how do you get the enthalpy for each compound? ex: CO2 is -393.5 kj/mol where did...
how do you get the enthalpy for each compound? ex: CO2 is -393.5 kj/mol where did that number come from
Homework Answers
Experimentally Enthalpy each compound is calculated using Bomb Calorimeter.
dH = nCpdT
where dT is the change in temperature
This enthalpy is mainly combustion enthalpy from which we can calculate other enthalpy
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how do you get the enthalpy for each compound? ex: CO2 is -393.5
kj/mol where did...
7. The enthalpy of combustion of C to CO2 is –393.5 kJ/mol C, and the enthalpy...
7. The enthalpy of combustion of C to CO2 is –393.5 kJ/mol C, and the enthalpy of combustion of Co to CO2 is -283.0 kJ/mol CO: C(s) + O2(g) + CO2(g) AH = -393.5 kJ CO(g) + 102(9) CO2(g) AH = -283.0 kJ Using these data, calculate the enthalpy of combustion of C to CO: C(s) + O2(g) → CO(g) AH = ? Answer: -110.5 kJ
[32] The enthalpy of reaction for [6] enthalpy of reaction for the combustion of C to CO, is-393.5 kJ/mol C, and th...
[32] The enthalpy of reaction for [6] enthalpy of reaction for the combustion of C to CO, is-393.5 kJ/mol C, and the enthalpy for the combustion of CO to CO, is-283.0 kJ/mol CO: (i) C(s) + O2(g) + CO2(e) AH -393.5 kJ CO(g) + O2(g) + CO2(g) AH -283.0 kJ Using these data, calculate the enthalpy for the combustion of C to CO. (iii) C(s) + O2(g) - CO(g) AH-?
From the following data, C(graphite) + O2(g) → CO2(g) AHrxn = -393.5 kJ/mol H2(g) + O2(g)...
From the following data, C(graphite) + O2(g) → CO2(g) AHrxn = -393.5 kJ/mol H2(g) + O2(g) → H200) AH"rxn = -285.8 kJ/mol 2C2H6(g) + 702(g) -> 4CO2(g) + 6H2O(l) Arxn=-3119.6 kJ/mol Calculate the enthalpy change for the reaction: 2 C(graphite) + 3H2(g) + C2H668)
Given: C(s) + O2(g) ---> CO2(g) ΔH = −393.5 kJ/mol S(s) + O2(g) ---> SO2(g) ΔH...
Given: C(s) + O2(g) ---> CO2(g) ΔH = −393.5 kJ/mol S(s) + O2(g) ---> SO2(g) ΔH = −296.8 kJ/mol C(s) + 2S(s) ---> CS2(ℓ) ΔH = +87.9 kJ/mol A) Calculate the standard enthalpy change for the following reaction CS2(ℓ) + 3O2(g) ---> CO2(g) + 2SO2(g) ΔH° rxn = -1075 kJ/mol B) Using the equation and standard enthalpy change for the reaction (from part A), calculate the amount of heat produced or consumed when 3.2 mol of CS2 reacts with excess...
If the enthalpy of sublimation for CO2 is 26.1 kJ/mol, what is the enthalpy of deposition...
If the enthalpy of sublimation for CO2 is 26.1 kJ/mol, what is the enthalpy of deposition for CO2? Your answer should have three significant figures (round your answer to one decimal place). Do not include units in your response.
. For the reaction C(s)+O2(g) CO2(g), AH = -393.5 kJ/mol. What is the amount of heat...
. For the reaction C(s)+O2(g) CO2(g), AH = -393.5 kJ/mol. What is the amount of heat (in kJ) produced during the combustion of 34.56 g of coal (pure carbon)? pec To abiod to yedmun Decide whether each of these reactinns is exothorm
Incorrect. Did you remember to multiply the enthalpy values by the stoichiometric coefficients? Did you...
Incorrect. Did you remember to multiply the enthalpy values by the stoichiometric coefficients? Did you do enthalphy of products minus enthalphy of reactants? a) CH4(g)+C2(g) CH3Cl(g) +HCI(g) The number of significant digits is set to 3; the tolerance is +/-2 % x Incorrect. Did you remember to multiply the enthalpy values by the stoichiometric coefficients? Did yoif do enthalphy of products minus enthalphy of reactants? co(NH2) 2(s) + H20() b) 2NH3(g) + Co2(g) kJ The number of significant digits is...
Given the following Thermodynamic data: CO2(g) H2O(l) NH3(g) CO(NH2)2(s) DeltaHof (kJ/mol): -393.5 -285.85 -45.9 -333.2 So...
Given the following Thermodynamic data: CO2(g) H2O(l) NH3(g) CO(NH2)2(s) DeltaHof (kJ/mol): -393.5 -285.85 -45.9 -333.2 So (J/K.mol): 214 70 193 105 (a) Calculate DeltaHo, DeltaSo, and DeltaGo at 25oC for the following reaction: CO2(g) + 2NH3(g) = CO(NH2)2(s) + H2O(l) (b) What is DeltaGo at 250oC? (Assume DeltaHo and DeltaSo do not change with temperature.) (c) Is the reaction spontaneous at each temperature? (Answer: (a) DeltaHo = -133.8 kJ; DeltaSo = -425 J/K; DeltaGo = -7.15 kJ; (b) DeltaGo =...
Please Explain how to get the answer if you can! Enter your answer in the provided...
Please Explain how to get the answer if you can!
Enter your answer in the provided box. Acetylene burns in air according to the following equation: CH99)+0302 C029) + H206) AH = -1255.8 kJ I'xn Given sy of CO2(9)=–393.5 kJ/mol and sH of H2O(g)--241.8 kJ/mol, find all of C_H28). kJ/mol
calculate the standard enthalpy change (in kJ/mol) for each of the following reactions. Ni(s) + Cl2(g)...
calculate the standard enthalpy change (in kJ/mol) for each of the following reactions. Ni(s) + Cl2(g) → NiCl2(s) kJ/mol B2O3(s) + 3 H2(g) → 2 B(s) + 3 H2O(l) kJ/mol 2 KOH(s) + CO2(g) → K2CO3(s) + H2O(g) kJ/mol 2 Cu(s) + Cl2(g) → 2 CuCl(s) kJ/mol
7. The enthalpy of combustion of C to CO2 is –393.5 kJ/mol C, and the enthalpy of combustion of Co to CO2 is -283.0 kJ/mol CO: C(s) + O2(g) + CO2(g) AH = -393.5 kJ CO(g) + 102(9) CO2(g) AH = -283.0 kJ Using these data, calculate the enthalpy of combustion of C to CO: C(s) + O2(g) → CO(g) AH = ? Answer: -110.5 kJ
[32] The enthalpy of reaction for [6] enthalpy of reaction for the combustion of C to CO, is-393.5 kJ/mol C, and the enthalpy for the combustion of CO to CO, is-283.0 kJ/mol CO: (i) C(s) + O2(g) + CO2(e) AH -393.5 kJ CO(g) + O2(g) + CO2(g) AH -283.0 kJ Using these data, calculate the enthalpy for the combustion of C to CO. (iii) C(s) + O2(g) - CO(g) AH-?
From the following data, C(graphite) + O2(g) → CO2(g) AHrxn = -393.5 kJ/mol H2(g) + O2(g) → H200) AH"rxn = -285.8 kJ/mol 2C2H6(g) + 702(g) -> 4CO2(g) + 6H2O(l) Arxn=-3119.6 kJ/mol Calculate the enthalpy change for the reaction: 2 C(graphite) + 3H2(g) + C2H668)
. For the reaction C(s)+O2(g) CO2(g), AH = -393.5 kJ/mol. What is the amount of heat (in kJ) produced during the combustion of 34.56 g of coal (pure carbon)? pec To abiod to yedmun Decide whether each of these reactinns is exothorm
Incorrect. Did you remember to multiply the enthalpy values by the stoichiometric coefficients? Did you do enthalphy of products minus enthalphy of reactants? a) CH4(g)+C2(g) CH3Cl(g) +HCI(g) The number of significant digits is set to 3; the tolerance is +/-2 % x Incorrect. Did you remember to multiply the enthalpy values by the stoichiometric coefficients? Did yoif do enthalphy of products minus enthalphy of reactants? co(NH2) 2(s) + H20() b) 2NH3(g) + Co2(g) kJ The number of significant digits is...
Please Explain how to get the answer if you can!
Enter your answer in the provided box. Acetylene burns in air according to the following equation: CH99)+0302 C029) + H206) AH = -1255.8 kJ I'xn Given sy of CO2(9)=–393.5 kJ/mol and sH of H2O(g)--241.8 kJ/mol, find all of C_H28). kJ/mol
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