1. Consider a galvanic cell consisting of the following two redox couples:
Ag+(0.010M) + e- --> Ag(s) E0 = +0.80 V
Cr3+(0.010M) + e- --> Cr(s) E0 = -0.74 V
Write the equation for the half reaction occurring at the cathode
Write the equation for the half reaction occurring at the anode.
Write the equation for the cell
What is the standard cell potential E0cell for the cell?
Realizing the nonstandard concentrations, what is the actual cell potential, E0cell for the cell? What is the value of the Nernst equation
In: Chemistry
In: Chemistry
Determine the mass (in g) of
Ca3(PO4)2 that is produced when
140 mL of a 8.48×10-2 M Na3PO4
solution completely reacts with 778 mL of a 1.54×10-2 M
CaCl2 solution according to the following balanced
chemical equation.
2Na3PO4(aq) + 3CaCl2(aq) →
Ca3(PO4)2(s) + 6NaCl(aq)
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A gas expands from an initial volume of 4.88 L to a final volume of 6.33 L against an external pressure of 810. mmHg. During the expansion the gas absorbs 10. J of heat. What is the change in the internal energy of the gas?
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An organic liquid is a mixture of methyl alcohol (CH3OH) and
ethyl alcohol (C2H5OH). A 0.220-g sample of the liquid is burned in
an excess of O2(g) and yields 0.347 g CO2(g) (carbon
dioxide).
Set up two algebraic equations, one expressing the mass of carbon
dioxide produced in terms of each reagent and the other expressing
the mass of sample burned in terms of each reagent.
What is the mass of methyl alcohol (CH3OH) in the sample?
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List the allowed quantum numbers ml and ms for the following subshells and determine the maximum occupancy of the subshells. a) 2p b) 3d c) 4f d) 5g
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Write the balanced reaction equation for the precipitation of
calcium carbonate from
potassium carbonate and calcium chloride. Don't forget to show the
states of matter.
Using this balanced equation in the above question, determine
the limiting reactant if 25 grams of calcium chloride
reacted with 25 grams of potassium carbonate. Show your work.
In: Chemistry
The freezing point of water is 0.00°C at 1 atmosphere. If 13.93 grams of manganese(II) bromide, (214.7 g/mol), are dissolved in 280.9 grams of water ...
The molality of the solution is _______ m.
The freezing point of the solution is ______ °C.
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Enough of a monoprotic acid is dissolved in water to produce a 0.0103 M solution. The pH of the resulting solution is 2.53. Calculate the Ka for the acid.
I got 8.45x10^-4 but it says its wrong.
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A buffer solution contains 0.14 mol of ascorbic acid
(HC6H7O6) and 0.84 mol of sodium
ascorbate (NaC6H7O6) in 2.80
L.
The Ka of ascorbic acid
(HC6H7O6) is Ka =
8e-05.
(a) What is the pH of this buffer?
pH =
(b) What is the pH of the buffer after the addition of 0.07 mol of
NaOH? (assume no volume change)
pH =
(c) What is the pH of the original buffer after the addition of
0.21 mol of HI? (assume no volume change)
pH =
In: Chemistry
Calculate the pH of a mixture that contains 0.25 M of HCOOH and 0.14 M of HClO. The Ka of HCOOH is 1.8 × 10-4 and the Ka of HClO is 4.0 × 10-8.
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If 4.1 g of butanoic acid, C4H8O2, is dissolved in enough water to make 1.0 L of solution, what is the resulting pH?
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A chemist weighed out 1.654 g of a mixture containing unknown amounts of iron (Fe) and lead (Pb) and placed the sample in a 0.500 L flask containing O2 (g) at 24.0 C and 846 torr. After heating, the reaction to form Fe2O3(s) and PbO2(s) was completed, the vessel was cooled to 24.0 C and the pressure of O2 (g) remaining was 452 torr. Calculate the mass percentage of lead in the mixture. Molar masses (g/mol) : PbO2: 239.20; Fe2O3: 159.69; Pb: 207.20; Fe: 55.85
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When exposed to air, aluminum metal, Al, reacts with oxygen, O2, to produce a protective coating of aluminum oxide, Al2O3, which prevents the aluminum from rusting underneath. The balanced reaction is shown here: 4Al+3O2→2Al2O3
What is the theoretical yield of aluminum oxide if 2.20 mol of aluminum metal is exposed to 1.95 mol of oxygen?
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