DrBob222
answered
P = ?
V = 0.500 L
n = 0.568
T = 298 K
R = 0.08206
Post your work if you run into trouble
Step-by-Step Bot
answered
PV = nRT
Where:
P = Pressure (in atm)
V = Volume (in liters)
n = moles of the gas
R = Ideal gas constant (0.0821 L.atm/mol.K)
T = Temperature (in Kelvin)
First, let's convert the given temperature from Celsius to Kelvin:
T (Kelvin) = T (Celsius) + 273.15
T = 25°C + 273.15 = 298.15 K
Next, convert the volume from mL to liters:
V (liters) = V (mL) / 1000
V = 500.0 mL / 1000 = 0.5 L
Now, we have all the values we need to calculate the pressure:
P * 0.5 L = 0.568 mol * 0.0821 L.atm/mol.K * 298.15 K
Solving for P:
P = (0.568 mol * 0.0821 L.atm/mol.K * 298.15 K) / 0.5 L
P = 8.31 atm
Therefore, the pressure exerted by 0.568 moles of CO2 at a temperature of 25°C and a volume of 500.0 mL is approximately 8.31 atm.
Explain Bot
answered
PV = nRT
Where:
P = pressure (in units of 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 convert the given volume from mL to L:
500.0 mL = 500.0 / 1000 = 0.5 L
Next, we need to convert the given temperature from degrees Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 25 + 273.15 = 298.15 K
Now we can substitute the values into the ideal gas law equation:
PV = nRT
P * 0.5 = 0.568 * 0.0821 * 298.15
Simplifying the equation further:
0.5P = 14.107
To find the pressure (P), we can solve for it:
P = 14.107 / 0.5
P = 28.214
Therefore, the pressure exerted by 0.568 moles of CO2 at a temperature of 25°C and a volume of 500.0 mL is approximately 28.214 atm.
