Use Mole Ratios Practice Test

Hydrogen peroxide decomposes according to $$\mathrm{2H_2O_2 \rightarrow 2H_2O + O_2}$$. If $7.0\ \text{mol}$ of $\mathrm{H_2O_2}$ decompose completely, how many moles of $\mathrm{O_2}$ form?

Consider the balanced equation: $$6CO_2 + 6H_2O \rightarrow C_6H_{12}O_6 + 6O_2$$ If a plant uses $12 \text{ mol}$ of $CO_2$ in photosynthesis, how many moles of $O_2$ are produced (assuming enough $H_2O$ is available)?