5 essay 2 points consider the following chemical reaction: 2b₅h₉(ℓ) + 12o₂(g) → 5b₂o₃(s) + 9h₂o(ℓ) how many…

Explanation:

Step1: Calculate molar mass of $B_2O_3$

The molar mass of $B$ is approximately $10.81\ g/mol$ and of $O$ is $16\ g/mol$. For $B_2O_3$, $M_{B_2O_3}=2\times10.81 + 3\times16=69.62\ g/mol$.

Step2: Calculate moles of $B_2O_3$

Use the formula $n=\frac{m}{M}$, where $m = 50.0\ g$ and $M = 69.62\ g/mol$. So, $n_{B_2O_3}=\frac{50.0}{69.62}\approx0.718\ mol$.

Step3: Determine mole - ratio from the balanced equation

From the equation $2B_5H_9(\ell)+12O_2(g)\to5B_2O_3(s)+9H_2O(\ell)$, the mole - ratio of $B_5H_9$ to $B_2O_3$ is $\frac{n_{B_5H_9}}{n_{B_2O_3}}=\frac{2}{5}$.

Step4: Calculate moles of $B_5H_9$

$n_{B_5H_9}=\frac{2}{5}\times n_{B_2O_3}=\frac{2}{5}\times0.718 = 0.2872\ mol$.

Step5: Calculate molar mass of $B_5H_9$

The molar mass of $B_5H_9$ is $M_{B_5H_9}=5\times10.81+9\times1.01 = 54.05+9.09=63.14\ g/mol$.

Step6: Calculate mass of $B_5H_9$

Use the formula $m = n\times M$. So, $m_{B_5H_9}=0.2872\ mol\times63.14\ g/mol\approx18.1\ g$.

Answer:

$18.1\ g$