chemistry
posted by amy .
Your balloon contains 22 grams of Carbon dioxide. Use the following link to determine the temperature in your area. and then use the following to convert to Kelvin. Record below. Given the Gas Constant R please use the ideal gas law to calculate the volume in liters of the balloon. Show all work for partial credit.
Here's what I have
temp= 52=>284 Kelvin
1008 pressure
I am lost......

1008 millibars

How do you come up with 284 for T.
K = C + 273 = ? or is that 52 F?
At my previous response of your earlier post you have P = 101.9. Where did that come from? 
52 F = 284 K.
1008 (hPa) = 101.9(kPa)
Is that right? I'm checking my book and its soooo confusing to me.
I have this info so far and want to know if I'm doing it right since its worth 12 points on my test!!!
.5*8.314*284/101.9=11.58L 
1008 hPa is not 101.9 kPa. Go to google window and type in "1008 hPa to kPa" without the quotation marks. I'm interested in the kind of test this is and the instructions. Open book? Is outside help allowed?

I am homeschooled...open book yes..here is the question..
Given a balloon you have at home, use this website to determine the barometric pressure by going to the following website in millibars..........removed website link....... in your area. Record the pressure below. Your balloon contains 22 grams of Carbon dioxide. Use the following link to determine the temperature in your area. and then use the following to convert to Kelvin. Record below. Given the Gas Constant R please use the ideal gas law to calculate the volume in liters of the balloon. Show all work for partial credit.
Am I doing this right? 
.5*8.314*284/100.8=11.71L

That looks right to me.

Thank you very much..