How many grams of silver sulfide are formed when 0.280 g of hydrogen sulfide reacts with excess silver and oxygen?

Explanation:

For this question we have to start with the reaction:

Now, we can balance the reaction, so:

With this in mind, we have to start with the amount of . The first step is to convert from grams to moles. For this, we need to find the molar mass of . If we check the periodic table we will find the atomic masses for Ag and H; H: 1 g/mol and A: 32 g/mol, so:

(1*2)+ (32*1) = 34 g/mol.

Now we can calculate the moles of :

With the moles of we can calculate the moles of if we check the molar ratio in the balanced equation, , so:

With the molar mass of we can convert from moles to grams (Ag: 107.86 g/mol, S: 32 g/mol), so:

(107.86*1)+(32*2)=247.80 g/mol

I hope it helps!

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