Problem: A student adds 4.00 g of dry ice (solid CO2) to an empty balloon. What will be the volume of the balloon at STP after all the dry ice sublimes (converts to gaseous CO2)?

🤓 Based on our data, we think this question is relevant for Professor Bojan's class at PSU.

FREE Expert Solution

The volume of the balloon is simply the volume occupied by CO2. We can use the ideal gas law to calculate the volume CO2 occupies. The ideal gas law is as follows:

At conditions of standard temperature and pressure (STP), temperature = 273.15 K and pressure = 1 atm.

We first need to determine the number of moles of CO2. The molar mass of CO2 is 12.01 g/mol C + 2(16.00 g/mol O) = 44.01 g/mol.

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Problem Details

A student adds 4.00 g of dry ice (solid CO2) to an empty balloon. What will be the volume of the balloon at STP after all the dry ice sublimes (converts to gaseous CO2)?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Standard Temperature and Pressure concept. You can view video lessons to learn Standard Temperature and Pressure. Or if you need more Standard Temperature and Pressure practice, you can also practice Standard Temperature and Pressure practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Bojan's class at PSU.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.