A 12.0L sample of a as at a constant pressure of 608 mm Hg was heated from 40 degrees celsius to 60 degrees celsius. What volume does the gas now occupy?

would I multiply 608 by 12 and then divide by the degrees celsius?

I wonuldn't do that.

Charles law:

V1/V2= T1/T2 temps in kelvins

So would I set it up as 12.0L / v2 = 313 K / 333K ?

I got 11.3 L as my answer. Is this correct?

The set up looks ok to me but if T goes up doesn't V go up? Your calculation is lower?

I tried again and got 12.8

I'll buy that.

Well the answer choices were 18L, 8.0L, 12.8L, 15L and 11.3L and when i divided 12 by 0.9399 which I got from 313/333 I got 12.76.

And I got 12.76 also BUT you have three significant figures in 12.0, 313 and 333 so you may have 3 in the answer (not 4); therefore, round 12.76 to 12.8.

ok thank you

To determine the new volume of the gas when it is heated, you would need to use the ideal gas law equation:

PV = nRT

Where:
P = pressure (in this case, 608 mm Hg)
V = volume (initially 12.0L, what we are trying to find)
n = number of moles (unknown in this case)
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature in Kelvin (initially 40 degrees Celsius, final temperature 60 degrees Celsius)

To solve for the new volume, we need to first convert the temperatures from Celsius to Kelvin. This conversion can be done by adding 273.15 to the Celsius temperature.

So, the initial temperature would be (40 + 273.15) = 313.15K, and the final temperature would be (60 + 273.15) = 333.15K.

Now let's rearrange the ideal gas law equation to solve for the final volume:

V = (nRT) / P

To use this equation, we need to first calculate the number of moles (n) using the known data. To do this, we need the initial and final temperatures in Kelvin, the initial volume (12.0L), and the pressure (608 mm Hg).

We can use the equation n = (P * V) / (R * T) to find the number of moles.

Substituting the known values:
n = (608 mm Hg * 12.0L) / (0.0821 L·atm/mol·K * 313.15K)

n ≈ 28.59 moles

Now, we can substitute all the known values into the rearranged equation to find the final volume:

V = (28.59 moles * 0.0821 L·atm/mol·K * 333.15K) / 608 mm Hg

Calculating this, we get:
V ≈ 44.10 L

Therefore, the gas now occupies approximately 44.10 liters after being heated from 40 degrees Celsius to 60 degrees Celsius at a constant pressure of 608 mm Hg.