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A solution containing copper (I), nickel, and Zinc cyanide complexes was eloctrolyzed, and a deposit of 0.175 grams was obtained. the deposit contained 72.8% Cu, 4.30% Ni, and 22.9% ZN. no other element or compound was released.
Calculate the number of coulombs passed through the solution.
If 24 mL of 6.2 M H2SO4 was spilled, what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid?
Could Kb for a weak base be determined in the same way that Ka for a weak acid is determined in an experiment
15.0 ml sample of .1m baoh2 is titrated with .125 m hcl. calculate the ph for atleast five different throughout the
How much heat is liberated at constant pressure if 0.834 g of calcium carbonate reacts with 48.9 mL of 0.668 M hydrochloric acid? CaCO3(s) + 2HCl(aq) > CaCl2(aq) + H2O(l) + CO2(g); DeltaH = -15.2 kJ
Acetylene, C2H2, can be converted to ethane, C2H6, by a processknown as hydrogenation. The reaction is
what would be the volume of an ideal gas at absolute zero? what happens to real gases before they reach absolute zero?
The final temp of the water is 78.26 degrees F. Calculate the specific heat of the metal. Assume that all energy lost by metal is gained by the water.
A current is drawn from the cell until 2.20 g of silver have been deposited at the silver electrode. Calculate E for the cell at this stage of operation in volts.
If the initial volume of the container, before any reaction takes place, is 5.70 L, determine the volume of the container after the N2 (g) and H2 (g) have reacted to completion.
What is the rate constant of a first-order reaction that takes 215 for the reactant concentration to drop to half of its initial value?
A 5.0 L bulb filled with 175 torr of He and a 7.5 mL bulb filled with 325 torr of Kr are connected together allowing the gases to mix. What is the final pressure in the combined bulbs, assuming the gases behave ideally and the volume of the connec..
A chemist dissolves 128 mg of pure hydrobromic acid in enough water to make up of 110 mL solution. Calculate the pH of the solution.
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