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Problem: When hydrogen sulfide gas is bubbled into a solution of sodium hydroxide, the reaction forms sodium sulfide and water.How many grams of sodium sulfide are formed if 1.60 g of hydrogen sulfide is bubbled into a solution containing 2.13 g of sodium hydroxide, assuming that the sodium sulfide is made in 93.0 % yield?

🤓 Based on our data, we think this question is relevant for Professor Zellmer's class at OSU.

FREE Expert Solution

Reactants:

hydrogen sulfide → H2S
sodium hydroxide → NaOH


Products:

sodium sulfide  → Na2S
water  → H2O


Balanced reaction:   H2S + 2 NaOH → Na2S + 2 H2O


Calculate theoretical yield:

Na2S from H2S:

molar mass Na2S = 78.04 g/mol
molar mass H2S = 34.08 g/mol

mass Na2S=1.60 g H2S×1 mol H2S34.08 g H2S×1 mol Na2S1 mol H2S×78.04 g Na2S1 mol Na2S

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Problem Details

When hydrogen sulfide gas is bubbled into a solution of sodium hydroxide, the reaction forms sodium sulfide and water.

How many grams of sodium sulfide are formed if 1.60 g of hydrogen sulfide is bubbled into a solution containing 2.13 g of sodium hydroxide, assuming that the sodium sulfide is made in 93.0 % yield?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Percent Yield concept. If you need more Percent Yield practice, you can also practice Percent Yield practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Zellmer's class at OSU.