On the left a Circuit A, which is a square box. The top, left, and right sides have circles with X's in them. The bottom side ha
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Answer : The mass of at temperature
28.47 g.
The mass of at temperature
29.51 g.
Solution : Given,
Pressure of gas = 1.35 atm
Temperature of gas =
Volume of gas =
Molar mass of = 65 g/mole
Part 1 : First we have to calculate the moles of gas at temperature . The gas produced in the given reaction is
.
Using ideal gas equation,
where,
P = pressure of the gas
V = volume of the gas
T = temperature of the gas
n = number of moles of gas
R = Gas constant = 0.0821 Latm/moleK
Now put all the given values in this formula, we get
By rearranging the terms, we get the value of 'n'
The moles of = 0.7015 moles
The given balanced reaction is,
As, 32 moles of produced from 20 moles of
So, 0.7015 moles of produced from
moles of
Now we have to calculate the mass of .
Therefore, the mass of needed are 28.47 g.
Part 2 : We have to calculate the moles of gas at temperature and same volume & pressure.
Using ideal gas equation,
Now put all the given values in this formula, we get
By rearranging the terms, we get the value of 'n'
The moles of = 0.726 moles
The given balanced reaction is,
As, 32 moles of produced from 20 moles of
So, 0.726 moles of produced from
moles of
Now we have to calculate the mass of .
Therefore, the mass of needed are 29.51 g.