please answer the following questions by typing, thanks. 1. How different is the
ID: 1050623 • Letter: P
Question
please answer the following questions by typing, thanks.
1. How different is the measured volume from the volume if it had been obtained under STP conditions? Is the difference greater than an assumed measurement error of 5%? If not, why should we go to all this trouble to make this calculation?
2. All gases should have the same standard volume of 22.4141 L. If your value is different, then comment on the sources of error in the experiment.
3. What is the volume occupied by 11 moles of oxygen gas at STP?
4. What is the mass in grams of 10.0 L of methane (CH4) gas at STP?
Explanation / Answer
Ans. 1. Difference in volume = Theoretical value – experimental (observed value)
% difference in volume =
[ (Theoretical value – experimental value) / Theoretical value ] x 100
Note: The theoretical and experimental value is obtained from your experiment. From the available data, it’s not possible to get the values.
Ans. 2. Sources of errors in the experiment:
Using, ideal gas equation, pV = nRT
Instrumental or human errors yielding erroneous values of one or more measurements (p, n, T) increases difference between thermotical and experimental value volume.
Ans. 3. 1 mol has volume of 22.4 L at STP
So, volume occupied by 11 moles = 11 x 22.4141 L
= 246.5551 L
Ans.4. Using pV = nRT
Given,
V = (nRT/ p) = 22.4141 L at STP ; where, n = 1= number of moles of gas, at STP
Suppose the number of moles in 10 L = Yn or Y moles
Now,
10 L = (Yn. RT/ p) = Y x (nRT/ p) = Y x 22.4141 L
Or, Y = 10 L / 22.4141 L = 0.4461
Thus, number of moles in 10 L methane = 0.4461
Mass of methane = number of moles x molecular mass
= 0.4461 moles x 16.043 g mol-1
= 7.16 g
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