Gaseous methane (ch4) reacts with gaseous oxygen gas (o2) to produce gaseous carbon dioxide (co2) and gaseous water (h2o) . if 0.122g of water is produced from the reaction of 0.16g of methane and 0.25g of oxygen gas, calculate the percent yield of water.

The percent yield of water is 84.72 %

Explanation:

To calculate the number of moles, we use the equation:

     .....(1)

For methane:

Given mass of methane= 0.16 g

Molar mass of methane = 16 g/mol

Putting values in equation 1, we get:

For oxygen gas:

Given mass of oxygen gas = 0.25 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

The chemical equation for the reaction is

By Stoichiometry of the reaction:

2 moles of oxygen gas reacts with 1 mole of methane

So, 0.008 moles of oxygen gas will react with = of methane

As, given amount of methane is more than the required amount. So, it is considered as an excess reagent.

Thus, oxygen gas is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of oxygen gas produces = 2 moles of water

So, 0.008 moles of oxygen gas will produce = of water

Mass of water=

To calculate the percentage yield of titanium (IV) chloride, we use the equation:

Experimental yield of water = 0.122

Theoretical yield of water = 0.144 g

Putting values in above equation, we get:

Hence, the percent yield of water is 84.72%.

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