how do you get the enthalpy for each compound? ex: CO2 is -393.5 kj/mol where did that number come from
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
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 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)
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...
. 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
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
I do not understand how to find the equation for the x-axis. Where did you get the components from?
3. The enthalpy of solution for sodium chloride is +4 kJ/mol while that of silver chloride is +65 kJ/mol. (a) Based on the enthalpies of solution and assuming that the change in entropy for the solution process is the same for each compound, which compound do you expect to be more soluble? Why? (b) Using enthalpy of hydration data from the appendix, calculate values for the two lattice enthalpies. (c) Estimate values for the lattice energies using the Born-Landé equation...