Question

The combustion of propane (C3H8) produces CO2 and H2O: C3H8 (g) 5O2 (g) → 3CO2 (g) 4H2O (g) The reaction of 2.5 mol of O2 will produce ________ mol of H2O.

Answer 1

To find the amount of water produced when 2.5 mol of O2 is consumed in the combustion of propane, we can use stoichiometry. The combustion of 2.5 mol of O2 will produce 2 mol of H2O.

Step-by-step explanation:

The balanced equation for the combustion of propane is:

C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g)

To find the amount of water produced when 2.5 mol of O2 is consumed, we need to use stoichiometry. Since the ratio of O2 to H2O is 5:4, we can set up the following proportion:

2.5 mol O2 / 5 mol O2 = x mol H2O / 4 mol H2O

Solving for x, we find that x = 2 mol H2O. Therefore, the combustion of 2.5 mol of O2 will produce 2 mol of H2O.

Answer 2

Answer: 2 moles of water.

Step-by-step explanation:

According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

The combustion of propane is represented as :

`C_3H_8(g)+5O_2(g)\rightarrow 3CO_2(g)+4H_2O(g)`

According to stoichiometry:

5 moles of
`O_2` produces = 4 moles of
`H_2O`

2.5 moles of
`O_2` will produce=
`(4)/(5)* 2.5=2` moles of
`H_2O`.

Thus 2 moles of water are produced by 2.5 moles of oxygen.