A student adds 5.50 g of dry ice (solid ) to an empty balloon. What will be the volume of the balloon at STP after all the dry ice sublimes (converts to gaseous )?
PV=nRT P=1atm, T=273
n=5.5/molemassCO2=5.5/44 check that.
solve for V
To find the volume of the balloon at STP (Standard Temperature and Pressure) after all the dry ice sublimes, we need to follow these steps:
1. Convert the mass of dry ice from grams to moles.
2. Use the ideal gas law equation to calculate the volume of the balloon.
Step 1: Convert mass to moles
The molar mass of carbon dioxide (CO2) is 44.01 g/mol. We can use this to convert the mass of dry ice to moles:
moles = mass / molar mass
moles = 5.50 g / 44.01 g/mol
Step 2: Calculate the volume
The ideal gas law equation is given as:
PV = nRT
Where:
P = pressure (at STP - 1 atm)
V = volume
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (at STP - 273.15 K)
Since we are looking for the volume, we can rearrange the equation to solve for V:
V = nRT / P
Substituting the known values:
n = moles (from Step 1)
R = 0.0821 L·atm/(mol·K)
T = 273.15 K (STP)
P = 1 atm
V = (moles)(R)(T) / P
Calculating the volume using the formula above will give us the final answer.