What is the volume of 3.11×10 to the power 23. Molecules of NH3 at S.T.P
To find the volume of a certain number of molecules of NH3 (Ammonia) at Standard Temperature and Pressure (STP), you need to use the ideal gas law equation. The ideal gas law equation is given as:
PV = nRT
Where:
P = pressure (in units of pressure, usually atm)
V = volume (in units of volume, usually liters)
n = number of moles
R = gas constant (0.0821 L·atm/(mol·K) - in this case, since we're using liters and atm for the units of pressure and volume)
T = temperature (in units of Kelvin)
At STP, the conditions are defined as 1 atm of pressure and 0°C (273.15 K) of temperature.
First, we need to convert the given number of molecules into moles. We can do this by using Avogadro's number, which states that 1 mole of any substance contains 6.022 × 10^23 particles. In this case, we have 3.11 × 10^23 molecules of NH3.
1 mole of NH3 = 6.022 × 10^23 molecules
So, the number of moles (n) of NH3 in this case is:
n = (3.11 × 10^23) / (6.022 × 10^23)
Now, we can substitute the values into the ideal gas law equation and solve for V (volume):
PV = nRT
(1 atm) · V = [(3.11 × 10^23) / (6.022 × 10^23)] · (0.0821 L·atm/(mol·K)) · (273.15 K)
Simplifying the equation:
V = [(3.11 × 10^23) / (6.022 × 10^23)] · (0.0821) · (273.15)
Now, plug in these values into a calculator and solve for V. The result will be the volume in liters.