Ch. 6
Ch. 7
Ch. 8
Ch. 9
Challenge Questions
100
If you're in the lab and calculate that you could get 2.837 g of product in a perfect world. In reality, you get 1.53 g. What is your percent yield?
54%
100
Name the element with the electron configuration
1s22s22p63s2
Magnesium (Mg)
100
Is CH3F polar or nonpolar?
polar
100
The atmospheric pressure in La Paz, capital of Bolivia, is 0.632 atm. Calculate the atmospheric pressure in mmHg and torr.
480. mmHg
100
Electron configuration for the Ga3+ ion
1s22s22p63s23p63d10
200
Calculate the energy required to heat 824.0 g of ammonia from 54.6°C to 66.9°C. Assume the specific heat capacity of ammonia is 4.70 J/(g·K).
47.6 kJ
200
Rank the following atoms/ions in order of DECREASING size:
Br, Cl, Br-
Br- > Br > Cl
200
Rank the following elements in order of decreasing electronegativity:
O, C, N
O > N > C
200
If a gas at 25.0°C occupies 3.60 liters at a pressure of 1.0 atm, what will be its volume at a pressure of 2.50 atm?
1.44 L
200
What mass of water is produced by the reaction of 6.4 g of oxygen gas? The reaction has been balanced for you.
2 C8H18 + 25 O2 → 16 O2 + 18 H2O
2.6 g of water
300
Use the balanced equation below. How many moles of oxygen are needed to produce 0.085 mol of water?
2C2H2 + 5O2 → 4CO2 + 2H2O
0.21 mol
300
What is the electron configuration for Ne2+
1s22s22p4
300
Draw the Lewis structure for N22-
300
A large silo has a volume of 600 L at a pressure of 732 torr. What volume would the tank need to be compressed to have a pressure of 512 torr?
858 L
300
Suppose 210 g of undecane are burned in air at a pressure of exactly 1 atm and a temperature of 11.0°C. Calculate the volume of carbon dioxide gas that is produced.
Balanceid Equation: C11H24 + 17 O2 -> 11 CO2 + 12 H2O
344 L
400
Identify the limiting reactant:
23 g of ethane with 21.8 g of oxygen
2 CH3CH3(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)
oxygen (O2)
400
What is the condensed electron configuration for indium (In)?
[Kr]5s24d105p1
400
What is the molecular geometry for HCO2-
trigonal planar
400
A 5.00 L tank at 4.2°C is filled with 3.05 g of dinitrogen difluoride gas and 9.75 g of trifluoride gas. Assume both gases behave as ideal gases under these conditions.
Calculate the partial pressure of dinitrogen difluoride.
0.210 atm
400
Aqueous sulfuric acid (H2SO4) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium sulfate (Na2SO4) and liquid water (H2O). If 8.64 g of sodium sulfate is produced from the reaction of of sulfuric acid and 7.85 g of sodium hydroxide, calculate the percent yield of sodium sulfate.
Round your answer to 3 sig figs
62%
500
Use the equation below. What mass of NH3 is consumed to make 8.76 g of O2?
4 NH3 + 5 O2 → 4 NO + 6 H2O
3.73 g
500
Rank the following in order of decreasing ionization energy:
Ga, He, Ra
He> Ga > Ra
500
What is the molecular geometry of hydrogen cyanide (HCN)?
linear
500
An arctic weather balloon is filled with 24 L of helium gas. The temperature inside the shed is 13°C. The balloon is then taken outside, where the temperature 3°C. Calculate the new volume of the balloon.
23.2 L
500
Suppose 0.320 kg of nonane are burned in air at a pressure of exactly 1 atm and a temperature of 12.0°C. Calculate the volume of carbon dioxide gas that is produced.
C9H20 (l) + 14 O2 (g) -> 9 CO2 (g) + 10 H2O (g)
525.0 L