what volume of chlorine is required to produce 25.4grams of copper II chloride at 18 degrees celsius and 2.13 atm
Produce 25.4 g CuCl2 from what? Cu? amd Cl2?
Cu + Cl2 == CuCl2
mols CuCl2 = 25.4 g/molar
mols Cl2 = same as mols Cu.
Then use PV = nRT, substitute mole Cl2 for n, substitute P and T (remember T must be in kelvin) and solve for V in Liters.
To determine the volume of chlorine gas (Cl2) required to produce 25.4 grams of copper(II) chloride (CuCl2), we can use the balanced chemical equation for the reaction between chlorine and copper:
2Cu + Cl2 -> 2CuCl2
From the balanced equation, we can see that 1 mole of chlorine gas reacts with 2 moles of copper to produce 2 moles of copper(II) chloride.
1. Calculate the number of moles of copper(II) chloride:
Using the molar mass of CuCl2, which is approximately 134.45 g/mol:
moles of CuCl2 = mass / molar mass
= 25.4 g / 134.45 g/mol
≈ 0.189 moles
2. Determine the moles of chlorine gas needed:
Since the molar ratio between chlorine gas and copper(II) chloride is 1:2:
moles of Cl2 = 2 * moles of CuCl2
= 2 * 0.189 moles
≈ 0.378 moles
3. Apply the ideal gas equation to find the volume of chlorine gas:
PV = nRT
P = pressure = 2.13 atm
V = volume (unknown)
n = moles of Cl2 = 0.378 moles
R = ideal gas constant = 0.0821 L·atm/(mol·K)
T = temperature = 18 °C = 18 + 273 = 291 K
Rearrange the equation and solve for V:
V = (nRT) / P
= (0.378 moles * 0.0821 L·atm/(mol·K) * 291 K) / 2.13 atm
≈ 4.15 L
Therefore, approximately 4.15 liters of chlorine gas is required to produce 25.4 grams of copper(II) chloride at 18 degrees Celsius and 2.13 atm.
To determine the volume of chlorine gas required to produce copper II chloride, we need to apply the ideal gas law equation: PV = nRT.
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
First, we need to calculate the number of moles of copper II chloride. To do this, we'll use the molar mass of copper II chloride (CuCl₂), which is approximately 134.45 g/mol.
Number of moles = mass / molar mass
Number of moles = 25.4 g / 134.45 g/mol
Number of moles ≈ 0.189 mol
Next, we'll use the balanced chemical equation to determine the stoichiometric relationship between chlorine gas and copper II chloride. The balanced equation for the reaction is:
Cu + Cl₂ → CuCl₂
From the equation, we can see that one mole of copper II chloride requires one mole of chlorine gas.
Since the stoichiometry is 1:1, the number of moles of chlorine gas required is also 0.189 mol.
Now, let's use the ideal gas law equation to find the volume.
PV = nRT
Given:
Pressure (P) = 2.13 atm
Temperature (T) = 18°C = 18 + 273.15 = 291.15 K (temperature converted to Kelvin)
Number of moles (n) = 0.189 mol
Ideal gas constant (R) = 0.0821 L·atm/(mol·K) (using the units suitable for atm and L)
V = (nRT) / P
V = (0.189 mol * 0.0821 L·atm/(mol·K) * 291.15 K) / 2.13 atm
Calculating the above expression will give us the volume (V) in liters.
V ≈ 2.06 L
Therefore, approximately 2.06 liters of chlorine gas are required to produce 25.4 grams of copper II chloride at 18 °C and 2.13 atm of pressure.