Question

1)The following chemical reaction takes place in aqueous solution:

CuCl2(aq)+2KOH(aq)→CuOH2(s)+2KCl(aq)

Write the net ionic equation for this reaction.

2)Calculate the volume in milliliters of a 2.4M silver nitrate solution that contains 150.g of silver nitrate AgNO3. Be sure your answer has the correct number of significant digits.

3)Write the empirical formula for at least four ionic compounds that could be formed from the following ions:MnO−4,SO−24,Fe+3, Pb+4

4)Green plants use light from the Sun to drive photosynthesis. Photosynthesis is a chemical reaction in which water

H2O and carbon dioxide CO2 chemically react to form the simple sugar glucose C6H12O6 and oxygen gas O2.What mass of water is consumed by the reaction of 8.64g of carbon dioxide?Be sure your answer has the correct number of significant digits.

Answer 1

CuCl2(aq)+2KOH(aq)--->Cu(OH)2(s)+2KCl(aq)

net ionic equation :

Cu2+(aq) + 2OH-(aq) --> Cu(OH)2 (s)
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concentration of AgNO3 = 2.4 M
we have molar mass of AgNO3 =169.87 g/mol
mass of AgNO3 used = 150 g
Hence moles of AgNO3 present = mass/molar mass
= 150 g/169.87 g/mol
= 0.883028 mols

volume of solution = MOles of solute/concentration
=0.883028 mols/2.4 M = 0.3679 L
volume in milli liters= 368 ml
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3)
Pb(SO4)2
Fe2(SO4)3
Fe(MnO4)3
Pb(MnO4)4
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6H2O +6CO2 --> C6H12O6 + 6O2
from balanced equation it is clear that 6 mols CO2 needs 6 mols H2O
mole ratio is 1:1
moles of CO2 reacted= mass of CO2 present/molar mass of CO2
=8.64 g/44.01 g/mol = 0.196319 mols
mols of H2O required = 0.196319 mols since mole ratio 1:1]

mass of H2O needed= 0.196319 mols* 18.015 g/mol = 3.54 g