CoCl3(aq) + K2S(aq) yield Co2S3(s) + KCl(aq)
How many moles of KCl would be produced when 0.470 moles of Co2S3 are produced in the above unbalanced reaction?
How many moles of K2S would be required to react with 0.940 moles of CoCl3?
How many moles of K2S would be required to produce 0.320 moles Co2S3?
First balance the equation. Then follow this example of a stoichiometry problem I've posted. It shows step by step what to do.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To answer these questions, we first need to balance the chemical equation given:
CoCl3(aq) + K2S(aq) → Co2S3(s) + KCl(aq)
Once the equation is balanced, we can use the stoichiometry of the reaction to determine the number of moles of each substance.
1. To find the number of moles of KCl produced when 0.470 moles of Co2S3 are produced, we can use the balanced equation. The stoichiometric ratio of Co2S3 to KCl is 1:1, meaning that for every 1 mole of Co2S3 produced, 1 mole of KCl is also produced. Therefore, the number of moles of KCl produced would be 0.470 moles.
2. To determine the number of moles of K2S required to react with 0.940 moles of CoCl3, we again refer to the balanced equation. The stoichiometric ratio of CoCl3 to K2S is 1:1, meaning that for every 1 mole of CoCl3, 1 mole of K2S is required. Therefore, the number of moles of K2S required to react with 0.940 moles of CoCl3 would also be 0.940 moles.
3. Finally, to calculate the number of moles of K2S required to produce 0.320 moles of Co2S3, we use the balanced equation. The stoichiometric ratio of Co2S3 to K2S is 1:1, similar to the previous two calculations. Therefore, the number of moles of K2S required would be 0.320 moles.
In summary:
1. 0.470 moles of KCl would be produced.
2. 0.940 moles of K2S would be required.
3. 0.320 moles of K2S would be required.