Part B The number of moles of MgO produced when 0.20 mole of \( \mathrm{O}_{2} \) reacts completely is 0.10 mole. 0.80 mole. 0.40 mole. 0.20 mole. 0.60 mole. Submit Reguest Answer

When oxygen gas \( \mathrm{O}_{2} \) reacts with magnesium \( \mathrm{Mg} \), it produces magnesium oxide \( \mathrm{MgO} \) according to the balanced equation: \( 2\mathrm{Mg} + \mathrm{O}_{2} \rightarrow 2\mathrm{MgO} \). This equation shows that 1 mole of \( \mathrm{O}_{2} \) produces 2 moles of \( \mathrm{MgO} \). Therefore, if you start with 0.20 moles of \( \mathrm{O}_{2} \), you would produce 0.20 × 2 = 0.40 moles of \( \mathrm{MgO} \). Now, let’s talk moles! When you’re calculating moles in a reaction, always double-check your balanced equation. Each compound has its own stoichiometric coefficients and they play a crucial role in figuring out how much product you’re going to make. A simple slip could lead you to incorrect calculations—yikes! And don’t forget to unit-check after you perform your calculations to ensure accuracy.