Question

How many moles of oxygen gas are required to combust a `4*mol` quantity of acetylene completely?

Answer 1

`H-C-=C-H(g) + 5/2O_2(g) rarr 2CO_2(g) + H_2O(g)`

Explanation:

The balanced chemical equation is given. Each mole of acetylene requires two and a half moles of oxygen gas. So if 4 mol acetylene are combusted, some 10 moles of dioxygen are necessary.

Answer 2

`10` `mol` `O_2`

Explanation:

1. First thing to do is to balance the chemical equation; The balanced equation is:
   `2C_2H_2 + 5O_2 rarr 4CO_2 + 2H_2O`

2. Then use the coefficients, which represents the number of mol of its compound/molecules in said reaction, to get the number of mol of `O_2` molecules;

3. Multiply the mol of acetylene as provided in the problem (`4 mol C_2H_2`) with the convertion ratio of the moles of acetylene and oxygen molecules (`(5 mol O_2)/(2mol C_2H_2`)) based on the balanced equation;
4. Make sure to cancel the mole of `C_2H_2` and get your desired mole of `O_2` molecules.
5. The answer per computation is 10 mol of `O_2`moleules