How is the ideal gas law related to the bursting of a pingpong ball when heated?

Ideal gas law is PV= nRt

Pressure

Volume

n= moles of substance ( in this case, oxygen gases in the ball, i assume)

R= constant

T= temperature

In your case, V and n stay constant as T and P are changing.

Assuming ideal gas law is valid, at some temperature (1) and pressure (1)

P1*V = n*R*T1

At some other temperature (2) and pressure (2)

P2*V = n*R*T2

Divide (1) by (2)

(P1*V) / (P2*V) = (n*R*T1) / (n*R*T2)

and you can see that V, n, and R cancel. This leaves you with:

P1/P2 = T1/T2 or P1/T1 = P2/T2

This way you can clearly see how the pressure changes with temperature (for constant n and V).

so, you start with the equation: PV=nRT

Looking at the equation, we need to look at what's staying the same and what's changing. As the ball is being heated, T will change on the right side of the equation, but n and R will remain the same, since you're not adding moles, and R is constant.

Now, we look at the other side. Since the expression nRT will get bigger, PV must get bigger, as well. As the volume does not change (since the pingpong ball is in a fixed shape) the pressure will increase. Eventually, the pressure will be so great that the material that the pingpong ball is made of will not be able to withstand the pressure, and the ball will explode. I hope I helped. Good luck!