When $Fe_{0.93}O$ is heated in presence of oxygen, it converts to $Fe_2O_3$. Evaluate the correct st

Question

When $Fe_{0.93}O$ is heated in presence of oxygen, it converts to $Fe_2O_3$. Evaluate the correct statements:\ A) Eq wt of $Fe_{0.93}O$ is M/0.79.\ B) Moles of $Fe^{2+}$ and $Fe^{3+}$ in 1 mole are 0.79 and 0.14.\ C) It is metal deficient.\ D) % composition of $Fe^{2+}$ and $Fe^{3+}$ is 85% and 15%.\ How many are correct?

Professor PC Thomas Classes · Answer

Solving $2x + 3(0.93-x) = 2 \implies x = 0.79$ ($Fe^{2+}$) and $0.14$ ($Fe^{3+}$). % $Fe^{2+} = 0.79/0.93 = 85\%$. It is metal deficient ($0.93 < 1$). To oxidize to $Fe_2O_3$, only $Fe^{2+}$ oxidizes, losing 0.79 mol electrons, so n-factor = 0.79. All 4 statements are correct.