Which of the following represents the total amount of energy

CHEMISTRY · Single correct · A Level · Chemistry · Periodicity and periodic trends · Periodicity and periodic trends

Problem

Which of the following represents the total amount of energy, in kJ, required to form one mole of oxide ions from one mole of oxygen atoms? (1st *EA* of oxygen = −141 kJ mol−1-141 \text{ kJ mol}^{-1} ; 2nd *EA* of oxygen = 753 kJ mol−1753 \text{ kJ mol}^{-1} ; NA=6.02×1023 mol−1N_A = 6.02 \times 10^{23} \text{ mol}^{-1} ) (1) −141-141 (2) −141×2×6.02×1023-141 \times 2 \times 6.02 \times 10^{23} (3) (−141+753)×6.02×1023(-141 + 753) \times 6.02 \times 10^{23} (4) −141+753-141 + 753

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