For the reaction: 2NO2(g) → N2O4(l),
the ΔH of the reactants, two moles of NO2 (g), is + 66 kJ/mol,
and the ΔH of the products, N2O4 (l), is -20 kJ/mol.
Which of the following shows the ΔH (change in enthalpy) for the reaction as a whole?
Question 8 options:
ΔrxnH =(- 20 kJ/mol) / (+66 kJ/mol)
ΔrxnH = (+66 kJ/mol) + (- 20 kJ/mol)
ΔrxnH =(+66 kJ/mol) - (- 20 kJ/mol)
ΔrxnH =(-20 kJ/mol) - (+ 66 kJ/mol)
Answers: 2
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For the reaction: 2NO2(g) → N2O4(l),
the ΔH of the reactants, two moles of NO2 (g), is + 66 kJ/mol,...
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