23g of of sodium reacted with 35.5g of chlorine. calculate the mass of the sodium chloride compound formed
1 answer:
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Answer:The molecular formula of the oxide of metal be . The balanced equation for the reaction is given by:
Explanation:
Let the molecular formula of the oxide of metal be
Mass of metal product = 1.68 g
Moles of metal X =
1 mol of metal oxide produces 2 moles of metal X.
Then 0.03005 moles of metal X will be produced by:
of metal oxide
Mass of 0.01502 mol of metal oxide = 2.40 g (given)
y = 2.999 ≈ 3
The molecular formula of the oxide of metal be . The balanced equation for the reaction is given by:
Answer:
The concentration of KOH is 0.186 M
Explanation:
First things first, we need too write out the balanced equation between HBr and KOH.
This is given as;
KOH (aq) + HBr (aq) → KBr (aq) + H2O (l)
From the reaction above, we can tell that it takes 1 mole of KOH to react with 1 mole of HBr.
We use the acid base formular in calculating unknown concentrations. This is given as;
where;
Ca = Concentration of acid
Va = Volume of acid
Cb = Concentration of base
Vb = Volume of base
na = Number of moles of acid
nb = Number of moles of base
KOH is the base and HBr is acid.
Hence;
Ca = 0.225
Va = 35
Cb = ?
Vb = 42.3
na = 1
nb = 1
Making Cb subject of formular we have;
Cb = (0.225 * 35 * 1) / (42.3 * 1)
Cb = 0.186 M