g) A,.H +184.6 kJ mol1 C(graphite)O2 (g)CO2 (g) A H°=-393.5 kJ...
The conversion of methane into products that contain two or more carbon atom, such as ethane,...
The conversion of methane into products that contain two or more
carbon atom, such as ethane, C2H2, is a very
important industrial chemical process. In principle, methane can be
converted directly into ethane and hydrogen.
(1) 2CH4(g) C2H6(g) +
H2(g)
In practice, however, this reaction is carried out in the
presence of oxygen:
(2) 2CH4(g) + 1/2 O2(g) C2H6(g) +
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The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O2(g) → 2 CO2(g) + 3 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. reaction (1): C(s) + O2(g) → CO2(g) ΔH = −393.5 kJ/mol reaction (2): H2(g) + 1/2 O2(g) → H2O(l) ΔH = −285.8 kJ/mol reaction (3): 2 C(s) + 3 H2(g) → C2H6(g) ΔH = −84.0 kJ/mol
The experimentally determined heat of combustion of methane is 50.1 kJ/g. Calculate the heat of combustion...
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 formation of gaseous methane (CH4) using the following thermochemical information: CO2(g)...
Calculate the standard enthalpy of formation of gaseous methane
(CH4) using the following thermochemical
information:
CO2(g) + 2
H2O(l) CH4(g) + 2 O2(g)
H = +890.4 kJ
CO2(g) C(s) + O2(g)
H = +393.5 kJ
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Natural gas is mostly methane, but it also contains some ethane and propane. The enthalpies of...
Natural gas is mostly methane, but it also contains some ethane and propane. The enthalpies of combustion of methane, ethane and propane are -810, -1420, and -2030 kJ mol-1, respectively. (A) Complete the chemical reactions for the combustion of these fuels and calculate the amount of heat released per mole of oxygen and carbon dioxide produced for the three gases using the enthalpy of the reaction. i. For methane: CH4 + O2 -> ___________ Heat released per...
Calculate the approximate enthalpy change, ?Hrxn, for the combustion of one mole of methane a shown...
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
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...
please explain each step in clear writing.
Chloroform (CHCI3) is formed from methane and chlorine in the following reaction: CH4 (g)3C12 (g)3HC1(g)+CHCI3 (g) Calculate A, Ho, the enthalpy change for this reaction, using the standard molar enthalpy change of formation of CHCI3 (g), AfH° = -103.1 kJ mol1, and the standard enthalpy changes for the following reactions: CH4 (g)202 (g)2H2O (e) CO2 (g) AH°=-890.4 kJ mol-1 2HC1(g) H2 (g)Cl2 (g) A,.H +184.6 kJ mol1 C(graphite)O2 (g)CO2 (g) A H°=-393.5 kJ...
The conversion of methane into products that contain two or more
carbon atom, such as ethane, C2H2, is a very
important industrial chemical process. In principle, methane can be
converted directly into ethane and hydrogen.
(1) 2CH4(g) C2H6(g) +
H2(g)
In practice, however, this reaction is carried out in the
presence of oxygen:
(2) 2CH4(g) + 1/2 O2(g) C2H6(g) +
H2O(g)
a) Using the thermodynamic data at 298K, determine ΔG° for each
reaction.
ΔGf° (kJ/mol)
ΔGf° (kJ/mol)
CH4(g)
H2(g)
0...
Calculate the standard enthalpy of formation of gaseous methane
(CH4) using the following thermochemical
information:
CO2(g) + 2
H2O(l) CH4(g) + 2 O2(g)
H = +890.4 kJ
CO2(g) C(s) + O2(g)
H = +393.5 kJ
2 H2O(l) 2 H2(g) + O2(g)
H = +571.7 kJ
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