Answer:
745.4K ~ 472.3 C
Explanation:
This is an Ideal Gas Law problem where we have to manipulate the equation a bit. Let's start with the basic:
PV = nRT will be used for both the initial and final, so we will rearrange this problem to state:
(V(initial))/(T(Initial)) = nR/P
Since we know that the pressure, number of moles of He, and ideal gas constant (R) remain the same from start to finish so we can write the problem as such:
(V(initial))/(T(Initial)) = nR/P = (V(final))/(T(final))
or
(V(initial))/(T(Initial)) = (V(final))/(T(final))
Now lets define some of these values:
T(initial) = 25degree (assuming degrees Celsius) ~ 298.15K
V(initial) = 2.0L
V(final) = 5.0L
T(final) = ?
Since we are solving for T(final) let's rearrange the problem once more to be solving for T(final):
T(final) = (V(final)T(Initial))/V(initial)
Now plug in your values:
T(final) = (5.0L*298.15K)/(2.0L) ~ 745.4K ~ 472.3degrees Celsius
Answer:
Yes it is related
Explanation:
Consider 2 points in a rectangular co-ordinate system
The distance between them can be found by
d =
This is clear from the figure attached below
I think its when there are higher energies.
43.75N (assuming only friction)
Answer:
cross out the false piece in blue and write the true piece in red