A chemist performs the following reaction:
1 answer:
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<u>Answer:</u>
211.9 J
<u>Explanation:</u>
The molecules of water release heat during the transition of water vapor to liquid water, but the temperature of the water does not change with it.
The amount of heat released can be represented by the formula:
where = heat energy,
= mass of water and
= latent heat of evaporation.
The latent heat of evaporation for water is and the mass of the water is
.
The amount of heat released in this process is:
211.9 J
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