Part 2 Calculate the amount in moles of H2O formed.
Answer in units of mol
1.3 and 1.3
The 1.3 moles of HCl is the limiting reagent. With the molar ratio at 1:1, NaCl and H2O are both 1.3 moles.
HCl + NaOH -> NaCl + H2O
Take note of how all the reactants and products are at a 1:1 ratio.
Hence the limiting reagant here would simply be HCl since there is less of it that NaOH.
We use the amount of NaOH to work out moles of NaCl. Since it is at a 1:1 ratio according to the equation
Therefore 1.3 mol of NaCl produced and also 1.3 mol of H2O formed.
Safely & Permanently Remove Moles, Warts and Skin Blemishes
1. Given:
HCl + NaOH → NaCl + H₂O
mol of HCl = 1.3 mol
mol of NaOH = 2.6 mol
Asked:
mol of NaCl formed
mol of H₂O formed
Answer:
Since HCl has the lower mol, HCl becomes the limiting reactant
= 1/1 x mol of HCl
= 1/1 x 1.3 mol
= 1.3 mol
Reaction: HCl + NaOH → NaCl + H₂O
Initial: 1.3 mol \ 2.6 mol
Reacted: 1.3 mol \ 1.3 mol \ 1.3 mol \ 1.3 mol
----------------------------------------------------------------------
End: ----------- mol \ 1.3 mol \1.3 mol \ 1.3 mol
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Answers & Comments
Verified answer
1.3 and 1.3
The 1.3 moles of HCl is the limiting reagent. With the molar ratio at 1:1, NaCl and H2O are both 1.3 moles.
HCl + NaOH -> NaCl + H2O
Take note of how all the reactants and products are at a 1:1 ratio.
Hence the limiting reagant here would simply be HCl since there is less of it that NaOH.
We use the amount of NaOH to work out moles of NaCl. Since it is at a 1:1 ratio according to the equation
Therefore 1.3 mol of NaCl produced and also 1.3 mol of H2O formed.
Safely & Permanently Remove Moles, Warts and Skin Blemishes
1. Given:
HCl + NaOH → NaCl + H₂O
mol of HCl = 1.3 mol
mol of NaOH = 2.6 mol
Asked:
mol of NaCl formed
mol of H₂O formed
Answer:
Since HCl has the lower mol, HCl becomes the limiting reactant
mol of NaCl formed
= 1/1 x mol of HCl
= 1/1 x 1.3 mol
= 1.3 mol
mol of H₂O formed
= 1/1 x mol of HCl
= 1/1 x 1.3 mol
= 1.3 mol
Reaction: HCl + NaOH → NaCl + H₂O
Initial: 1.3 mol \ 2.6 mol
Reacted: 1.3 mol \ 1.3 mol \ 1.3 mol \ 1.3 mol
----------------------------------------------------------------------
End: ----------- mol \ 1.3 mol \1.3 mol \ 1.3 mol