Mole Ratios: Silver Nitrate + Copper (Equation)
[F]
\
Silver Nitrate + Copper
AgNO3 + Cu ---> CuNO3 + Ag
The reaction starts with
weight of empty beaker - 111.420
200ml of Silver Nitrate with a weight of 316.262g(including beaker)
added 1g of Copper weight 317.262g(including beaker)
After given amount of time:
Decanted solution into empty beaker2 weight is now 313.868
In beaker 1 Silver remains weight is 114.815
a.) 1 gram of copper
b.) 114.815g silver and beaker
c.)empty beaker 111.420g
d.)3.395g of silver produced
(e) Moles of solid copper used in reaction (mol)
1g x 1mol/63.546 = .016 mol
(f) Moles of solid silver produced in reaction (mol)
3.395 x 1 mol/107.868 = .031 mol
I have gotten this far but this is the rest of my assignment and I am stuck when it comes to the mole ratios and fractional coefficients.
2. Write the equation for the reaction between copper and silver ion. Include your experimentally determined mole ratios as fractional coefficients.
3. Convert the fractional coefficients to a whole number ratio and rewrite the equation using the whole number ratio.
4. If the silver in the beaker contained water during your last weighing, how would this affect your results?
5. Assume that magnesium would act atom-for-atom exactly the same as copper in this experiment. How many grams of magnesium would, have been used in the reaction if one gram of silver were produced? The atomic mass of magnesium is 24.31 g/mol.
6. Explain the source of the blue color of the solution after the reaction.