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Question 2 [25]
Suppose that the latest census indicates that for every 10 young people available to work only 4 are
employed. Suppose a random sample of 20 young graduates is selected.
Required:
a) What is the probability that they are all employed?
b) What is the probability that none of them are employed?
c) What is the probability that at least four are employed?
d) What is the probability that at most fifteen are employed?
e) What is the probability that the number of young graduates who are employed is greater than
ten but less than fifteen?
f) What is the expected number of graduates who are not employed?
g) What is the standard deviation for the number of graduates who are not employed?
a gas with a pressure of 845 torrs occupies 11.0 l what will the pressure be for a volume of 2.50 l if the temperature remains constant
The ideal gas law relates the amount of gas present to its pressure, volume, and temperature. The ideal gas law is typically written as
đđ=đđ đ
Â
where đ is the pressure, đ is the volume, đ is the number of moles of gas, đ  is the ideal gas constant, and đ is the temperature.
Rearrange the equation to solve for đ.
What is the temperature of 0.597 mol of an ideal gas with a volume of 8.22 L and a pressure of 1.678 atm?
A flexible container at an initial volume of 8.15 L contains 5.51 mol of gas. More gas is then added to the container until it reaches a final volume of 17.1 L. Assuming the pressure and temperature of the gas remain constant, calculate the number of moles of gas added to the container.
a gas with a pressure of 845 torrs occupies 11. o l what will the pressure be for a volume of 2.50 l if the temperature remains constant
What mass of C4H6 must react to produce 43.2 L of CO2 gas at 499 K and 2.57 atm.Â
2C4H6(g)+11O2(g)â¶8CO2(g)+6H2O(l)
Â
First, use the ideal gas equation to calculate the moles of CO2.
Then, calculate the mass of C4H6 from the moles of CO2. Show the conversions required to solve this problem.
What mass of Al2O3 is produced when 13.1 L of O2 gas react with Al at 482 K and 3.40 atm.Â
4Al(s)+3O2(g)â¶2Al2O3(g)
Â
First, use the ideal gas equation to calculate the moles of O2.Â
Then, calculate the mass of Al2O3 from the moles of O2. Show the conversions required to solve this problem.
If 34.5 mol of an ideal gas occupies 11.5 L at 31.00 âC, what is the pressure of the gas?
Calculate the mass of Kr in a 4.59 L cylinder at 34.2 âC and 3.28 bar .
The ideal gas law relates the amount of gas present to its pressure, volume, and temperature. The ideal gas law is typically written as
đđ=đđ đ
Â
where đ is the pressure, đ is the volume, đ is the number of moles of gas, đ  is the ideal gas constant, and đ is the temperature.
Rearrange the equation to solve for đ.
What is the pressure of 0.293 moles of an ideal gas at a temperature of 298.0 K and a volume of 4.62 L?Â
