Which of the following would double the pressure on a contained gas at constant temperature?
1 answer:
Answer: C. doubling the number of particles in the container
Explanation: According to the ideal gas equation:'
P= Pressure of the gas
V= Volume of the gas
n= number of moles
T= Temperature of the gas
R = gas constant
As the gas is contained in a container with fixed volume and temperature is also constant.
Therefore, the pressure will double when number of moles or number of particles double.
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Answer:
Explanation:
The formula we must use is given to us:
q is the energy, m is the mass, and L(vapor) is the latent heat of vaporization.
The energy is what we calculate and the mass is 2 kilograms. We need to find the latent heat of vaporization, which is on the table.
- We know the sample is copper.
- Find that element on the table, then the third box tells us it's latent heat of vaporization is 4730 kJ/kg
Now we know:
Substitute the values into the formula.
Multiply. Note that the kilograms (kg) will cancel each other out.
<u>9460 kilojoules</u> are required to vaporize 2 kilograms of copper.
Answer:
The chemical formula of the gas is .
Explanation:
The difference between the container with gas and empty container is equal to the mass of the gas.
Let the gas be
Mass of the gas = m
Molar mass of diatomic gas = M
Pressure of the gas = P = 1.80 atm
Volume of the gas = V = 4.6 L
Temperature of the gas= T = 27.0 C = 27.0 + 273 K = 300 K
Moles of diatomic gas = n =
Using ideal gas equation:
Atomic mass of the element X =
The element is nitrogen and the diatomic gas is .