Chemical Reaction: CS2 + 2NH3 → H2S + NH4SCN
How many grams of hydrogen sulfide (H2S) are produced when 0.532 grams of carbon disulfide (CS2) are consumed?
Final answer: 0.532 grams of hydrogen sulfide (H2S) are produced when 0.532 grams of carbon disulfide (CS2) are consumed by using stoichiometry
Answer:
0.532 grams of hydrogen sulfide (H2S) are produced when 0.532 grams of carbon disulfide (CS2) are consumed in the chemical reaction described above. This is based on the stoichiometry calculation where the molar ratio between CS2 and H2S is 1:1. Therefore, the mass of H2S produced is equivalent to the mass of CS2 consumed.
In this balanced chemical equation: CS2 + 2NH3 → H2S + NH4SCN, the stoichiometry relationship allows us to determine the amount of products formed from the reactants utilized. In this case, when 0.532 grams of carbon disulfide (CS2) is consumed, an equal amount of hydrogen sulfide (H2S) will be produced.
Stoichiometry plays a crucial role in understanding the quantitative aspects of chemical reactions. By applying the principles of stoichiometry and utilizing balanced equations, we can accurately predict the quantities of reactants and products involved in a reaction.