To calculate the pressure in 1.6 mol of the gas at 0°C using the Van der Waals equation, we need to use the formula (P + a(n/V)²)(V - nb) = nRT. Substitute the given values for n, V, T, a, and b into the equation and solve for P. Convert the temperature from Celsius to Kelvin and then plug in all the values to calculate the pressure.
To calculate the pressure in 1.6 mol of the gas at 0°C using the Van der Waals equation, we need to use the formula:
(P + a(n/V)²)(V - nb) = nRT
Where:
P is the pressure
a is the Van der Waals constant for the gas
n is the number of moles
V is the volume
b is another Van der Waals constant
R is the ideal gas constant
T is the temperature in Kelvin
In this case, the number of moles (n) is 1.6 mol, the volume (V) is 0.68 L, and the temperature (T) is 0°C. We also need to convert the temperature to Kelvin, which can be done by adding 273.15 to the Celsius temperature. Using the given Van der Waals constants for the gas, we can substitute these values into the equation and solve for the pressure (P).
Let's do the calculations:
First, convert the temperature to Kelvin: T = 0°C + 273.15 = 273.15 K
Next, substitute the values into the equation:
(P + a(1.6/0.68)²)(0.68 - 1.6b) = (1.6)(0.0821)(273.15)
Now, solve for P:
P = [(1.6)(0.0821)(273.15) - a(1.6/0.68)²(0.68 - 1.6b)] / (0.68 - 1.6b)
Plug in the given values for a and b, and calculate to find the pressure.