Calculate the Z (oxidation number) and densities of the following two compounds: 1) K2O (regular tpe) and 2) K2O with K filling all retrahedral sites of hcp O (assuming idea c/a ration)
Please see the attachment.
Reduction through constant current electrolysis a) How much Cr3+ was reduced to Cr2+? b) A few seconds after the electrolysis was stopped, the potential of the cell came to rest at -0.524 volts. How much Cr3+ actually remains in the solution? c) What was the original Cr3+ concentration?
In the following reaction, identify the oxidizing and reducing agents. Cd + NiO2 + 2H2O to Cd(OH)2 + Ni(OH)2 a) Cd+2 is the reducing agent, NiO2 is the oxidizing agent. b) Cd is the reducing agent, H2O is the oxidizing agent. c) Cd is the reducing agent, NiO2 is the oxidizing agent. d) Cd is the reducing agent,
6. In the following reaction, identify the oxidizing and reducing agents. 3Ca + VO3 --> 3CaO + V a. Ca+2 is the reducing agent, VO3 is the oxidizing agent b. Ca is the oxidizing agent, VO3 is the reducing agent c. Ca is the reducing agent, V is the oxidizing agent d. Ca is the reducing agent, O-2 is
How many coulombs of charge are required to oxidize 1.0g of copper to copper(II) ions?
What is the oxidation half reaction for: 2H2O-->O2(g)+2H2(g)
A first order reaction has a half-life of 1.34 x 10^-3 hours. If the initial concentration of the reactant is 8.00M, what is its concentration after 4 half-lives? a. 4.00M b. 2.00M c. 1.00M d. 0.50M e. 0.25M
Working with half lives to determine the time required to reach a certain percentage of its initial concentration.
A first order reaction has a half-life of 157 seconds. How much time is required for the reactant to be reduced to 12.5% of its initial concentration?
It is given that the electrochemical cell is at 298K. At time zero [Zn 2+ ]= 1.0 x 10 ^-3 M and [Ag +] = 0.500 M. Calculate the molarities of zinc and silver ions after a current of 2.00 amperes flow for 20 hours. Please show step by step and the units you are using.