(CO2) (O2) (He) (N2) (CH4) (Imagine these are balloons with the specified gas inside)
1 answer:
Answer:
Highest speed: He
Lowest speed: CO2
Explanation:
The rms speed (average speed) of the molecules/atoms in an ideal gas is given by:
where
R is the gas constant
T is the absolute temperature of the gas
M is the molar mass of the gas, which is the mass of the gas per unit mole
From the equation, we see that at equal temperatures, the speed of the molecules in the gas is inversely proportional to the molar mass: the higher the molar mass, the lower the speed, and vice-versa.
In this problem, we have 5 gases:
(CO2) (O2) (He) (N2) (CH4)
Their molar mass is:
CO2: 44 g/mol
O2: 16 g/mol
He: 4 g/mol
N2: 14 g/mol
CH4: 16 g/mol
The gas with lowest molar mass is Helium (He): therefore, this is the gas with greatest average speed.
The gas with highest molar mass is CO2: therefore, this is the gas with lowest average speed.
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Answer:
a)
b)
d)
d)
Explanation:
From the question we are told that:
Moles of N2
Atmospheric pressure
Temperature
Initial heat
a)
Generally the equation for change in temperature is mathematically given by
Where
b)
Generally the equation for ideal gas is mathematically given by
For v double
Therefore
Total Work-done
c)
Generally the equation for amount of heat added is mathematically given by
d)
Generally the equation for change in internal energy of the gas is mathematically given by