Did I Make a Calculation Error in the Elastic Collision of Two Football Players?

  • Thread starter Thread starter LSarah6
  • Start date Start date
  • Tags Tags
    Biomechanics
AI Thread Summary
The discussion centers on a calculation involving an elastic collision between two football players, where Player 1 has a mass of 75 kg and a velocity of 6 m/s, while Player 2 has a mass of 150 kg and a velocity of -3 m/s. The user applied the provided equation for final velocity but arrived at 3 m/s for Player 2, conflicting with the online solution of -3 m/s. Concerns are raised about potential errors in the equation or the application of momentum principles. Other participants suggest that the initial equation may be incorrect and provide alternative resources for clarification. The conversation highlights the importance of accurate equations in solving physics problems.
LSarah6
Messages
4
Reaction score
0

Homework Statement


A collision occurs between two football players. Player 1 has mass of 75 kg and a velocity of 6 m/s. Player 2 has mass of 150 kg and a velocity of -3 m/s (meaning going in an opposite direction). Assuming an ELASTIC collision, what is the final velocity of player 2?

Homework Equations


They gave us this equation in class to calculate the final velocity:
m = mass
Vi = initial velocity
Vf = final velocity
a = player 1
b = player 2

Vfb = [(2*ma)/(ma+mb)]*Via + [(mb-ma)/(ma+mb)]*Vib

The Attempt at a Solution



Using the equation above and plugging in the numbers:

Vfb =
[(2*75kg)/(75kg + 150kg)]*(6 m/s)
+
[(150kg - 75kg)/(75kg + 150kg)]*(-3 m/s)

which gives me:

Vfb = 4 m/s + -1 m/s = 3 m/s


The "online" homework solution says it is -3 m/s. Am I incorrect? Did I miss a negative sign somewhere, or is there a principle of momentum that I am not getting?
 
Physics news on Phys.org
Thread 'Confusion regarding a chemical kinetics problem'
TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
Back
Top