CHM 131 Chapter Notes - Chapter 3.1-3.9: Limiting Reagent, Reagent, Americium

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lavendergiraffe572

8 Sep 2015

School

University of Rochester

Department

Chemistry

Course

CHM 131

Professor

Hafensteiner

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Document Summary

Mass 13c divided by mass 12c = 1. 0836129 which is the ratio of the masses. Atomic mass unit is defined such that the mass of 12c is exactly 12 atomic mass units: 98. 89% of 12 amu + 1. 11% of 13. 0034 amu = (0. 9889)(12 amu) + (0. 0111)(13. 0034 amu) = Calculate the mass in grams of a sample of americium containing six atoms: 6 atoms times 243 amu/atom = 1. 46*10^3 amu. 1. 46*10^3 amu times (1 gram)/(6. 022*10^23 amu) = 2. 42*10^(-21) grams. Mass of c = 2 moles times 12. 011 g/mol = 24. 022 grams. Mass of h = 6 moles times 1. 008 g/mol = 6. 048 grams. Mass of o = 1 mole times 15. 9999 g/mol = 15. 9999 grams. Mass of 1 mole of c2h5oh = 46. 069 grams. Mass percent of carbon in ethanol will be found by comparing the mass of carbon in 1 mole of ethanol with the total mass of 1 mole of ethanol and multiplying the result by 100%:

Related Questions

Having trouble with thse questions. Please answer all questions correctly. Will provide a thumbs up.

1.Which of these equations is the balanced reaction between nitrous acid solution and solidmagnesium hydroxide ?

A.2NH₃(aq) + MgOH (s) Mg(NH₄)₂(aq) + 2 H₂O(l)

B.2HNO₂(aq) + Mg(OH)₂(s) Mg(NO₂)₂(aq) + 2 H₂O(l)

C.2HNO₃(aq) + Mg(OH)₂(s) Mg(NO₃)₂(aq) + 2 H₂O(l)

D.2HNO₂(aq) + MgOH (s) Mg(NO₃)₂(s) + 2H₂O(l)

2.Balance the following chemical equation:

C₃H₇OH(l) + O₂(g)CO₂(g) + H₂O(g)

a. C₃H₇OH(l) + 4 O₂(g)3 CO₂(g) + 4 H₂O(g)

b.2 C₃H₇OH(l) + 9 O₂(g)6 CO₂(g) + 8 H₂O(g)

c.C₃H₇OH(l) + 5 O₂(g)3 CO₂(g) + 4 H₂O(g)

d.C₃H₇OH(l) + O₂(g)CO₂(g) + H₂O(g)

3.Which species would be considered a spectator ion based on the following equation?

Ba²⁺ + 2NO₃^â + 2Na⁺ + SO₄^2- â BaSO₄(s) + 2NO₃^â + 2Na⁺

SO₄^2-

2NO₃^â

Ba²⁺

BaSO₄

4.Barium sulfate is often ingested to aid in the diagnosis of GI tract disorders. The equation for its production is Ba²⁺ + SO₄^2- â BaSO₄(s). What type of equation is this?

A full equation

A net ionic equation

A total ionic equation

An oxidation-reduction equation

5.Which species is being reduced in this reaction?

CuO(s) + H₂(g) Cu(s) + H₂O(g)

H₂O

CuO

H₂

6.Which of the following is an oxidizing agent?

H₂

NH₃

O₂

H₂O

7.The following chemical equation,

HC₂H₃O₂(aq) + KOH(aq) KC₂H₃O₂(aq) + H₂O(l),

is an example of a(n) _______ reaction.

a.oxidation-reduction and acid-base

b.acid-base

c.precipitation

d.oxidation-reduction and precipitation

e.oxidation-reduction

8.What substance is oxidized in the following reaction?

4HCl + MnO₂ â Cl₂ + 2H₂O + MnCl₂

a.Mn in MnO₂

b.O in MnO₂

c.Cl in HCl

d.H in HCl

9.What is the reducing agent in the following reaction?

4HCl + MnO₂ â Cl₂ + 2H₂O + MnCl₂

Cl₂

MnCl₂

HCl

MnO₂

10.All redox reactions involve oxygen.

True

False

11.The term formula weight can be used with respect to which of the following?

A.ionic compounds

B.covalent compounds

C.both a and b

D.neither a nor b

12.What is the molecular weight of ibuprofen, C₁₃H₁₈O₂?

A.206.3 amu

B.377.7 amu

C.29.0 amu

D.289.4 amu

13.The mass of an atom of ¹²C is exactly 12 atomic mass units. Which of the following describes a mole of ¹²C atoms?

A.a sample which weighs exactly 12 atomic mass units

B.a sample which contains 6.02 Ã 10²³ atoms of ¹²C

C.both a and b

D.neither a nor b

14.The mass of an atom of ¹²C is exactly 12 atomic mass units. Which of the following describes a mole of ¹²C atoms?

A.a sample which contains 6.02 Ã 10²³ atoms of ¹²C

B.a sample which weighs exactly 12.011 grams

C.both a and b

D.neither a nor b

15.What is the molar mass of water, H₂O?

A.18.02 g

B.18.02 amu

C.17.01 g

D.17.01 amu

16.What is the molar mass of glucose, C₆H₁₂O₆?

A.180.2 amu

B.180.2 g

C.60.05 amu

D.60.05 g

17.In the reaction 2H₂O â 2H₂ + O₂, 2.0 mol water will produce how many grams of O₂?

18.In the reaction 2CH₄ + O₂ â 2CO + 4H₂, how many molecules of CO will be produced by the complete reaction of 1.60 grams of CH₄?

3.01 Ã 10²²

2.00

12.0 Ã 10²³

6.02 Ã 10²²

19.Suppose 2.43 g of magnesium is reacted with 3.20 g of oxygen: 2Mg + O₂ â 2MgO. How many grams of MgO will be produced?

1.27

4.03

5.63

8.06

20.Which of the following conversion factors would allow one to calculate the amount of PbI₂produced from a given amount of NaI in the following unbalanced reaction?

Pb(NO₃)₂ + Nal â Pbl₂ + NaNO₃

21.The unbalanced equation for the reduction of copper(I) sulfide with oxygen is given below. What mass of copper is produced from the reduction of 7.50 g Cu₂S?

Cu₂S(s) + O₂(g) Cu(s) + SO₂(g)

18.8 g

5.99 g

1.50 g

9.39 g

2.99 g

22.How many grams of aluminum oxide are produced by the complete reaction of 19.8 g aluminum with excess oxygen?

10.5 g aluminum oxide

37.4 g aluminum oxide

49.9 g aluminum oxide

74.8 g aluminum oxide

23.If 5 grams of CO and 5 grams of O₂ are combined according to the reaction, which is the limiting reagent?

2CO + O₂ â 2CO₂

O₂

CO and O₂

CO₂

24.In an industrial process, nitrogen is reacted with hydrogen to produce ammonia. The percent yield of this particular process is 26%. How much hydrogen is needed to produce 4.8 kg ammonia?

1.5 kg

7.0 kg

0.85 kg

3.3 kg

25.A percentage yield greater than 100% has been reported in a scientific paper you are assigned to read. What would be a reasonable explanation for this?

a. The product was measured more than once.

b. It must be a typographical error since yields can't exceed 100%.

c. A lack of training of the professor who published the study.

d. Small measurement errors could have caused this to occur.

26.In an industrial process, nitrogen is reacted with hydrogen to produce ammonia. The percent yield of this particular process is 24.8%. How much hydrogen is needed to produce 3.7 kg ammonia?

1.8 kg

1.2 kg

4.4 kg

12 kg

2.7 kg

27.The following reaction has a percent yield of 90.5%. How many grams of carbon dioxide are produced from 78.5 g calcium carbonate via this reaction?

2 HNO₃(aq) + CaCO₃(aq) Ca(NO₃)₂(aq) + H₂O(l) + CO₂(g)

34.5 g

21.6 g

38.1 g

31.2 g

28.When gas molecules dissolve in liquids to form a saturated system, the process is usually

exothermic.

endothermic.

independent of the nature of the liquid.

temperature independent.

29.The reaction below would be considered.

CaCO₃ + heat â CaO + CO₂

an exothermic combination.

an exothermic decomposition.

an endothermic combination.

an endothermic decomposition.

30.The combustion of one mole of propane, C₃H₈, releases 531 kcal. How much heat is released by the combustion of 1.20 moles of propane?

A.584 kcal

B.690 kcal

C.443 kcal

D.637 kcal

31.The combustion of one mole of propane, C₃H₈, releases 531 kcal. How much heat is released by the combustion of 4.40 g of propane?

A.531 kcal

B.5.31 Ã 10⁴ kcal

C.53.1 kcal

D.5.31 Ã 10³ kcal

32.Metabolism of one mole of glucose, C₆H₁₂O₆, releases 670 kcal. How much heat is released by the combustion of 0.300 moles of glucose?

A.201 kcal

B.2.41 Ã 10³ kcal

C.186 kcal

D.2.23 Ã 10³ kcal

33.Metabolism of one mole of glucose, C₆H₁₂O₆, releases 6.70 Ã 10² kcal. How much heat is released by the combustion of 50.0 g of glucose?

A.201 kcal

B.2.41 Ã 10³ kcal

C.186 kcal

D.2.23 Ã 10³ kcal

golddinosaur326

There are two stable isotopes of supposium (Su). Su-191=190.9609u(27.30%) Su-194=193.9633 u(72.70%) Compute the atomic mass ofsupposium.
a. 194.0 u b. 193.1 u c. 191.8 u d. 190.9 u e. 192.5 u

Which would not be found with a mass spectrometer.
a. the atomic mass of a single isotope of potassium
b. the number of stable isotopes of potassium c.the mass of aproton
d. the number of protons in potassium e. the relative abundance oftwo isotopes of potassium

How many protons, neutrons, and electrons are in 24 Mg2+?
12
a. 10 protons, 12 electrons, 24 neutrons b. 12 protons, 10electrons, 12 neutrons
c.12 protons, 12 electrons, 24 neutrons d. 24 protons, 10electrons, 12 neutrons
e. 12 protons, 12 electrons, 12 neutrons

1.The age of rocks is sometimes calculated from the measured excessof lead 206 atoms over the normal abundance. The uranium isotopeU-238 decays to lead-206.What is the percent abundance of lead-206if there aare 4.52 X 10^21 atoms of lead-206 in a 198 g sample ofore that is 2.58% lead? a. 27.7 b. 0.0202 c. 4.70 x 10^-3 d. 30.4e. 0.782

2. The average atomic mass of B is 10.80 u. Boron has only twostable froms 10
5 B(10.00 u) and 11
5 B (11.00 u). What is the natural percent abundance of B?
a. 1.0% b. 20% c. 75% d. 3.8% e. 80%

3. 57.7 g Ni contains how many atoms? a. 3.47x10^23 b.0.983 c. 1.24x 10^24
d. 6.13x10^23 e. 5.92x10^23

4. What mass of magnesium is necessary to make 10.5 g of magnesiumbromide if 1.04 g of magnesium makes 7.88 g of magnesiumbromide?
a. 7.89 g b. 1.39 g c. 79.9 g d. 3.66 g e. 1.58 g

5. How many atoms of lead are required to cover a 33.0 cm by 45.0cm area witha sheet of lead that is 0.140 mm thick? The density oflead is 11.35 g/cm3.
a. 1.42x10^26
b. 2.29x10^25
c. 6.86x10^22
d. 2.29x10^26
e. 6.86X10^23

6. The natural abundance of calcium in the earth's crust is 3.4% bymass. How many calcium atoms are present in a 1.50 g sample of theearth's crust?
a. 7.7x10^22 b. 7.7x10^20 c. 3.1x 10^22 d.6.6x10^23 e.5.1x10^20

9.Rubidium possesses two stable forms and has an average mass of85.5. 85Rb has a mass of 84.9 and a percent abundance of 72.2%.What is the mass of the other form of Rb?

a. 85.7 u
b. 88.3 u
c. 86.1 u
d. 89.4 u
e. 87.1 u

10. Which is the more abundant isotope, CI-35 or CI37?
a. CI-17
b. CI-37
c. The two isotopes are equal in balance
d. CI-35
e. A third unstable isotope is more abundant

11. An element has 5 stable isotopes. The mass and percentage ofeach are:
69.9243 20.52%
71.9217 27.43%
72.9234 7.76%
73.9219 36.54%
75.9214 7.76%
The element is which of the following
a. Se b. Ge c. Ga d. As e. Zn

12. Lead-206 has a relative abundance of 23.6%. What sized block oflead (in cubic centimeters) will contain 8.34x10^21 atoms oflead-206? The density of lead is 11.35 is g/cm3.
a. 0.253
b. 0.0107
c. 1.07
d. 12.1
e. 0.330

13. When decomposed chemically, 73.0 grams of a sample of HCIproduce 71.0 g of Cl2 and 2.0 g of H2, while 34.0 g of a sample ofH2s produce 32.0g of S and 2.0g of H2. This is an example of theLaw:
a. of Definate Proportions
b. E=mc^2
c. of multiple proportions
d. of Conservation of Mass
e. none of these

Calculate the percent yield of Ba(OH)_2.8H_2O. You are making spaghetti for dinner tonight. You intend to use a little less than 2 quarts of water (2 Kilogram) and put in a small handful (10 grams) of salt (NaCI). What is the morality of the solution? How much of a change will the above salt make in the billing point of the solution? (K= .5121*/m) At what temperature do you expect the above to boil? You need to make up an isotonic solution (same concentration) of salt (NaCI) for your job, you are told that en isotonic solution of salt is 0.154 M. If you need to make up 500 milliliters of the solution, how much slat do you need? The gram molecular mass of an unknown compound was determined by measuring the freezing point of an aqueous solution of the compound. The following data were obtained: (the freezing point constant for water is 1.853 C/m) mass of unknown 4.42 g freezing point of water 0.04 degree C mass of water 26.242 g freezing point of solution - 1.46 degree C calculate the gram molecular mass of the unknown. What mass of antifreeze (ethylene glycol, C_2H_5O_2) should be added to a radiator with a capacity of 4 liters of water (1 liter is about 1000 g) to provide protection down to -30 degree F (-34.4 degree C)? Express 0.46,0.0067/1.8531 to the correct number of sigficant figures Express (3.51 + 87.6) times 0.035/6.000 to the correct # of significant figures. Express 9.53/0.063. (43.2 times 0.024) to the correct # of significant figures. Na_3PO_4+AIF_3 Cs + H_2O FeF + CU(NO_3)_2 Hg+FeCI_3 H_2O + SO_2 K+MnBr_2 Based on their location on the periodic table, what is the empirical formulas that forms between AI and CI? Octane has a molecular formula of C_8H_18. What is the empirical formula of octane? Fructose has an empirical formula of C_8H_18. What is the empirical formula of octane? Fructose has an empirical formula of C_8H_18. What is the molecular formula of fructose if the molecular formula has 6 carbon atoms? What compounds from when solid magnesium metal is heated in the presence of air? Based on your observations in the Getting acquainted with Metals lab, would you predict that Ga would or would not react with water? Based on your observations in the Getting acquainted with Metals lab, would you predict that a piece of Au would or Would not react when placed in a solution of NiCl_2? Based on your observations in the Getting acquainted with Metals lab, would you predict that Au would or would not react with HCI? Ammonia gas & hydrogen chloride gas were allowed to diffuse from opposite ends of a glass tube. It took exactly 78.2 seconds for a white smoky ring to form in the tube. The distance of the ring form the HCI(g) Source = 27.9 cm while the NH_3(g) = 49.6 cm. What was the diffusion rate of the HCI gas? What was the diffusion rate of the NH3 gas? What is the ratio of the diffusion rates of HCI(g) to NH_3 (g)?

CHM 131 Chapter Notes - Chapter 3.1-3.9: Limiting Reagent, Reagent, Americium

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