1. Consider the equation 2KOH + H2SO4 → K2SO4 + 2H2O a) If 25g H2SO4 is reacted with 7.7g KOH, how many grams of K2SO4 are produced? b) For part (a) of this problem, identify the limiting reactant and calculate the mass of excess reactant that remains after the reaction is completed. c) Calculate the theoretical yield of the reaction. How many grams of material would you expect to obtain if the reaction has a 47.2% yield?

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Chapter1: Chemical Foundations
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TE l 48% 7:38 PM
NFC
INSTITUT UNIVERSITAIRE
SIANTOU
UNIVERSITY INSTITUTE
General chemistry problem set
L'Ecole des Majors
Answer all the questions
Тopic: Mole сoncept
1. Consider the equation
2KOH + H2SO4 → K2SO4 + 2H2O
a) If 25g H2SO4 is reacted with 7.7g KOH, how many grams of K2SO4 are produced?
b) For part (a) of this problem, identify the limiting reactant and calculate the mass of excess reactant that
remains after the reaction is completed.
c) Calculate the theoretical yield of the reaction. How many grams of material would you expect to obtain if the
reaction has a 47.2% yield?
2. Phenol, commonly known as carbolic acid, was used by Joseph Lister as an antiseptic for surgery in 1865. Its
principal use today is in the manufacture of phenolic resins and plastics. Combustion of 5.23 mg of phenol yields
14.67 mg CO2 and 3.01 mg H2O. Phenol contains only C, H, and O. What is the per-centage of each element in
this substance?
3. Adipic acid is used in the manufacture of nylon. The composition of the acid is 49.3% C, 6.9% H, and 43.8%
O (by mass), and the molecular mass is 146 amu. What is the mole-cular formula?
Topic: Chemical kinetics
4. Hydrogen sulfide is oxidized by chlorine in aqueous solution.
H2S(aq) Cl2(aq)→ S(s) 2HC1(aq)
The experimental rate law is
Rate = k[H2S][Cl2]
What is the reaction order with respect to H2S? with respect to
Cl2? What is the overall order?
5. The following data were collected for the reaction A(g) + B(g)→ Products.
Еxperiment
[A]o (M)
[B], (M)
Rate (M/s)
1
0.0100
0.100
1.0 x 10–03
0.0300
3.0 × 10–03
0.100
0.0300
0.300
2.7 × 10–02
a) Determine the rate law for this reaction.
b) Calculate the rate constant.
c) Calculate the rate when [A] 0.200 M and [B] 0.200 M.
6. A reaction of the form aA → Products is second order with a half-life of 425 s. What is the rate constant of the
reaction if the initial concentration of A is 5.99 x 10³ mol/L?
7. The following values of the rate constant were obtained for the decomposition of nitrogen dioxide at various
temperatures. Plot the logarithm of k versus 1/T and from the graph obtain the energy of activation.
Тетрerature ( C)
k (L/mol s)
320
0.527
Transcribed Image Text:TE l 48% 7:38 PM NFC INSTITUT UNIVERSITAIRE SIANTOU UNIVERSITY INSTITUTE General chemistry problem set L'Ecole des Majors Answer all the questions Тopic: Mole сoncept 1. Consider the equation 2KOH + H2SO4 → K2SO4 + 2H2O a) If 25g H2SO4 is reacted with 7.7g KOH, how many grams of K2SO4 are produced? b) For part (a) of this problem, identify the limiting reactant and calculate the mass of excess reactant that remains after the reaction is completed. c) Calculate the theoretical yield of the reaction. How many grams of material would you expect to obtain if the reaction has a 47.2% yield? 2. Phenol, commonly known as carbolic acid, was used by Joseph Lister as an antiseptic for surgery in 1865. Its principal use today is in the manufacture of phenolic resins and plastics. Combustion of 5.23 mg of phenol yields 14.67 mg CO2 and 3.01 mg H2O. Phenol contains only C, H, and O. What is the per-centage of each element in this substance? 3. Adipic acid is used in the manufacture of nylon. The composition of the acid is 49.3% C, 6.9% H, and 43.8% O (by mass), and the molecular mass is 146 amu. What is the mole-cular formula? Topic: Chemical kinetics 4. Hydrogen sulfide is oxidized by chlorine in aqueous solution. H2S(aq) Cl2(aq)→ S(s) 2HC1(aq) The experimental rate law is Rate = k[H2S][Cl2] What is the reaction order with respect to H2S? with respect to Cl2? What is the overall order? 5. The following data were collected for the reaction A(g) + B(g)→ Products. Еxperiment [A]o (M) [B], (M) Rate (M/s) 1 0.0100 0.100 1.0 x 10–03 0.0300 3.0 × 10–03 0.100 0.0300 0.300 2.7 × 10–02 a) Determine the rate law for this reaction. b) Calculate the rate constant. c) Calculate the rate when [A] 0.200 M and [B] 0.200 M. 6. A reaction of the form aA → Products is second order with a half-life of 425 s. What is the rate constant of the reaction if the initial concentration of A is 5.99 x 10³ mol/L? 7. The following values of the rate constant were obtained for the decomposition of nitrogen dioxide at various temperatures. Plot the logarithm of k versus 1/T and from the graph obtain the energy of activation. Тетрerature ( C) k (L/mol s) 320 0.527
LTE 47% 7:36 PM
NFC
Еxperiment
[A]o (M)
[B], (M)
Rate (M/s)
1
0.0100
0.100
1.0 x 10–03
0.0300
3.0 × 10–03
0.100
0.0300
0.300
2.7 × 10–02
a) Determine the rate law for this reaction.
b) Calculate the rate constant.
c) Calculate the rate when [A] 0.200 M and [B] 0.200 M.
6. A reaction of the form aA → Products is second order with a half-life of 425 s. What is the rate constant of the
reaction if the initial concentration of A is 5.99 x 10³ mol/L?
7. The following values of the rate constant were obtained for the decomposition of nitrogen dioxide at various
temperatures. Plot the logarithm of k versus 1/T and from the graph obtain the energy of activation.
Тетрerature ( С)
k (L/mol s)
320
0.527
330
0.776
340
1.121
350
1.607
Topic: Nuclear chemistry
8. Complete the following nuclear reactions.
a. 14Si
b. STi + ?
isP + ?
2Sc
» 36BA + ? + 4on
15
44,
22
44.
>
142
c. Cf
252,
98
9. Consider Rn-222
a. Predict the type of radioactive decay that Rn-222 is most likely to undergo.
b. Write the equation for the decay process.
c. The half-life of Rn-222 is 3.82 days. If you start with a 150.0-g sample of Rn-222, how much remains after
15.0 days?
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Transcribed Image Text:LTE 47% 7:36 PM NFC Еxperiment [A]o (M) [B], (M) Rate (M/s) 1 0.0100 0.100 1.0 x 10–03 0.0300 3.0 × 10–03 0.100 0.0300 0.300 2.7 × 10–02 a) Determine the rate law for this reaction. b) Calculate the rate constant. c) Calculate the rate when [A] 0.200 M and [B] 0.200 M. 6. A reaction of the form aA → Products is second order with a half-life of 425 s. What is the rate constant of the reaction if the initial concentration of A is 5.99 x 10³ mol/L? 7. The following values of the rate constant were obtained for the decomposition of nitrogen dioxide at various temperatures. Plot the logarithm of k versus 1/T and from the graph obtain the energy of activation. Тетрerature ( С) k (L/mol s) 320 0.527 330 0.776 340 1.121 350 1.607 Topic: Nuclear chemistry 8. Complete the following nuclear reactions. a. 14Si b. STi + ? isP + ? 2Sc » 36BA + ? + 4on 15 44, 22 44. > 142 c. Cf 252, 98 9. Consider Rn-222 a. Predict the type of radioactive decay that Rn-222 is most likely to undergo. b. Write the equation for the decay process. c. The half-life of Rn-222 is 3.82 days. If you start with a 150.0-g sample of Rn-222, how much remains after 15.0 days? End I Recommended Share Extract Pages Picture Sharing PDF Annotation L--
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