Question

Complete the below chemical reaction-
$\_\_{{C}_{2}}{{H}_{6}}+\_\_{{O}_{2}}\to \_\_C{{O}_{2}}+\_\_{{H}_{2}}O$

Answer 1

Hint: Hydrocarbons react with oxygen gas which is pressure in the atmosphere and liberates carbon dioxide and water as the products. The number of moles of the carbon dioxide and water produced are going to depend on the number of moles of the hydrocarbon that are going to react with the number of moles of the oxygen gas.

Complete answer:
- In the question we have to fill the blanks with proper numerical values to balance the chemical reaction.
- Hydrocarbons has a property to react with oxygen and forms carbon dioxide and water as the products with the liberation of the huge amount of the energy.
- The liberated energy can be used in different ways.
- The given chemical reaction is as follows.
\[\_\_{{C}_{2}}{{H}_{6}}+\_\_{{O}_{2}}\to \_\_C{{O}_{2}}+\_\_{{H}_{2}}O\]
- We have to fill the blanks with proper numerical values to get the balanced chemical reaction and it is as follows.
\[2{{C}_{2}}{{H}_{6}}+7{{O}_{2}}\to 4C{{O}_{2}}+6{{H}_{2}}O\]
- In the above chemical reaction 2 moles of the ethane is going to react with 7 moles of the oxygen and produces 4 moles of the carbon dioxide and 6 moles of the water as the product.
- Means we have to balance the number of carbon atoms, the number of oxygen atoms on the both sides of the chemical reaction then only it is called a balanced chemical reaction.

Note:
The reaction of 2 moles of the ethane with 7 moles of the oxygen gas is called complete combustion chemical reaction. The combustion of the ethane gas in the presence of the oxygen liberates huge amounts of energy also.