Question

Boron hydrides were once evaluated for possible use as rocket fuels. Complete and balance the following equation:

${\text{B}}_2{\text{H}}_6+{\text{O}}_2\to \text{B}(\text{OH}{)}_3$

Short answer

The balanced equation: ${\text{B}}_2{\text{H}}_6\left(g\right)+3{\text{O}}_2\left(g\right)\to 2\text{B}(\text{OH}{)}_3\left(s\right)$.

Step-by-step solution

Definition of bond

A chemical bond is that holds atoms in a molecule together.

Balance the equation

• Boranes were formerly used as rocket fuel, but they were discovered to be too pyrophoric to handle properly.
• An imbalanced diborane-oxygen reaction is shown below.

${\text{B}}_2{\text{H}}_6\left(g\right)+{\text{O}}_2\left(g\right)\to \text{B}(\text{OH}{)}_3\left(s\right)$

• Subscripts and coefficients are the two sorts of numbers that appear in chemical equations.
• Subscripts are an integral element of the formulae and cannot be modified.
• The coefficients represent the number of each substance involved in the reaction, and they can be modified to make the equation balanced.
• As a result, the coefficients must be adjusted to achieve the equal amount of atoms of each element on both sides.
• At the imbalanced equation, it can be seen that there are two boron atoms on the left side and only one on the right.
• Hence, put the coefficient 2 in front of$\text{B}(\text{OH}{)}_3$ to balance the equation.
• Also, you can see that the total number of oxygen atoms on the right side is now $6$, therefore the coefficient in front of${\mathrm{O}}_2$ needs to be $3$.

${\text{B}}_2{\text{H}}_6\left(g\right)+3{\text{O}}_2\left(g\right)\to 2\text{B}(\text{OH}{)}_3\left(s\right)$