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Chem 1A
Quiz 1A
1. (4) Write the name for each of the following elements:
(a) Fe (b) P (c) Pb (d) Sn
2. (4) Write the symbol for each of the following elements:
(a) sodium (b) arsenic (c) mercury (d) nitrogen
3. (2) Write the following in correct exponential notation.
(a) 0.00482 x 10 –1277 (b) 48200 x 10 1525
4. (2) Round to 4 significant figures.
499950
5. (5) Give the answer to the following with the correct number of significant figures.
(a) (6.0030 x 10 –1452 ) (1.750 x 10 326 ) =
(125.817 - 120.41)
(b) (4.0 x 10 –25 ) 5 =
6. (5) Write the formula for the ion which has a +2 charge and has 20.0% more protons than electrons.
7. (3) The following data were obtained in the boric acid experiment:
Mass test tube + A 25.6358
mass test tube + A 25.6389
What is the difference (in milligrams) between these two masses?
Chem 1A Quiz 2A
At. Wt: C = 12.0, H = 1.0, O = 16.0, N = 14.0, Na = 23.0, P = 31.0, S = 32.1, Cl = 35.5, K = 39.1, Ba = 137.3
Numbers: 0.0821, 1.987, 4.184, 8.314, 14.7, 62.36, 273, 760, 8314, 101325
1. (4) Name by the IUPAC system:
(a) MnO (b) As(NO3)3
(c) H2SO4 (d) Al2(Cr2O7)3
2. (4) Name classically
(a) Ba(ClO2)2 (b) P2O5
(c) Sn(C2O4)2 (d) H2S (aq)
3. (6) Write the formulas
(a) magnesium sulfate (b) perchloric acid
(c) iron (II) phosphate (d) cobaltic oxalate
(e) mercurous bromide (f) tin(IV) carbonate
Chem 1A Quiz 3A
At. Wt: C = 12.0, H = 1.0, O = 16.0, N = 14.0, Na = 23.0, P = 31.0, S = 32.1, Cl = 35.5, K = 39.1, Ba = 137.3
Numbers: 0.0821, 1.987, 4.184, 8.314, 14.7, 62.36, 273, 760, 8314, 101325
1. (5) Indicate the solubility in water of the following compounds with an S for soluble or an I for insoluble.
(a) Sr(OH)2 ____, (b) BaSO4 ____, (c) MnS ____, (d) Pb(CO3)2 ___, (e) AgCl ____
2. (2) Write the net ionic equation for the reaction, if a reaction occurs, when the following reagents are combined. If there is no reaction, write N.R.
(a) LiOH + HC2H3O2 =
3. (12) 25.0 mL of an 12.0 M solution of H2SO4 were reacted with 40.0 mL of 9.00M KOH. If 25.6 grams of K2SO4 are produced, what is the % yield in the reaction?
4. (6) Complete and balance: Name the type of reaction.
(a) Ca + HBrO4 =
(b) H2SO4 + Al(OH)3 =
Chem 1A Quiz 4A
At. Wt: C = 12.0, H = 1.0, O = 16.0, N = 14.0, Na = 23.0, P = 31.0, S = 32.1, Cl = 35.5, K = 39.1, Ba = 137.3
Numbers: 0.0821, 1.987, 4.184, 8.314, 14.7, 62.36, 273, 760, 8314, 101325
1. (3) Write the equation for the combustion of C5H11CONH2 in oxygen. The nitrogen is converted to N2O5.
2.
(3) Write the balanced equation for the synthesis
of the binary compound produced, when oxygen is reacted with
arsenic. The product will have arsenic in its higher oxidation state.
3. (5) How many moles of bromine atoms in 0.725 g of BiBr3 ?
4. (7) Chlorine (atomic weight = 35.4527) has two stable isotopes, 35 Cl (34.96885 u) and 37 Cl (36.96590 u). What is the % abundance of 37 Cl?
5. (7) How many grams of CO2 can be prepared, when 2.75 g of C3H8 are reacted with excess oxygen?
Chem 1A Quiz 5A
At. Wt: C = 12.0, H = 1.0, O = 16.0, N = 14.0, Na = 23.0, Al = 27.0, P = 31.0, S = 32.1, Cl = 35.5, K = 39.1, Ba = 137.3
1. (5) Indicate the solubility in water of the following compounds with an S for soluble or an I for insoluble.
(a) MgS ____, (b) AgCl ____, (c) Mn(OH)2 ____, (d) Pb(CO3)2 ___, (e) BaSO4____
2. (4) Complete and balance:
(a) Ca + HClO4 =
(b) H2SO4 + Bi(OH)3 =
3. (5) Write the net ionic equation for the reaction, when the following reagents are combined. If no reaction write N.R.
(a) KOH + HBr =
(b) Na2CO3 + HNO3 =
4. (12) 2.6500 g of a mixture of BiCl3 and Sn3N4 were reacted with excess H2S to produce 2.500 g of Bi2S3 and SnS2. The other products were NH3 and HCl. What was the % of BiCl3 in the original mixture
Chem 1A Fall 2000 Quiz 6A
At. Wt: C = 12.0, H = 1.0, O = 16.0, N = 14.0, Na = 23.0, P = 31.0, S = 32.1, Cl = 35.5, K = 39.1, Ba = 137.3
Numbers: 0.0821, 1.987, 4.184, 8.314, 14.7, 62.36, 273, 760, 8314, 101325
1. (5) Write the net ionic equation for the reaction, when the following reagents are combined. If no reaction write N.R.
(a) KOH + HBr =
(b) Na2CO3 + HNO3 =
2. (10) Balance the following equation in acidic solution.. oxidant ________________
reductant ______________
Sb + ClO3 – = H3SbO3 + ClO –
3. (10) Balance the following in basic solution. oxidant _______________
reductant_______________
NO2 – + Sn = NH3 + Sn(OH)6 2–
Chem 1A Quiz 7A
At. Wt: C = 12.0, H = 1.0, O = 16.0, N = 14.0, Na = 23.0, P = 31.0, S = 32.1, Cl = 35.5, K = 39.1, Bi = 209.0
Numbers: 0.0821, 1.987, 4.184, 8.314, 14.7, 62.36, 273, 760, 8314, 101325
1. (5) 35.0 mL of 0.270 M Na2S are added to 45.0 mL of 0.150 M Bi(NO3)3. Assuming volumes are additive, what is the concentration of the NO3– ion in the final solution?
2. (6) The density of an unknown gas is 0.00295 g/mL at 75 °C and 0.885 atm. What is the molecular mass of the unknown gas ?
3. (5) What is the pressure (in torr) in a 35.0 mL container, if the container is filled with 45.8 g of nitrogen at 39.0 °C?
4. (5) What is the volume at STP of 762 mL of oxygen ( measured at 85 °C and 555 Pa) ?
5. (4) Write the net ionic equation for the reaction, if one occurs, when the following reagents are combined. If no reaction occurs, write NR.
a. KOH + H2SO4 =
b. Na3PO4 + CaCl2 =
Chem 1A Quiz 8B
At. Wt: C = 12.0, H = 1.0, O = 16.0, N = 14.0, Na = 23.0, Al = 27.0, P = 31.0, S = 32.1, Cl = 35.5, Ar = 39.9
Numbers: 0.0821, 1.987, 4.184, 8.314, 14.7, 62.36, 273, 760, 8314, 101325
1. (6) What is the pressure (in Pa) in a 445 mL cylinder, which contains 8.25 g of oxygen at 188.0°C ?
2. (7) What is the density of a 125.0 mL sample of N2O4 (g) at 45°C and 605 torr ?
3. (5) What is the volume at STP of 45.0 mL of nitrogen collected at 155° C and 1655 torr?
4. (8) 6.00 g of aluminum were reacted with excess HCl (aq). What is the volume of hydrogen collected at 55° C and 1.16 atm ?
Chem 1A Quiz 9A
At. Wt: C = 12.0, H = 1.0, O = 16.0, N = 14.0, Na = 23.0, P = 31.0, S = 32.1, Cl = 35.5, K = 39.1, Ba = 137.3
1. (4) What is the maximum number of electrons in
(a) the N shell of electrons
(b) the set of f orbitals
2. (2) Write the symbol of the element with the lowest atomic number, Z, that has a completely filled N shell of electrons.
3. (8) Using the short method of spdf notation, write the electron configuration for bromine. Draw circle(s) around the valence electrons in the configuration you have drawn. Rationalize the oxidation states of bromine in terms of its valence electrons. Assume bromine forms the same ions as chlorine.
4. (3) Using the long method of spdf notation, write the electron configuration for silver.
5. (8) For each of the following: (a) Draw a good electron dot (Lewis) structure
(b) Give the formal charge of each atom
(c) Give the oxidation number of each atom
(i) N2 (ii) ClO3– (Cl is the central atom)
Chem 1A Quiz 10A
At. Wt: C = 12.0, H = 1.0, O = 16.0, N = 14.0, Na = 23.0, P = 31.0, S = 32.1, Cl = 35.5, K = 39.1, Ba = 137.3
Numbers: 0.0821, 1.987, 4.184, 8.314, 14.7, 62.36, 273, 760, 8314, 101325
1. (4) What is the maximum number of electrons in
(a) the P shell of electrons
(b) the set of p orbitals
2. (3) Write the electron configuration for the gold atom by the short method.
3. (2) What is the last completely filled electron shell in the silver atom?
4. (8) For each of the following: (a) Draw a good electron dot (Lewis) structure
(b) Give the formal charge of each atom
(c) Give the oxidation number of each atom
(i) N2 (ii) IO3– (I is the central atom)
5. (1) What is the electron group geometry for a molecule with 4 electron groups?
6. (7) For each of the following molecules, draw a Lewis electron dot structure. Write the VSEPR notation (A = the central atom, X = is an atom bonded to the central atom, and E = is a lone pair of electrons) for each of the molecules.
(a) CO2 (C is central)
(b) H2O (O is central)
(c) NH3 (N is central)
Chem 1A
At. Wt: C = 12.0, H = 1.0, He = 4.0, O = 16.0, N = 14.0, Na = 23.0, Al = 27.0, S = 32.1, Cl = 35.5, K = 39.1
Numbers: .0821, 8.314, 62.36, 273, 101325
1. (6) What is the final temperature of the system, if a 48.50 g piece of aluminum (sp ht = 0.903 J/g° )at 135 °C is put into a calorimeter containing 145 g of water (sp ht = 4.184 J/g° ) at 22.0 ° C ?
2. (5) What is the work (in kJ) done by the system, if 3.00 moles of He (g) are expanded from a volume of 2.00 L to a volume of 13.20 L at a constant pressure of 25.0 atm and temperature of 300K ?
3. (9) When 0.150 mole of C3H8O (g) are burned with excess O2 (g) in a constant pressure calorimeter (with a heat capacity of 89.5 kJ/ºC ) to produce CO2 (g) and H2O (l), the temperature of the calorimeter increased from 21.75ºC to 28.40ºC. What is DH° for the combustion of 1 mole of C3H8O ?
4. (5) Given:
C6H4(OH)2 (aq) = C6H4O2 (aq) + H2 (g) DH° = 177.4 kJ
H2 (g) + O2 (g) = H2O2 (aq) -191.2
H2 (g) + ½O2(g) = H2O (g) -241.8
H2O (g) = H2O (l) - 43.8
Calculate DH° for the reaction :
C6H4O2 (aq) + 2H2O (l) = C6H4(OH)2 (aq) + H2O2 (aq)
Chem 1A Quiz 11A
At. Wt: C = 12.0, H = 1.0, O = 16.0, N = 14.0, Na = 23.0, P = 31.0, S = 32.1, Cl = 35.5, K = 39.1, Ba = 137.3
Numbers: 0.0821, 1.987, 4.184, 8.314, 14.7, 62.36, 273, 760, 8314, 101325
1. (3) Tungsten, W, has a body centered cubic crystal structure. If the radius of the tungsten atom is 139 pm, what is the length of the unit cell edge?
2. (8) What are the molarity and molality of an aqueous solution of H2SO4 which has a density of 1.33 g/mL and contains 71.5% H2SO4 by mass?
3. (7) Calculate DH° for: 2 Fe3O4 (s) + CO2 (g) = 3 Fe2O3 (s) + CO (g)
Given: DH° kJ
Fe2O3 (s) + 3 CO (g) = 2 Fe (s) + 3 CO2 (g) – 28.7
3 FeO (s) + CO2 (g) = Fe3O4 (s) + CO (g) 22.5
FeO (s) + CO (g) = Fe (s) + CO2 (g) 1.3
4. (7) Cerium, Ce, (atomic mass = 140.12) crystallizes in an fcc structure with a unit cell edge length of 516 pm. The density of Ce is 6.657 g/cm3. Use this data to CALCULATE a value for Avogadro’s number.
Chem 1A Quiz 12A
At. Wt: C = 12.0, H = 1.0, O = 16.0, N = 14.0, Na = 23.0, P = 31.0, S = 32.1, Cl = 35.5, K = 39.1, Ba = 137.3
Numbers: 0.0821, 1.987, 4.184, 8.314, 14.7, 62.36, 273, 760, 8314, 101325
1. (8) Sodium crystallizes in a body centered cubic (bcc) structure, with a density of 0.970 g/mL. If the length of its unit cell edge is 438 pm, what is the value of Avogadro’s number based on the data for sodium?
2. (9) A 3.60 M solution of H2SO4 in water has a density of 1.32 g/mL .
(a) What is the molality of the solution?
(b) What is the mole fraction of H2SO4 in the solution?
3. (6) What is the equilibrium vapor pressure at 35°C above a solution of 2.65 moles of volatile C6H12 in 5.75 moles of C5H10O ? (pure C5H10O has a vapor pressure of 225 torr and C6H12 has a vapor pressure of 415 torr at 35°C)
4. (2) What is the mole fraction of C6H12 in the vapor?
Chem 1A Quiz
Atomic weights: Ba = 137.3, C = 12.0, Cl = 35.5, H = 1.0, O = 16.0
1. (10) What are the molality and mole fraction of BaCl2 in a 4.10 M solution of BaCl2 in water? The density of the solution is 1.35 g/mL.
2. (7) What is the equilibrium vapor pressure at 35 C above a solution of 5.65 g of non-volatile C6H12O6 in 65.0 g of C5H10O ? (pure C5H10O has a vapor pressure of 125 torr at 35 C)
3. (8) What is the freezing point of a solution of 3.40 g of C3H8O in 95.0 g of C6H6 ?
For pure C6H6 Kf = –5.10°C/m, tf = 5.50°C, for pure C3H8O Kf = –2.20°C/m, tf = 25.00°C,
