Assuming that all of the carbon dioxide ends up in the balloon, what will be the volume of the balloon at a temperature of 20 ∘C and a pressure of 734 mmHg ?
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If you know grams CO2 or mols CO2, use PV = nRT and solve for V.
To determine the volume of the balloon at a temperature of 20 ∘C and a pressure of 734 mmHg, we can use the ideal gas law equation, which is given by:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles of gas
R = ideal gas constant
T = temperature
In this case, we are assuming that all of the carbon dioxide ends up in the balloon, so we need to find the number of moles of gas and plug in the known values for pressure, temperature, and the gas constant.
Step 1: Convert the pressure from mmHg to atm
1 atm = 760 mmHg
So, P (in atm) = 734 mmHg / 760 mmHg = 0.9658 atm
Step 2: Convert the temperature from Celsius to Kelvin
To convert from Celsius to Kelvin, we need to add 273.15 to the Celsius value.
T (in Kelvin) = 20 ∘C + 273.15 = 293.15 K
Step 3: Plug in the values into the ideal gas law equation
PV = nRT
V = (nRT) / P
Now we need to calculate the number of moles of gas. To do this, we can use the molar mass of carbon dioxide (CO2).
The molar mass of CO2 is 44.01 g/mol.
Assuming you have the mass of the carbon dioxide, you can divide it by the molar mass to get the number of moles.
Once you have the number of moles, you can substitute it into the equation along with the values for pressure, temperature, and the gas constant to calculate the volume of the balloon.