A student adds 3.50 g of dry ice (solidCO2 ) to an empty balloon. What will be the volume of the balloon at STP after all the dry ice sublimes (converts to gaseousCO2 )?
mol of CO2 is 12+32 = 44 grams
so we have
3.5/44 = .08 mol of CO2
at stp 22.4 liters/mol
.08*22.4 = 1.78 liters
To find the volume of the balloon at STP after all the dry ice sublimes, we need to use the ideal gas law. The ideal gas law can be represented as:
PV = nRT
where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
At STP (Standard Temperature and Pressure), the temperature is 273.15 K (0 °C) and the pressure is 1 atm. We also need to calculate the number of moles of CO2 in 3.50 g of dry ice.
To find the number of moles, we use the formula:
moles = mass / molar mass
The molar mass of CO2 is approximately 44.01 g/mol.
moles = 3.50 g / 44.01 g/mol
moles ≈ 0.08 mol
Now we can substitute these values into the ideal gas law equation to solve for the volume:
(1 atm) * V = (0.08 mol) * (0.0821 L·atm/(mol·K)) * (273.15 K)
Simplifying the equation:
V = (0.08 mol) * (0.0821 L·atm/(mol·K)) * (273.15 K) / (1 atm)
V ≈ 1.8 L
Therefore, the volume of the balloon at STP after all the dry ice sublimes will be approximately 1.8 liters.