The average kinetic energy of a gas when the particles of the gas collide against each other at a constant temperature and volume will not changes.
<h3>What is average kinetic energy?</h3>
The product of half the mass of each gas molecule with the square of root mean square speed is the average kinetic energy of the molecules.
And this average kinetic energy is deirectly proportional to the absolute temperature of the system but in the given question temperature and volume of the gas is constant. So that there is no change in average kinetic energy of molecules when they collide.
Hence no change in the average kinetic energy of a gas takes place.
To know more about average kinetic energy, visit the below link:
brainly.com/question/13868723
#SPJ1
By Gayle-Lussac's law, the pressure and temperature of a fixed volume and amount of gas is directly proportional.
Thus,
P/T = constant
So if the temperature is increased four times, the pressure is also increased four times.
The answer is C Nuclear Regulatory Commission
Answer:
Learn from their experiment and know the possible results from trial and error
Step 1: Change density from g/mL to g/L;
0.807 g/mL = 807 g/L
Step 2: Find Moles of N₂;
As,
Density = Mass / Volume
Or,
Mass = Density × Volume
Putting Values,
Mass = 807 g/L × 1 L
Mass = 807 g
Also,
Moles = Mass / M.mass
Putting values,
Moles = 807 g / 28 g.mol⁻¹
Moles = 28.82 moles
Step 3: Apply Ideal Gas Equation to Find Volume of gas occupied,
As,
P V = n R T
V = n R T / P
Putting Values, remember! don't forget to change temperatue into Kelvin (25 °C + 273 = 298 K)
V = (28.82 mol × 0.08206 atm.L.mol⁻¹.K⁻¹ × 298 K) ÷ 1 atm
V = 704.76 L
