A.
Because you increase the concentration of the reactants, it means that there are more molecules of the reactants present in a smaller amount of space.
This being the case, there is a higher chance that these molecules will collide with enough energy to overcome the activation barrier.
The other ones are completely wrong, but if you would like an explanation as to why they are, just ask :)
This is how far I got:
put equation 3. into 1. together with h = 5:
4.
when I double m₁ the ratio becomes:
5.
when I put these to ratios back into equation nr 1 and nr2, I find the ratio:
and new v₁ = 2.95
I'm not sure this is correct.
D. Must be implemented using a computer.
It is possible to make scientific models without computers and/or other technology.
Answer:
35.5KJ
Explanation:
Heat transferred (Q) = change in internal energy (∆U) + work done (W)
Q = 30KJ, W = 500Nm = 500J = 500/1000KJ = 0.5KJ
∆U = Q - W = 30 - 0.5 = 25.5KJ
∆U = final energy (U2) - initial energy (U1)
U2 = ∆U + U1 = 25.5 + 10 = 35.5KJ
Explanation:
u = 0m/s
v = 30m/s
a = 2m/s²
Using Kinematics, we have v = u + at.
Therefore t = (v - u) / a
= (30 - 0) / (2) = 15 seconds. (B)