In the bohr model of the hydrogen atom, the energy required to excite an electron from n = 2 to n = 3 is <u>greater than</u> the energy required to excite an electron from n = 3 to n = 4
Bohr's energy levels:
The essential concept of Bohr's atomic model is that electrons occupy specified orbitals that call for the electron to have a certain amount of energy. An electron needs to be in one of the permitted orbitals and have the correct amount of energy needed for that orbit in order to be in the electron cloud of an atom. An electron would require less energy to orbit near the nucleus, while an electron would need more energy to orbit away from the nucleus. Energy levels are the potential orbits. One of Bohr's models' flaws was that he was unable to explain why just specific energy levels or orbits were permitted.
It is evident that the energy required to escape an electron from n=2 to n=3 is greater than the energy required to exit an electron from n=3 to n=4. This is because as n increases, the energy levels move closer to one another.
Learn more about Bohr's model here:
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Answer:
The square root of the molar mass of B ÷ the square root of the molar mass of A
Explanation:
Graham’s Law applies to the effusion of gases:
The rate of effusion (r) of a gas is inversely proportional to the square root of its molar mass (M).
If you have two gases A and B, the ratio of their rates of effusion is
Answer: 28.3 g/mol
Explanation:
According to the ideal gas equation:'
P= Pressure of the gas = 0.951 atm
V= Volume of the gas = 280 mL = 0.28 L (1L=1000 ml)
T= Temperature of the gas = 25°C=(25+273)K=298 K (0°C = 273 K)
R= Value of gas constant = 0.0821 Latm/K mol
To calculate the moles, we use the equation:
Thus the molar mass of the gas is 28.3 g/mol.