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20 g chunk of dry ice is placed in an empty 0.75 litre wine bottle tightly closed. What would be the final pressure (in atm) in the bottle after all CO2 has been evaporated and temperature reaches to 25°C?(rounded up to first decimal place)
Correct answer is between '14.0,15.0'. Can you explain this answer?
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Most Upvoted Answer
20 g chunk of dry ice is placed in an empty 0.75 litre wine bottle tig...
To solve this problem, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
First, we need to determine the number of moles of CO2 in the 20 g of dry ice. The molar mass of CO2 is 44.01 g/mol, so:
n = mass / molar mass
n = 20 g / 44.01 g/mol
n = 0.454 mol
Next, we need to convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 25 + 273.15
T(K) = 298.15 K
Now we can substitute the values into the ideal gas law equation:
PV = nRT
P * 0.75 L = 0.454 mol * 0.0821 L·atm/(mol·K) * 298.15 K
P * 0.75 L = 11.897 atm·L
P = 11.897 atm·L / 0.75 L
P ≈ 15.86 atm
Therefore, the final pressure in the bottle after all CO2 has evaporated and the temperature reaches 25 °C would be approximately 15.86 atm.
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
First, we need to determine the number of moles of CO2 in the 20 g of dry ice. The molar mass of CO2 is 44.01 g/mol, so:
n = mass / molar mass
n = 20 g / 44.01 g/mol
n = 0.454 mol
Next, we need to convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 25 + 273.15
T(K) = 298.15 K
Now we can substitute the values into the ideal gas law equation:
PV = nRT
P * 0.75 L = 0.454 mol * 0.0821 L·atm/(mol·K) * 298.15 K
P * 0.75 L = 11.897 atm·L
P = 11.897 atm·L / 0.75 L
P ≈ 15.86 atm
Therefore, the final pressure in the bottle after all CO2 has evaporated and the temperature reaches 25 °C would be approximately 15.86 atm.
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Community Answer
20 g chunk of dry ice is placed in an empty 0.75 litre wine bottle tig...
Given
w = 20g dry CO2 which will evaporate to develop P
m = 44
V = 0.75 litre
P = ?
T = 298 K
PV = wmRT
P�0.75=2044�0.0821�298
⇒ P = 14.828 atm
Pressure inside bottle = P + atm. pressure
⇒ 14.828 + 1 = 15.828 atm
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20 g chunk of dry ice is placed in an empty 0.75 litre wine bottle tightly closed. What would be the final pressure (in atm) in the bottle after all CO2 has been evaporated and temperature reaches to 25°C?(rounded up to first decimal place)Correct answer is between '14.0,15.0'. Can you explain this answer?
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