If each balloon is filled with carbon dioxide gas at 20 degrees C and 1 atmosphere, calculate the mass and the number of moles of carbon dioxide in each balloon at maximum inflation. Use the ideal gas law in your calculation. Someone please let me know the answer! Thank you so much!!

Please post ALL of problem.

That is all the problem sir.

The volume of maximum inflation is 55cm. That's part of the problem but I'm still having trouble finding the answer.

To calculate the mass and number of moles of carbon dioxide in each balloon at maximum inflation, we can use the ideal gas law, which is given by the equation:

PV = nRT

Where:
P = pressure (in our case, 1 atmosphere)
V = volume (at maximum inflation, which we do not know yet)
n = number of moles of carbon dioxide
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin, which is 20°C + 273.15)

First, let's convert the temperature from Celsius to Kelvin:
T = 20°C + 273.15 = 293.15 K

Now, we can rearrange the ideal gas law equation to isolate 'n' (number of moles of carbon dioxide):

n = PV / RT

Since the volume (V) is not given, we need to find it for each balloon.

To calculate the volume, we need an additional parameter, such as the balloon's diameter or radius. Assuming the balloon is spherical, we can use the formula for the volume of a sphere:

V = (4/3) * π * r^3

Where 'r' is the radius.

Without the specific diameter or radius of the balloon, it is not possible to calculate the volume and therefore the mass and number of moles of carbon dioxide in each balloon at maximum inflation. Please provide additional information for further assistance.