how grams of oxygen can be produced from the decomposition of 100g KClO3?
how much iron can be recovered from 25.0g of Fe2O3
how can be produced from 125g Ag2S
Figure the precentage composition of the compound. For instance
percent of Fe in Fe2O3 = 2*atomicmassFe/(2atomicmassFe + 3atomicmass)
Then, you can multiply that decimal percent by the grams of Fe2O3 to get the yield.
To determine the grams of oxygen produced from the decomposition of 100g KClO3, you need to consider the balanced chemical equation for the reaction. The equation is:
2 KClO3(s) -> 2 KCl(s) + 3 O2(g)
From the equation, you can see that for every 2 moles of KClO3 decomposed, 3 moles of O2 are produced.
1. Find the molar mass of KClO3, which consists of potassium (K), chlorine (Cl), and oxygen (O).
Molar mass of KClO3 = (molar mass of K) + (molar mass of Cl) + 3 x (molar mass of O)
= atomic mass of K + atomic mass of Cl + 3 x atomic mass of O
2. Calculate the number of moles of KClO3 in 100g using the molar mass of KClO3 obtained in step 1.
Moles of KClO3 = Mass of KClO3 / Molar mass of KClO3
3. Use the stoichiometry of the balanced equation to convert moles of KClO3 to moles of O2.
Moles of O2 = (Moles of KClO3) x (3 moles of O2 / 2 moles of KClO3)
4. Convert moles of O2 to grams of O2 using the molar mass of O2.
Grams of O2 = (Moles of O2) x (Molar mass of O2)
Follow a similar approach to solve the other two questions by balancing the chemical equations and applying stoichiometry.
For the recovery of iron from Fe2O3:
1. Balance the equation for the reaction of Fe2O3 with a suitable reducing agent (such as carbon or hydrogen) to obtain elemental iron.
2. Determine the molar mass of Fe2O3, which consists of iron (Fe) and oxygen (O).
3. Calculate the number of moles of Fe2O3 in 25.0g using the molar mass obtained in step 2.
4. Use the stoichiometry of the balanced equation to convert moles of Fe2O3 to moles of iron.
5. Convert moles of iron to grams of iron using the molar mass of iron.
For the production of silver from Ag2S:
1. Balance the equation for the reaction of Ag2S with a suitable reducing agent (such as hydrogen or carbon) to obtain elemental silver.
2. Determine the molar mass of Ag2S, which consists of silver (Ag) and sulfur (S).
3. Calculate the number of moles of Ag2S in 125g using the molar mass obtained in step 2.
4. Use the stoichiometry of the balanced equation to convert moles of Ag2S to moles of silver.
5. Convert moles of silver to grams of silver using the molar mass of silver.