the work for the problem/reasoning is zero for 14) For calculating the enthalpy of combustion of...
For the combustion reaction of methane, AHºf is zero for CH4 (g) + O2 (g) → 2H2O(g) + CO2 (g) A) 02 (g) B) CH4 (g) CO2 (g) D) H20 (g) E) Both O2 (g) and CH4 (g) 8 Given the following reactions N2 (g) + 202 (g) - 2NO2 (g) AH = 66.4 kJ 2NO (g) + O2 (g) → 2NO2 (g) AH = -114.2 kJ the enthalpy of the reaction of the nitrogen to produce nitric oxide N2...
URGENT Given the following data, calculate the enthalpy change of combustion for 2.5mol of nitromethane. [5A] overall reaction: 4CH3NO2(g)+3O2(g)-->4CO2(g)+2N2(g)+6H 20 (1) C(g)+O2(g)-->CO2(g) AH=-393.5k) 2H2(g)+O2(g)--> 2H2O(g) AH=-483.6k) 2C(8)+3H2(g)+2O2(g)+N2(g)-->2CH3NO2(g) AH=-226.2k)
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...
4 For the combustion reaction of methane, AHºf is zero for CH4 (g) + O2 (g) → 2H2O(g) + CO2 (g) A) 02 (g) B) CH4 (g) C CO2 (g) B) H20 (g) E) Both O2 (g) and CH4 (g)
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.
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
Given the following thermochemical equation for the combustion of methane gas: CH4 (9) + 2O2 (g) → CO2 (g) + 2H20 (1) AH = -890 kJ How many grams of methane are required to produce 132 kJ of energy?
e In Canvas D Question 3 2 pts Complete combustion of 1 mole of acetone (C3H&O) liberates 1790 kJ. Which of the following equations (with their correct AH° values) would not need to be used in any form to determine the enthalpy of formation of acetone? O C(graphite) + O2(g) CO2(8) ○ 3CO2(g) + 3H20(I) → 402(g) + C3H6O(1) O C(graphite) + 1/202(8) CO(g) ○ 2H2(g) + O2(g)-→ 2H2O(l) Next 4 Previous
Please explain Data: C(graphite) + O2(g) => CO2(g) AH = -393.5 kJ H2(g) + 1/2O2(g) => H2O(1) AH = -285.8 kJ CH3OH(1) + 3/202(9) A CO2(g) + 2H20(1) AH = -726.4 kJ Using the data above, calculate the enthalpy change for the reaction below. Reaction: C(graphite) + 2H2(g) + 1/2O2(g) => CH3OH(1) A. +238.7 kJ B.-238.7 kJ C. +548.3 kJ D.-548.3 kJ E. +904.5 kJ
Which of these reactions demonstrate the enthalpy of atom combination? N(g)+3H(g)⟶NH3(g)N(g)+3H(g)⟶NH3(g) C(graphite)+2O2(g)⟶CO2(g)C(graphite)+2O2(g)⟶CO2(g) NO2(g)⟶N(g)+2O(g)NO2(g)⟶N(g)+2O(g) 2H2(g)+O2(g)⟶2H2O(g)2H2(g)+O2(g)⟶2H2O(g) C(g)+O(g)⟶CO(g)