20 g of CO2 is placed in 0.75l Bottle and sealed. what is the pressure in the bottle if the temp is 25C?
Convert 20 g CO2 to moles. moles = grams/molar mass
Then use PV = nRT and solve for P.
To calculate the pressure in the bottle, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in Pascals or atmospheres)
V = volume (in liters)
n = number of moles of gas
R = ideal gas constant (0.0821 L·atm/(mol·K) - when using atm as the unit for pressure)
T = temperature (in Kelvin)
First, we need to convert the given temperature from Celsius to Kelvin by adding 273.15:
T = 25°C + 273.15 = 298.15 K
Next, we need to calculate the number of moles of gas using the molecular weight of carbon dioxide (CO2), which is approximately 44.01 g/mol. The molar mass of CO2 is the sum of the atomic masses of carbon (C) and two oxygen (O) atoms:
n = mass of CO2 / molar mass of CO2
n = 20 g / 44.01 g/mol ≈ 0.454 mol
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
Solving for P:
P = (0.454 mol * 0.0821 L·atm/(mol·K) * 298.15 K) / 0.75 L
P ≈ 9.27 atm
Therefore, the pressure in the bottle is approximately 9.27 atmospheres.