Unit 1
Unit 2
Unit 3
Unit 4
Surprise:)
100
Which element has the valence configuration 3s23p6?
Argon
100
Identify the electron domain geometry and molecular geometry of NI3
Electron domain geometry: tetrahedral
Molecular geometry: trigonal pyramidal
100
State what would happen to a human cell in a hypotonic, isotonic, and hypertonic solution and why.
Hypotonic - water moves into cell (higher ion concentration) and it bursts
Isotonic - no net water movement
Hypertonic - water moves into solution (higher ion concentration) and cell shrinks/crenates
100
N2O4(g) ⇌ 2NO2(g)
At equilibrium, [N2O4] = 0.060 M and [NO2] = 0.210 M.
Calculate the equilibrium constant (Kc) and determine if the reaction is reactant- or product-favored.
Kc = 0.735
Reactants are favored
100
Identify what state of matter and if a phase change is occurring at each point on the following heating curve.
1. solid; no phase change
2. solid to liquid; melting
3. liquid; no phase change
4. liquid to gas; vaporization
5. gas; no phase change
200
Convert -321°F to °C
-196°C
200
Name the compound Zn(ClO2)2
Zinc chlorite
200
A sample of gas has a pressure of 1.5 atm at 320 K. What is the pressure of the sample at 450 K?
2.1 atm
200
2SO2(g) + O2(g) ⇌ 2SO3(g)
State two change that would shift equilibrium towards SO3
Removing SO3
Adding SO2
Adding O2
200
Will table salt (NaCl) dissolve in hexane (C6H12)?
No
300
What occurs when the vapor pressure of a substance is equal to the atmospheric pressure?
The substance boils
300
Which substance has the highest boiling point?
HF, HCl, CF4, SO2, O2
HCl
300
What is the molarity of 3.25 mol KNO3 in 250 mL of solvent?
13.0 M
300
2SO2(g) + O2(g) ⇌ 2SO3(g) ΔH = –198 kJ
Which change(s) will shift the equilibrium toward the products?
a. Increasing the volume of the container
b. Decreasing the volume of the container
c. Increasing the pressure
Both b and c
300
Which of the following solutions would have the highest osmotic pressure?
0.10 M CaCl2
0.10 M Fe(OH)3
0.10 M glucose
0.10 M NaCl
0.10 CaCl2
Fe(OH)3 is insoluble!
400
Calculate the average atomic mass of an element with two isotopes found in the following amounts in nature:
57.30% of isotopes are 19.23 amu
42.70% of isotopes are 21.22 amu
20.08 amu
400
How many sulfur atoms are in 7.80 mol of Al2S3?
1.41 x 1025 sulfur atoms
400
How amount of total solution is needed to produce a 0.3% (m/m) solution containing 0.500 g Na?
167 g of solution
(add 166.5 g of solvent)
400
What is the equilibrium concentration of HF if the equilibrium concentrations of H3O+ and F- are both found to be 1.7 × 10-3 M?
HF(aq) + H2O(l) ⇌ H3O+(aq) + F-(aq)
Ka = 6.8 × 10-4
[HF] = 4.3 x 10-3 M
400
2NOBr(g) ⇌ 2NO(g) + Br2(g) ΔH = +30 kJ
What temperature change shifts equilibrium toward the products?
Increasing the temperature
500
A 15.0 g sample of a metal absorbs 325 J of heat, causing its temperature to rise from 22.0°C to 48.0°C.
What is the specific heat (c) of the metal?
325 J = (15.0 g)(c)(48.0°C - 22.0°C)
q = mcΔT
c = 0.833 J/g*°C
500
Write the products of the following reaction and determine if a precipitate forms
Li2SO4(aq) + NaOH(aq) →
Li2SO4(aq) + NaOH(aq) → LiOH(s) + Na2SO4(aq)
Rule 6: hydroxide does not have exception cation
500
Identify 1) the following regions of the reaction curve, 2) if the reaction is exothermic or endothermic, and 3) what portion of the graph determines the rate of the reaction
a. reactants
b. activation energy (EA)
c. transition state
d. products
e. ΔG
2. Exothermic
3. b, the activation energy
500
A solution has [OH-] = 2.5 x 10-4 M. Calculate the pH of the solution.
pH = 10.40
500
What is everyone getting as their final grade in CHEM:1070?
A+!