A piece of dry ice (solid carbon dioxide) with a mass of 25.5 g is allowed to sublime (convert from solid to gas) into a large balloon.

Assuming that all of the carbon dioxide ends up in the balloon, what will be the volume of the balloon at a temperature of 18 degrees Celsius and a pressure of 745mmHg?

See your other post above.

To calculate the volume of the balloon, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure in atm (convert mmHg to atm by dividing by 760: 745 mmHg / 760 = 0.979 atm)
V = volume in liters (what we want to find)
n = number of moles of gas (convert mass of dry ice to moles using molar mass of CO2: 25.5 g / 44.01 g/mol = 0.579 mol)
R = ideal gas constant (0.0821 L•atm/mol•K)
T = temperature in Kelvin (convert Celsius to Kelvin: 18 degrees Celsius + 273.15 = 291.15 K)

Now, we can rearrange the equation to solve for V:

V = (nRT) / P

Substituting the known values:

V = (0.579 mol * 0.0821 L•atm/mol•K * 291.15 K) / 0.979 atm

Calculating:

V = 0.377 L

Therefore, the volume of the balloon will be approximately 0.377 liters.

To find the volume of the balloon when the dry ice sublimes, we first need to calculate the number of moles of carbon dioxide (CO2) in the 25.5 g of dry ice.

To do this, we can use the molar mass of carbon dioxide, which is 44.01 g/mol.

The number of moles (n) can be calculated using the formula:

n = mass / molar mass

n = 25.5 g / 44.01 g/mol

n ≈ 0.58 mol

Since the sublimation of dry ice is an endothermic process, it absorbs heat from the surroundings. However, for simplicity, we will assume that the heat absorbed is negligible and the temperature and pressure remain constant during the sublimation.

Now, we can use the ideal gas law to find the volume of the gas:

PV = nRT

Where:
P = pressure (745 mmHg)
V = volume (unknown)
n = number of moles of gas (0.58 mol)
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (18 °C + 273.15 = 291.15 K)

Plugging in the values and solving for V, we have:

V = (nRT) / P

V = (0.58 mol * 0.0821 L·atm/(mol·K) * 291.15 K) / 745 mmHg

V ≈ 0.143 L (rounded to three decimal places)

Therefore, the volume of the balloon, assuming all the CO2 ends up in it, would be approximately 0.143 liters at the given temperature and pressure.

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