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..
To calculate the volume of the balloon using the ideal gas law, we need the values for temperature, pressure, and the gas constant.
1. Temperature conversion: You mentioned that the temperature is 52 degrees, and we need to convert it to Kelvin. To do this, we add 273 to the Celsius temperature to get the Kelvin temperature.
Celsius to Kelvin: 52 + 273 = 325 Kelvin
2. Pressure: You provided the pressure value of 1008, which should be in units of millibars. The ideal gas law requires pressure to be in units of Pascal (Pa), so we need to convert millibars to Pascal. Since 1 millibar is equal to 100 Pascal, we can convert the pressure as follows:
1008 millibars * 100 Pascal/millibar = 100,800 Pascal
Now that we have the temperature (325K) and pressure (100,800 Pa), we can calculate the volume using the ideal gas law:
Ideal Gas Law: PV = nRT
In this case, we are given the mass of carbon dioxide (22 grams), so we need to convert the mass (grams) to moles (mol). To do this, we use the molar mass of carbon dioxide, which is 44 grams/mol.
22 grams of CO2 * (1 mol CO2 / 44 grams CO2) = 0.5 moles CO2
Now, we can rearrange the ideal gas law equation using the given values:
PV = nRT
The gas constant (R) is 0.0821 L * atm / (mol * K).
V = (nRT) / P
V = (0.5 mol * 0.0821 L * atm / (mol * K) * 325 K) / 100,800 Pa
Simplifying:
V = (0.5 * 0.0821 * 325) / 100,800 L
V = 0.02004025 L
So, the volume of the balloon is approximately 0.020 L or 20 milliliters.