Answer:
0.975 mole of O₂
Explanation:
We'll begin by calculating the number of mole in 80 g of KClO₃. This can be obtained as follow:
Molar mass of KClO₃ = 122.45 g/mol.
Mass of KClO₃ = 80 g
Mole of KClO₃ =?
Mole = mass /Molar mass
Mole of KClO₃ = 80 / 122.45
Mole of KClO₃ = 0.65 mole
Next, we shall write the balanced equation for the reaction. This is illustrated below:
2KClO₃ —> 2KCl + 3O₂
From the balanced equation above,
2 moles of KClO₃ decomposed to produce 3 moles of O₂.
Finally, we shall determine the number of mole O₂ produced by the decomposition of 80 g (i.e 0.65 mole) of KClO₃. This can be obtained as follow:
From the balanced equation above,
2 moles of KClO₃ decomposed to produce 3 moles of O₂.
Therefore, 0.65 mole of KClO₃ will decompose to produce = (0.65 × 3)/2 = 0.975 mole of O₂.
Thus, 0.975 mole of O₂ was obtained from the reaction.
Answer:
25.9g
Explanation:
Molecular mass of Fe₂O₃ = (56 * 2) + (16 * 3)
= 112 + 48 = 160
Let's follow the unitary method now
In 160g Fe₂O₃ , there is 112 g Fe
In 1 g Fe₂O₃ , there is 112 / 160 g Fe
In 37 Fe₂O₃ , we need 112 * 37 / 160
= 25.9 g Fe
It’s either not testable since hypothesis need to be able to be tested or it could be not likely tho second option it has been poorly written
Answer:
Metals have one or two electrons in their outermost shell
C. 1-2
Explanation:
- Metals have low ionisation energy because they easily looses the outermost electrons
- They have only one- two electrons in the outer most shell.
- They loose these electron to form charged species called cation.