which gas has the greatest kinetic energy at STP?
a)He
b)Ne
c)Ar
d) None of the above(All have the same kinetic energy)
how do I solve for this?
ALL HAVE THE SAME>
ALL HAVE SAME.
ALL HAVE SAME
To determine which gas has the greatest kinetic energy at STP (Standard Temperature and Pressure), you need to consider the concept of kinetic theory. According to the kinetic theory of gases, the average kinetic energy of gas molecules is directly proportional to the temperature.
To solve this, we need to compare the temperatures at STP for each gas. STP is defined as a temperature of 273.15 K (0 °C) and a pressure of 1 atmosphere (atm).
First, let's calculate the molecular mass of each gas:
a) He (Helium): 4 atomic mass units (amu)
b) Ne (Neon): 20 amu
c) Ar (Argon): 40 amu
Since we know the molecular mass, we can determine the root mean square velocity (v) of each gas at a given temperature using the equation:
v = √(3kT / m)
Where:
v = root mean square velocity
k = Boltzmann constant (1.38 × 10^-23 J/K)
T = temperature in Kelvin
m = molecular mass
For STP, T = 273.15 K
Using this information, we can calculate the root mean square velocity for each gas. Since kinetic energy is directly proportional to the square of the velocity (KE = 0.5mv^2), the gas with the highest velocity will also have the greatest kinetic energy.
To compare the velocities, we only need to compare the molecular masses directly without calculating the actual velocities.
Comparing the molecular masses:
a) He: 4 amu
b) Ne: 20 amu
c) Ar: 40 amu
Since helium (He) has the lowest molecular mass, it will have the highest root mean square velocity and thus the greatest kinetic energy at STP.
Therefore, the answer is a) He (Helium).