Ch. 10: IMFs, heat of fusion/vaporization
How do IMFs affect boiling points, melting point, and vapor pressure?
stronger IMFs increase boiling point and melting points
stronger IMFs decrease vapor pressure
What is the better solvent for I2: H2O or CH3(CH2)4CH3?
What is the better solvent for NaCl: H2O or CH3(CH2)4CH3?
What is the better solvent for KCl: H2O or CCl4?
For I2: CH3(CH2)4CH3
For NaCl: H2O
For KCl: H2O
Write the equilibrium constant expression for the following reaction:
2 CuI(s) + I2(aq) → 2 Cu2+(aq) + 4 I-(aq)
[I-]4[Cu2+]2 / [I2]
Name 3 strong acids
HCl, HBr, HI, HNO3, HClO3, HClO4, H2SO4
What intermolecular forces are present in the following compounds:
Ar2
HClO
hydrogen chloride
ammonia
Ar2: dispersion only
HClO: dispersion, dipole-dipole, hydrogen bonding
hydrogen chloride: dispersion, dipole-dipole
ammonia: dispersion, dipole-dipole, hydrogen bonding
A chemist prepares a solution of silver(I) nitrate (AgNO3) by measuring out 94.1μmol of silver(I) nitrate into a 250 mL volumetric flask and filling the flask to the mark with water.
Calculate the concentration in M of the chemist's silver(I) nitrate solution
3.76 x 10-4 M (mol/L)
Consider the reaction below:
2H2S(g) + 3O2(g) -> 2SO2(g) + 2H2O(g)
What would happen to the equilibrium if you removed some H2S?
the reaction would shift to the left
Identify the Bronsted-Lowry acid and base in the following equation:
HCl(aq) + NH3(aq) -> Cl-(aq) + NH4+(aq)
Acid: HCl
Base: NH3
In each pair of compounds, which one has the higher boiling point?
CS2 vs. C2H4
GeH4 vs. PbH4
Ar vs. Ne
CS2
PbH4
Ar
A chemist must dilute 90.4 mL of 6.71 mM aqueous copper(II) fluoride (CuF2) solution until the concentration falls to 1.00 mM. Calculate the final volume, in liters, round your answer to 3 sig figs.
0.607 L
What is the solubility constant (Ksp) for CuCO3?
Ksp = [Cu2+][CO32-]
if the pH of a solution is 3, what is the pOH?
11
Are the following compounds capable of H-bond between itself and/or between itself and water:
CHClO
HF
CHClO: not between itself but yes between itself and water
HF: yes between itself and between itself and water
In the following reaction, what mass of NaHCO3 is needed to neutralize 150 mL of 0.051 M HCl solution?
HCl + NaHCO3 → NaCl + H2O + CO2
0.64 g of NaHCO3
Consider the following reaction:
Fe2O3(s) + 3CO(g) -> 2Fe(s) + 3CO2(g)
Which reaction vessel would have a higher initial rate of reaction given the following conditions:
Vessel A: 2.0 L / 1200 °C
Vessel B: 4.0 L / 1100 °C
Vessel A
higher temp= more reactions between atoms
lower volume= more reactions between atoms
What is the equilibrium constant equation for the reaction of acetic acid (HCH3CO2)?
[H3O+][CH3CO2-]/[HCH3CO2]
Calculate the amount of heat needed to melt 32.4 g of acetic acid and bring it to a temperature of 109.8°C.
(The molar mass of acetic acid is 60.05 g/mol. The heat of fusion for acetic acid is 11.73 kJ/mol. The change in temp is 98 K. The specific heat capacity for acetic acid is 2.053 J/g*K.)
12.85 kJ
A chemistry student weighs out 0.0712 g of phosphoric acid (H3PO4) into 250 mL flask and dilutes to the mark with water. He plans to titrate the acid with 0.0600 M NaOH solution.
Calculate the volume of NaOH in mL needed to reach the final equivalence point. The balanced equation is shown below:
H3PO4 + 3 OH- → PO43- + 3 H2O
36.3 mL
Determine Kc for the following reaction:
Ti(s) + 2 Cl2(g) → TiCl4(l)
The reaction happens in a 7.4 L vessel.
Ti = 3.11 g, Cl2 = 2.71 g, TiCl4 = 2.25 g
(write out the expression for Kc, and make sure you convert everything into concentrations!)
Kc = 3743.4
A chemist dissolves 431 mg of HCl in 150 mL of solution. Calculate the pH of the solution.
(hint: the molar mass of HCl is 36.458 g/mol)
pH = 1.1034