Answer:
Explanation:
Given
Required
Calculate the number of moles
We'll apply the following formula to solve this question
Where
The above equation is an illustration of the ideal gas law
Substitute values for p, V, R and T in:
<em>Hence, there are 243.605 moles</em>
Answer:
The new temperature of the nitrogen gas is 516.8 K or 243.8 C.
Explanation:
Gay-Lussac's law indicates that, as long as the volume of the container containing the gas is constant, as the temperature increases, the gas molecules move faster. Then the number of collisions with the walls increases, that is, the pressure increases. That is, the pressure of the gas is directly proportional to its temperature.
Gay-Lussac's law can be expressed mathematically as follows:
Where P = pressure, T = temperature, K = Constant
You want to study two different states, an initial state and a final state. You have a gas that is at a pressure P1 and at a temperature T1 at the beginning of the experiment. By varying the temperature to a new value T2, then the pressure will change to P2, and the following will be fulfilled:
In this case:
Replacing:
Solving:
T2= 516.8 K= 243.8 C
<u><em>The new temperature of the nitrogen gas is 516.8 K or 243.8 C.</em></u>
<u>Answer:</u> The volume of the vessel is and total internal energy is 162.0 kJ.
<u>Explanation:</u>
or,
where,
P = pressure of container = 700 kPa
V = volume of container = ? L
m = Given mass of R-134a = 3.98 kg = 3980 g (Conversion factor: 1kg = 1000 g)
M = Molar mass of R-134a = 102.03 g/mol
R = Gas constant =
T = temperature of container =
Putting values in above equation, we get:
Converting this value into , we use the conversion factor:
So,
or,
where,
U = total internal energy
m = given mass of R-134a = 3.98 kg = 3980 g (Conversion factor: 1kg = 1000g)
M = molar mass of R-134a = 102.03 g/mol
R = Gas constant =
T = temperature =
Putting values in above equation, we get:
Converting this into kilo joules, we use the conversion factor:
1 kJ = 1000 J
So, 161994.6 J = 162.0 kJ
Hence, the volume of the vessel is and total internal energy is 162.0 kJ.