How many moles of magnesium are needed to react with 0.50 mole of \( \mathrm{O}_{2} \) ? 2.0 moles 4.0 moles 3.0 moles 1.0 moles 0.50 mole
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Bonus Knowledge
In a typical reaction between magnesium (Mg) and oxygen (O₂), the balanced equation is: \[ 2 \, \text{Mg} + \text{O}_2 \rightarrow 2 \, \text{MgO} \] From the equation, you can see that 2 moles of magnesium react with 1 mole of oxygen. Therefore, if you have 0.50 moles of O₂, you would need just 1 mole of magnesium to react with it. So the answer is **1.0 moles** of magnesium! Now imagine you're planning a camping trip, and you want to bring your trusty magnesium fire starter. Knowing how much magnesium you need for your oxygen supply means you'll have enough to safely ignite those campfires without running short—practical knowledge for the great outdoors! If you want to dive deeper into chemistry, there are countless resources available, from textbooks that cover basic stoichiometry and chemical equations to interactive online courses that can provide labs and simulations. Playing around with reaction formulas can turn you into a chemist in your own kitchen!
