Ok, so this is what I got, and I hope this helps others out. Good Luck.
What are the full and abbreviated electron configurations for P?
Full: 1s22s22p63s23p3
Abbreviated= [Ne]3s23p3
2.) Describe (using what you know about gases) why a can of compressed air gets cold after you use it to clean your keyboard.
Thermodynamics in Action... use a web search
3.) A 325 mL sample of gas is initially at a pressure of 721 torr and a temperature of 32°C. If this gas is compressed to a volume of 286 mL and the pressure increases to 901 torr, what will be the new temperature of the gas (reported to three significant figures in °C)
•
P1V1 =
P2V2 • T1 T2
• T2 =
P2V2T1 • P1V1
Convert Celsius into Kelvin Kelvin = 273+oC
K=273+32
K=305
•
(721 torr x 325mL) =
(901 torr x 286mL)• 305K T2
• T2 =
(901 torr x 286mL x 305K)• (721 torr x 325mL)
• T2 = 335.41K
• 335.41-273= 62.41
• T2 = 62.4oC
4.) A KNO3 solution is made using 8.84 g of KNO3 and diluting to a total solution volume of 1.50L. Calculate the molarity and mass percent of the solution. Density of the solution = 1.05g/mL
molarity (M) = moles solute/liters solution
First, convert 8.84 g KNO3 to mol KNO3.
8.84 g KNO3 * (1 mol KNO3/101.14 g KNO3) = 0.0874 mol KNO3
M = 0.0874 mol KNO3/1.50 L solution
M = 0.058 M
% of mass solution = mass solute/ total mass * 100. (total mass = mass of solute + mass of solvent)
mass of solute = 8.84 g
mass of solvent = 1L = 1000 mL = 1000mg
mass of solution = 8.84g+1000mg=1008.84 mg
8.84g/1008.84mg*100= 0.88%
Molarity = 0.058 M
Mass % = 0.88%
5.) If a 10.00mL sample of unknown concentration of HF is titrated with 31.84mL of 0.1340M NaOH, what is the concentration of HF?
Use the formula M1*V1=M2*V2
Here, we are looking for M1.
10.00ml * x = 31.84mL * 0.134M
10.00ml * x = 4.267M
x = 4.267/10.00
x = 0.4267M
6.) Provide an example of a common amine and where you might find it.
Ammonia look up text page 648 in Chapter 8
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