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

Convert 4.0 g CO2 to moles. moles = grams/molar mass.

1 mole of a gas occupies 22.4 L at STP. So ?? moles will occupy ?? moles x (22.4L/mole) = xx

Strictly speaking the volume of the balloon will be the same (no increase) if the correct use of sublime is being used here. The term sublime or sublimation means going from the solid phase directly to the gas phase AND back again. So the dry ice is sill a solid at the end of the process.

The correct word that should have used in the question is evaporate or evaporation.

To determine the volume of the balloon at STP after all the dry ice sublimes, we need to follow these steps:

Step 1: Convert the mass of the dry ice to moles.
The molar mass of carbon dioxide (CO2) is approximately 44.01 g/mol.
Number of moles = mass / molar mass
Number of moles = 4.00 g / 44.01 g/mol = 0.0908 mol

Step 2: Use the ideal gas equation to find the volume at STP.
The ideal gas equation is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/(mol·K)), and T is the temperature in Kelvin.

At STP, the temperature is 273.15 K, and the pressure is 1 atm.

Rearranging the equation, we have:
V = (nRT) / P

V = (0.0908 mol * 0.0821 L·atm/(mol·K) * 273.15 K) / 1 atm
V ≈ 2.2 L

Therefore, the volume of the balloon at STP, after all the dry ice sublimes, will be approximately 2.2 liters.

To find the volume of the balloon at Standard Temperature and Pressure (STP) after all the dry ice sublimes, we need to understand the properties of dry ice and the conditions of STP.

Firstly, let's establish the conditions of STP:
- Standard Temperature is 0 degrees Celsius or 273.15 Kelvin (K).
- Standard Pressure is 1 atmosphere (atm) or 101.325 kilopascals (kPa).

Now, let's understand the properties of dry ice (solid CO2):
- Dry ice directly changes from a solid to a gas in a process called sublimation, without going through the liquid state.
- The molar mass of CO2 is 44.01 grams per mole (g/mol).

To determine the final volume of the balloon, we will need to use the Ideal Gas Law, which states that the product of the pressure (P), volume (V), and number of moles (n) of gas is equal to the product of the gas constant (R) and the temperature (T) in Kelvin.

The Ideal Gas Law formula is: PV = nRT

Since we don't have information about the pressure and temperature after the dry ice sublimes, we will use the conditions of STP for the calculation.

Now, let's calculate the number of moles (n) of CO2 gas released by the dry ice:
- Given the mass of dry ice is 4.00 grams (g).
- Calculate the number of moles using the formula: moles = mass / molar mass.

moles = 4.00 g / 44.01 g/mol ≈ 0.0909 mol (rounded to four decimal places)

Since one mole of any gas at STP occupies 22.4 liters (L), we can use this information to find the volume of CO2 gas released:
- Multiply the number of moles by the molar volume at STP (22.4 L/mol).
- V = n * 22.4 L/mol

V = 0.0909 mol * 22.4 L/mol ≈ 2.04 L (rounded to two decimal places)

Therefore, the volume of the balloon at STP after all the dry ice sublimes will be approximately 2.04 liters.