How many moles are in 3.0g of A1203?
1 answer:
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Answer:
0.050 mol
Explanation:
The reaction that takes place is:
- H₃PO₄ + 3NH₃ → (NH₄)₃PO₄
Then we convert 0.050 moles of phosphoric acid into moles of ammonium phosphate, using the stoichiometric coefficients of the reaction:
- 0.050 mol H₃PO₄ *
= 0.050 mol (NH₄)₃PO₄
Thus, the complete reaction of 0.050 moles of phosphoric acid would produce 0.050 moles of ammonium phosphate.
Explanation:
According to the law of conservation of mass, mass can neither be created nor destroyed but it can simply be transformed from one form to another.
For example,
Mass of Na = 23 g/mol
Mass of Cl = 35.5 g/mol
Sum of mass of reactants = mass of Na + mass of Cl
= 23 + 35.5 g/mol
= 58.5 g/mol
Mass of product formed is as follows.
Mass of NaCl = mass of Na + mass of Cl
= (23 g/mol + 35.5) g/mol
= 58.5 g/mol
As mass reacted is equal to the amount of mass formed. This shows that mass is conserved.
As a result, law of conservation of mass is obeyed.
Answer : The volume (in mL) of 95% ethanol added would be, 1.39
Explanation :
As we are given that:
Mass of 95 % ethanol = 1.2 g
Density of 95 % ethanol = 0.86 g/mL
Formula used :
Therefore, the volume (in mL) of 95% ethanol added would be, 1.39