Atomic Structure, Nomenclature, & Formulas
Chemical Reactions
Solution Chemistry
Thermochemistry
Quantum Theory & Behavior of Light
100
How many hydrogen atoms are in 2.5 g pharmacolite,
CaHAsO4 dot 2H2O? (M = 216.0)
3.48 x 1022
100
Which metal reacts most vigorously with water?
a. Na
b. Mg
c. K
d. Ca
c. K
100
Which diagram represents the most concentrated solution?
C
100
Given the enthalpy changes
A + B --> C. ∆H= –35 kJ•mol–1
A + D --> E + F. ∆H= +20 kJ•mol–1
F --> C + E ∆H= +15 kJ•mol–1
What is ∆H for the reaction 2A + B + D --> 2 F?
–30 kJ•mol–1
200
Which pair has the same number of electrons?
a. F-, Mg2+
b. Ne, Ar
c. Br-, Se
d. Al3+, P3-
a. F-, Mg2+
200
One mole of which hydrocarbon requires 8 mol O2 to achieve complete combustion to give carbon dioxide and water?
a. C3H8
b. C4H10
c. C5H10
d. C5H12
d. C5H12
200
In a titration experiment, 15.0 mL of 0.146 M H2SO4 is titrated and neutralized by 13.1 mL of NaOH solution. What is the concentration of the NaOH solution?
0.335 M
200
A block of iron at 25.0 °C is placed in 500. g of water at 35.0 °C in an insulated container. The final temperature of the solution is 32.0 °C. What is the mass of the iron block? The specific heat of iron is 0.450 J/g°C.
1990 g
200
Which gas phase atom has no unpaired electrons in its ground state?
a. Li
b. Be
c. B
d. C
b. Be
300
The formula for terbium phosphate is TbPO4. The formula for terbium sulfate is:
Tb2(SO4)3
300
Which is an example of an oxidation reduction reaction?
D. Pb(s) + PbO2(s) + 2H2SO4(aq) --> 2PbSO4(s) + 2H2O(l)
300
What is the concentration of H2O2 in a solution that is 30.0% by mass hydrogen peroxide and has a density of 1.1 g/mL?
9.79 M
300
What is ΔH° for the reaction shown?
2H2S(g) + 3O2(g) --> 2H2O(l) + 2SO2(g)
-1124.1 kJ mol-1
300
A fluorescent dye absorbs a photon of light at 485 nm and emits a photon of light at 540 nm. How much energy is lost as heat?
4.17 x 10-20 J
400
Alkali metals (group 1) differ from alkaline metals (group 2) of the same period in what way?
a. Alkali metals have larger ionic radii
b. Alkali metals have higher melting points
c. Alkali metals have greater first ionization energies
d. Alkali metals have greater densities
a. Alkali metals have larger ionic radii
400
Given the following balanced chemical equation, if 40.8 grams of C6H6O3 is reacted giving a 39% yield, how many grams of H2O are produced?
C6H6O3 + 6O2 --> 6CO2 + 3H2O
6.81 g
400
A 25.0 mL sample of 0.15 M silver nitrate, AgNO3, is reacted with a 3.58 g sample of calcium chloride, CaCl2 (M = 111.0). Which of the following statements is true?
a. Silver nitrate is the limiting reactant and calcium nitrate precipitates
b. silver nitrate is the limiting reactant and silver chloride precipitates
c. calcium chloride is the limiting reactant and calcium nitrate precipitates
d. calcium chloride is the limiting reactant and silver chloride precipitates
b. silver nitrate is the limiting reactant and silver chloride precipitates
400
100.0 g of nickel at 150 °C was placed in 1.00 L of water at 25.0 °C. The final temperature of the water was 26.3 °C. What is the specific heat of nickel? (cwater = 4.184 J/g °C)
0.44 J/g °C
400
Which period 3 element has these successive ionization energies?
Silicon
500
Chlorine occurs naturally as a mixture of two isotopes with atomic masses of 34.97amu and 36.97amu. What are the relative abundances of these two isotopes?
a). 24% and 76%
b). 50% and 50%
c). 76% and 24%
d). 95% and 5%
C). 76% and 24%
500
What is the net ionic equation for a reaction between Na2S (aq) and Pb(NO3)2 (aq).
S2-(aq) + Pb2+ ----> PbS (s)
500
A solution is made by dissolving 60g of NaOH in enough distilled water to make 300mL of a stock solution. What volumes of this solution and distilled water, when mixed will result in a solution that is approximately 1M NaOH?
20mL stock, 80 mL distilled water
500
What mass of Cl2(g) is needed to release 45.2kJ of energy as heat during the reaction of carbon and chlorine gas?
C(s) + 2Cl2(g) ---> CCl4(l)
standard enthalpy of the rxn= -135. 4 kJ mol
a). 0.67g
b). 11.8g
c).23.7g
d).47.3g
d). 47.3g
500
C