Students set up three trials of an experiment to test the
1 answer:
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Gay-Lussac's law gives the relationship between pressure and temperature of gas. For a fixed amount of gas, pressure is directly proportional to temperature at constant volume.
P/T = k
where P - pressure , T - temperature and k - constant
parameters for the first instance are on the left side and parameters for the second instance are on the right side of the equation
substituting the values in the equation
T = 4342 K
initial temperature was 4342 K
P/T = k
where P - pressure , T - temperature and k - constant
parameters for the first instance are on the left side and parameters for the second instance are on the right side of the equation
substituting the values in the equation
T = 4342 K
initial temperature was 4342 K
Answer : The value of work done for the system is 1144.69 J
Explanation :
First we have to calculate the moles of
Molar mass of = 65.01 g/mole
Now we have to calculate the moles of nitrogen gas.
The balanced chemical reaction is,
From the balanced reaction we conclude that
As, 2 mole of react to give 3 mole of
So, 0.311 moles of react to give
moles of
Now we have to calculate the volume of nitrogen gas.
Using ideal gas equation:
where,
P = Pressure of gas = 1.00 atm
V = Volume of gas = ?
n = number of moles = 0.466 mole
R = Gas constant =
T = Temperature of gas =
Putting values in above equation, we get:
As initially no nitrogen was present. So,
Volume expanded = Volume of nitrogen evolved
Thus,
Expansion work = Pressure × Volume
Expansion work = 1.00 atm × 11.3 L
Expansion work = 11.3 L.atm
Conversion used : (1 L.atm = 101.3 J)
Expansion work = 11.3 × 101.3 = 1144.69 J
Therefore, the value of work done for the system is 1144.69 J