Describe what you expect to happen when the following
solutions are electrlized: aqueous Cu(NO3)2. That is,...
Describe what you expect to happen when the following
solutions are electrlized: aqueous Cu(NO3)2. That is, what are the
electrode reactions? what is the overall reaction? Nitrate ion is
not reduced.
A concentration cell containing aqueous solutions of Cu(NO3)2
and solid copper metal is constructed so that the Cu2+ ion
concentration in the cathode half-cell is 0.66 M. What is the
concentration of the Cu2+ ion in the anode half-cell if the cell
potential for the concentration cell at 25 oC is 0.034 V?
When Aqueous solutions of CaCl2 and AgNO3 (aq),are mixed ,a
reaction takes place producing acqueous Ca(NO3)2 and Solid AgCl
a)How many moles of each are used in the above chemical
equation?
b)Write ionic equations for MgCl2(aq) and AgNO3 (aq)
c)Identify spectator ions for part b
d)Name all compounds in the given complete and balanced
reaction
1. What is the oxidation number for each of the elements in
Cu(NO3)2?
2. What is the oxidation number for each element in MgCr2O7?
3. The oxidation number of
a. any substance is the charge of the substance
b. an uncombined element is zero
c. hydrogen is +2 when combined with nonmetals
d. none of the above is correct
4. The oxidation numbers of ______ are equal to their ionic
charges.
5. The term oxidation can be used to describe...
1.0 mol of Cu(NO3)2 is dissolved in 1000 g of water. What is the
molality of the solution for use in colligative property equations?
The answers are 1, 2, 3, 4, or cannot be determined.
If 3.35 g Cu(NO3)2 are obtained from allowing 1.46g of Cu to
react with excess HNO3--
How many grams of copper nitrate are formed from 1.46 g
copper?
What is the percent yield of copper nitrate for this
reaction?
1. Describe how you would prepare each of the following aqueous
solutions.
a. 1.30 L of 0.130 M (NH4)2SO4
solution, starting with solid (NH4)2SO4. Enter your
answers numerically separated by a comma.
b. 120 g of a solution that is 0.55 m
in Na2CO3, starting with the solid solute, Enter your answers
numerically separated by a comma.
c. 1.30 L of a solution that is 15.0 %
of Pb(NO3)2 by mass (the density of the solution is...
Insoluble PbBr2(s) precipitates when solutions of Pb(NO3)2(aq)
and NaBr(aq) are mixed.
Pb(NO3)2(aq) + 2 NaBr(aq) → PbBr2(s) + 2 NaNO3(aq) ΔrH° = ?
To measure the enthalpy change, 200. mL of 0.75 M Pb(NO3)2(aq)
and 200. mL of 1.5 M NaBr(aq) are mixed in a coffee-cup
calorimeter. The temperature of the mixture rises by 2.44 °C.
Calculate the enthalpy change for the precipitation of PbBr2(s), in
kJ/mol. (Assume the density of the solution is 1.0 g/mL, and its
specific heat...