Answer:
The Combined Gas Law shows that the pressure of a gas is inversely proportional to volume and directly proportional to temperature. Avogadro's Law shows that volume or pressure is directly proportional to the number of moles of gas. Putting these together leaves us with the following equation:
P1×V1T1×n1=P2×V2T2×n2(11.9.1)
As with the other gas laws, we can also say that (P×V)(T×n) is equal to a constant. The constant can be evaluated provided that the gas being described is considered to be ideal.
The Ideal Gas Law is a single equation which relates the pressure, volume, temperature, and number of moles of an ideal gas. If we substitute in the variable R for the constant, the equation becomes:
P×VT×n=R(11.9.2)
The Ideal Gas Law is conveniently rearranged to look this way, with the multiplication signs omitted:
PV=nRT(11.9.3)
The variable R in the equation is called the ideal gas constant.
Explanation:
Answer:
The temperature will increase or doubled.
Explanation:
In Amonton's Law, it states the pressure of a given amount of gas is directly proportional to its temperature on Kelvin scale when the volume is held constant.
The electrons are electrically charged
Cation is formed when an atom of mercury (Hg) loses two electrons.
Answer:
The correct answer is 16 gram per mole.
Explanation:
Let A be the gas helium, and B be the unknown gas. It is clearly mentioned in the question that the effusion rate of helium gas is two times more than that of gas B. The molar mass of helium is 4.0 gram per mole. To solve the problem, Grahm's law is used, that is,
Rate of effusion A/rate of effusion B = √ (Molar mass B/Molar mass of A
2.0 = √Molar mass of B/4.0 gram per mole.
Now squaring both the sides we get,
4.0 = Molar mass of B / 4.0
The molar mass of B = 16 gram per mole.
