Starting with 9.3 moles of O2, how many moles of H2S will be needed and how many moles of SO2 will be produced in the following reaction? SHOW YOUR WORK!

The amount of hydrogen sulfide needed is 6.2 moles and amount of sulfur dioxide gas produced is 6.2 moles

Explanation:

We are given:

Moles of oxygen gas = 9.3 moles

The chemical equation for the reaction of oxygen gas and hydrogen sulfide follows:

For hydrogen sulfide:

By Stoichiometry of the reaction:

3 moles of oxygen gas reacts with 2 moles of hydrogen sulfide

So, 9.3 moles of oxygen gas will react with = of hydrogen sulfide

For sulfur dioxide:

By Stoichiometry of the reaction:

3 moles of oxygen gas produces 2 moles of sulfur dioxide

So, 9.3 moles of oxygen gas will produce = of sulfur dioxide

Hence, the amount of hydrogen sulfide needed is 6.2 moles and amount of sulfur dioxide gas produced is 6.2 moles

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !