A sample of chlorine gas at a pressure of 420 mm Hg and in a volume of 3.50L was heated from 18.0 degrees celsius to 45 degrees celsius after being transferred to a container of volume 2.35L. The pressure in this new container should be about?

Would I use (p1)(v1) = (p2)(v2)

420 * 3.50 = 2.35* v2

The problem is confusing. What is the original T when P is 420 mm Hg and in the 3.50L container? If it is 18 C, then use

(P1V1/T1) = (P2V2/T2). If it isn't 18 C, then I don't know what the problem is asking.

Yes the original T is 18 degrees celsius so would it be

420*3.50 / 291 K = p2 * 2.35 / 318

5.05 = p2 * 2.35 / 318.

I am just not sure how to solve for the right side of the equation to find p2.

Yes, you are correct. To solve this problem, you can use the formula known as Boyle's Law, which states that the product of pressure and volume is constant at constant temperature.

To apply Boyle's Law, you can equate the initial pressure and volume (p1)(v1) to the final pressure and volume (p2)(v2):

(p1)(v1) = (p2)(v2)

In this case, the initial pressure (p1) is 420 mm Hg, the initial volume (v1) is 3.50 L, and the final volume (v2) is 2.35 L. You need to find the final pressure (p2).

Plugging in the given values, the equation becomes:

(420 mm Hg)(3.50 L) = (p2)(2.35 L)

Now, you can solve for p2 by rearranging the equation and dividing both sides by 2.35 L:

p2 = (420 mm Hg)(3.50 L) / (2.35 L)

p2 = 623.40 mm Hg

Therefore, the pressure in the new container should be approximately 623.40 mm Hg.