Reference no: EM132776332

1. Calculate the standard enthalpy change, ΔH°rxn8NO(g) + 12H232, in kJ for the following chemical equation, using only the thermochemical equations below:

O(l) → 8NH(g) + 10O(g)

Report your answer to three significant figures in scientific notation.

Equations:     ΔH°_rxn (kJ)

1/2N₂(g) + 1/2O₂(g) → NO(g)    90.4

1/2N₂(g) + O₂(g) → NO₂(g)    33.8

4NH₃(g) + 7O₂(g) → 4NO₂(g) + 6H₂O(l)    -1326.2

2a The enthalpy of combustion (ΔH°_c) of 2-ethylbutanedioic acid (C₆H₁₀O₄) is -2801.00 kJ/mol. Using the appropriate information given below, calculate the enthalpy of formation (ΔH°_f), in kJ/mol, for 2-ethylbutanedioic acid.

Report your answer to two decimal places.

ΔH°_f (CO₂ (g)) = -393.51 kJ/mol

ΔH°_f (H₂O (l)) = -285.83 kJ/mol

2b  Determine the mass (in g) of 2-ethylbutanedioic acid produced, if ΔH° was determined to be -118.71 kJ during an experiment in which 2-ethylbutanedioic acid was formed.

Report your answer to three significant figures.