$sub{e}^{}$ Consider the following balanced chemical equation. $5O_2+C_3{H}_8$longrightarrow$3C{O}_2+4H_{2}O$ How is the rate of appearance of $H_{2}O,\frac{[H_{2}O]}{t},$ related to the rate of disappearance of $O_2?-\frac{4}{5}(\frac{[O_2]}{t})-\frac{5}{4}(\frac{[O_2]}{t})-\frac{1}{5}(\frac{[O_2]}{t})-\frac{5}{4}(\frac{[O_2]}{t})\frac{1}{5}(\frac{[O_2]}{t})\frac{4}{5}(\frac{[O_2]}{t})$