The standard enthalpy of formation, ΔHf0, for N2O4 is the enthalpy change for which reaction?
a. 2NO(g) + O2(g) → N2O4(g)
b. 2NO2(g) → N2O4(g)
c. 2N(g) + 4O(g) → N2O4(g)
d. N2(g) + 2O2(g) → N2O4(g)
e. N2O(g) + O3(g) → N2O4(g)
Enthalpy of formation of a compound is the enthalpy of the reaction in which one mole of the required compound is formed from the reactants having enthalpy of formation 0.
In thermodynamics , all elements in their standard states (Oxygen gas (O2) , Nitrogen gas(N2), graphite form of solid carbon etc ) have a standard enthalpy of formation zero , as there is no change involved in their formation , or we can say it takes no energy to form a naturally-occuring compound.
Now, ΔHfo, for N2O4 is the enthalpy change for
reaction involving only O2 and N2 in the reactant side .
Thus d is the correct answer. (N2(g) + O2(g) →
N2O4(g)).
The standard enthalpy of formation, ΔHf0, for N2O4 is the enthalpy change for which reaction? a....
5.84 for which of the following reactions does delta H degree run represent an enthalpy of formation? A) 2N2(g) + 3O2(g) —-> 2NO(g) + 2NO(g) B) N2(g) + O2(g) —> 2NO (g) C) 2NO2(g) —> N2O4(g) D) N2(g) + 2O2(g) —> 2NO2 (g)
Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) Given the following reactions and enthalpies of formation: N2(g) + 2O2(g)→ 2NO2(g), ΔH∘ = 66.4kJ N2(g)+ O2(g)→ 2 NO(g), ΔH∘=180.4 kJ Please explain the steps as well!
A.Using standard heats of formation, calculate the standard enthalpy change for the following reaction. N2(g) + 3H2(g) = 2NH3(g) B.Using standard heats of formation, calculate the standard enthalpy change for the following reaction. CaCO3(s) = CaO(s) + CO2(g) C. A scientist measures the standard enthalpy change for the following reaction to be -2910.6 kJ: 2C2H6(g) + 7 O2(g) = 4CO2(g) + 6 H2O(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy...
Using standard heats of formation, calculate the standard enthalpy change for the following reaction. 2NH3(g) + 2O2(g)N2O(g) + 3H2O(l) kJ
The standard enthalpy of formation of NO(g) is +90.3 kJ·mol-1 and that of NO2(g) is +33.2 kJ·mol-1. Calculate the reaction enthalpy for 2NO(g) + O2(g) ® 2NO2(g) A. -47.8 kJ B. -57.1 kJ C. +123.5 kJ D. -23.9 kJ E. -114.2 kJ Please explain why/steps.
Using standard heats of formation, calculate the standard enthalpy change for the following reaction. 2NO(g) + 2H2(g) N2() + 2H20(1) ANSWER: Submit Answer
2. Use the thermochemical equations shown below to determine the enthalpy for the final reaction: Nz (e) + 2O2 (g) → N204 (g) AH = ? Using: (1) 2NO2(g) → N2 (g) +202 (8) AH = -66.4 kJ (2) N2O. (g) → 2NO, (e) AH = 57.2 kJ
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) NO(g) 90.2 O2(g) 0 NO2(g) 33.2 Then the standard heat...
Based on the standard free energies of formation, which of the following reactions represent a feasible way to synthesize the product? A. N2(g)+2O2(g)?2NO2(g); ?G?f=102.6 kJ/mol B. 2Na(s)+O2(g)?Na2O2(s); ?G?f=?451.0 kJ/mol C. N2(g)+O2(g)?2NO(g); ?G?f=173.2 kJ/mol D. 2CO(g)+O2(g)?2CO2(g); ?G?f=?788.0 kJ/mol
Given the standard enthalpy changes for the following two reactions: (1) N2(g) + O2(g) +2NO(g) AH° = 181.8 kJ (2) N2(g) + 202(g)—>2NO2(g) AH° = 66.4 kJ what is the standard enthalpy change for the reaction: (3) 2NO(g) + O2(g) 2NO2(g) AH° = ? Submit Answer Try Another Version 2 item attempts remaining