Question

Calculate the mass of water formed when 2 gram of hydrogen combines with 18 gram of oxygen, if this problem is in agreement with law of constant proportion​

Answer 1

Explanation:

2G of oxygen and 12g of hydrogen is combined with each other. How many grams of water is formed?

This homework question can be solved with the following steps:

Write the chemical equation for the reaction (this is the first step for 80% of all chemistry problems).

Look up the molar mass of all the compounds in the reaction

For each of the amounts given in grams, calculate the amounts in moles using the appropriate molar mass.

Check which of the reacting compounds is in shortest supply. Once that compound has completely reacted, there is no reaction any more even though other compounds may still be available.

Calculate using the reaction proportions and the amount of reactant that is in short supply how much can be formed in moles

Using the molar mass of the product, calculate how many grams of product is formed.

To double check: Verify how much of each of the reactants is consumed, and how much is left. Then check that the total amount of grams of mass is unchanged by the reaction.

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Calculate the number of mols of oxygen first

n=mass/Molar mass

therefore oxygen mols=2g/16

oxygen mol=0.125 mol

then Hydrogen mols=12g/1

hydrogen mol=12mol

So the limiting reactant is oxygen

2H+1 O provides one H2O molecule.

So Oxygen reacts completely.

Therefore 0.125*2 mol of Hydrogen reacts with one Oxygen

Only one water molecule is formed. Therefore the mols of formed water molecules will be equal to oxygen mols since it is the limiting reagent

therefore water mols=0.125

Now calculate mass of water

m=mol*molar mass

0.125mol*18g per mol

2.25g of water formed

Hope it helps ☺☺