Question

1. H_{2} is produced by the reaction of 119.1 mL of a
0.9147 *M* solution of H_{3}PO_{4} according
to the following equation.

2 Cr + 2 H_{3}PO_{4} →
3 H_{2} + 2 CrPO_{4}

(a) Determine the number of moles of H_{2}.
------mol

(b) Determine the mass (in g) of H_{2}. -------g

2. Molecules of I_{2} are produced by the reaction of
0.4245 mol of CuCl_{2} according to the following
equation.

2 CuCl_{2} + 4 KI → 2 CuI
+ 4 KCl + I_{2}

(a) How many molecules of I_{2} are produced?

(b)What mass (in g) of I_{2} is produced? ------g

Answer #1

Calculate moles of H3PO4

Mol = volume in L x molarity

Volume is 0.1191 L and molarity is 0.9147 M

Mol = 0.1191*0.9147=0.1089 mol H3PO4

Determine mol ratio between H3PO4 and H2

2 mol H3PO4 : 3 mol H2

Moles of H2 formed = moles of H3PO4 x 3 mol H2 / 2 mol H3PO4

0.1089*3/2=0.1634 mol H2

Mass of H2

Mass = moles x molar mass

Molar mass of H2 is 2.0158 g/mol

0.1634*2.0158=0.3294 g

Mass of H2 produced is 0.3294 g

2).

a) determine mol ratio between CuCl2 : I2

Its 2 : 1

Calculate moles using moles of CuCl2

Mol I2 = 0.4245 mol CuCl2 x 1 mol I2 / 2 mol CuCl2

0.4245*1/2=0.2123 mol I2

b) mass of I2

Molar mass of I2 = 253.8 g/mol

Mass of I2 = 0.2123 x 253.8=53.88 g

So the mass of I2 produced would be 53.88 g

1)
Molecules of I2 are produced by the reaction of
0.3737 mol of CuCl2 according to the following
equation.
2 CuCl2 + 4 KI → 2 CuI + 4 KCl + I2
(a) How many molecules of I2 are produced?
(b)What mass (in g) of I2 is produced?
2)
What mass (in g) of silver oxide, Ag2O, is required
to produce 26.7 g of silver sulfadiazine,
AgC10H9N4SO2, from the
reaction of silver oxide and sulfadiazine?
2 C10H10N4SO2 +
Ag2O →...

What mass of KCl is required
to make 46 mL of a 0.10 M KCl
solution?
____________ g KCl
How many moles of
potassium ions are present in the solution?
____________ mol

A solution of 500.0 mL of 0.500 M strong acid HA was used as
part of an electrolytic cell.
The reduction half-reaction that took place was:
2 H+(aq) + 2e --> H2 (g)
The hydrogen gas collected in this reaction occupied a volume of
98.00 mL at 22.0 oC
and 738.5mm Hg.
1. How many moles of hydrogen gas were produced?
________ mol H2
2. How many moles of H+ ions were reduced?
________ mol H+
3. What was the...

4.58 M Ca(OH)2 150.0 mL and 8.24 M H3PO4 60.0 mL were used for
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Hydrogen iodide decomposes according to the following reaction.
2 HI(g) equilibrium reaction arrow H2(g) + I2(g) A sealed 1.5 L
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A chemist dissolved 65.353 grams of CuSO4 *
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Please do D, I already know the answer to C
(c) He then
reacted the above
CuSO4 solution with some 0.225 M KI
solution. The reaction occurs as
follows: 2
CuSO4 (aq) + 4 KI (aq) à 2 CuI (s) + I2 (aq)
+ 2 K2SO4 (aq)
How many mL of the KI solution will be needed to completely
precipitate out all the copper...

A sample 25.0 mL of an NaCl solution is diluted to a final
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solution?
How many moles of product, KHCO3 will be produced
when1.0 mol of K2O reacts with 1.0 mol H2O
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h) A...

1)Obtain a volume of 0.25 M Na2CrO4 to deposit all ions
contained in 0.2 M AgNO3 75 mL. Also, calculate the type of
sediment and the mass of the sediment. (However, Ag 107.9 g/mol and
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2)4.58 M Ca(OH)2 150.0 mL and 8.24 M H3PO4 60.0 mL were used for
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hydrogen gas, H2, reacts with nitrogen gas,N2, to form
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3H2+N2 --->2NH3
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Part 1 : A solution of sodium thiosulfate,
Na2S2O3, is 0.4899 M. 29.65 mL of
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2(Na2S2O3) +
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→ 2(H3AsO4) + 4HI

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