Part A What mass of calcium can be produced by this process if a
current of 6300 A is applied for 39 h ? Assume that the
electrolytic cell is 65 % efficient. Part A What mass of calcium
can be produced by this process if a current of 6300 A is applied
for 39 h ? Assume that the electrolytic cell is 65 % efficient.
Part B What is the minimum voltage needed to cause the
electrolysis?
Part B...
Determine the mass (in g) of sodium hydrogen phosphate
(Na2HPO4) that must be added to 87.8 mL of
0.0264 M sodium dihydrogen phosphate to yield a pH of 7.78. Report
your answer to 3 significant figures.
Assume the volume of the solution does not change and that the 5%
approximation is valid.
5.0 g of calcium phosphate is mixed into 1 L of solution
a) what is the concentration of Ca^2+ and PO4^3-? calculate
b) explain how you could dissolve will calcium phosphate
c) what is the molarity of the solutions, if you were able to
dissolve all of it?
If 9.95 g of carbon dioxide is produced from the reaction of
6.90 g of methane and 20.1 g of oxygen gas, calculate the percent
yield of carbon dioxide.
Consider the reaction 3CaCl2(aq) +
2Na3PO4(aq) -->
Ca3(PO4)2(s) + 6 NaCl(aq) (molar
mass of calcium phosphate is 310.18 g/mol)
What mass of Ca3(PO4)2 is
produced from 275 mL of 0.150 M CaCl2? _____ g (