If 0.45 mol of neon gas occupies a volume of 789 mL at a certain temperature and pressure, what volume would 0.376 mols of neon occupy under the same conditions?
what Law is used to solve?
789 mL x 0.376/0.45 = ?
To solve this problem, we can use the Ideal Gas Law, which states that the pressure (P), volume (V), and number of moles (n) of a gas are related by the equation PV = nRT, where R is the ideal gas constant and T is the temperature in Kelvin.
First, we need to find the value of R. The ideal gas constant is generally given as 0.0821 L·atm/(mol·K). However, since the given pressure and volume are not in atmospheres and liters, we need to use the proper units for R.
In this case, we are given the volume in milliliters (mL). There are 1000 mL in one liter, so we convert the volume to liters by dividing by 1000:
789 mL ÷ 1000 = 0.789 L
Now that we have the volume in liters, we can find the value of R:
R = 0.0821 L·atm/(mol·K)
Next, let's calculate the initial pressure (P) using the given data:
n = 0.45 mol
V = 0.789 L
Rearranging the Ideal Gas Law equation, we have:
P = nRT / V
Substituting the values we know:
P = (0.45 mol)(0.0821 L·atm/(mol·K))(T) / 0.789 L
Now, let's calculate the volume (V) when there are 0.376 moles of neon:
n = 0.376 mol
P = (calculated using the previous steps)
Using the Ideal Gas Law equation, we can rearrange it to solve for V:
V = nRT / P
Substituting the values we know:
V = (0.376 mol)(0.0821 L·atm/(mol·K))(T) / P
Please note that in order to fully solve the problem and find the value of V, we need to know the temperature (T) and pressure (P) at which the gases are being held. Without these values provided in the question, we cannot determine the exact volume.