Given: C2H2(g) +2HF(g) -> C2H4F2(g)
Find: pressure in a 10.0L flask when the reaction is complete
When 1.0 mol of C2H2 and 5.0 mol pf HF are reacted in a 10.0 L flask, what will be the pressure in the flask at 0 degrees C when the reaction is complete?
See your post on CO and O2.
To find the pressure in the flask when the reaction is complete, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
First, let's determine the number of moles of each gas present in the reaction.
Given:
- C2H2 (acetylene) reacts with 2 HF (hydrogen fluoride) to form C2H4F2 (tetrafluoroethylene)
From the balanced chemical equation, we can see that 1 mole of C2H2 reacts with 2 moles of HF.
Given:
- 1.0 mol of C2H2
- 5.0 mol of HF
Since the reaction is in a 10.0 L flask, we can assume the volume remains constant throughout the reaction.
Now, let's calculate the total number of moles of gas in the flask by adding the moles of C2H2 and HF:
1.0 mol + 5.0 mol = 6.0 mol
Next, we substitute the values into the ideal gas law equation and solve for P:
PV = nRT
P * 10.0 L = 6.0 mol * (0.0821 L·atm/mol·K) * (273.15 K)
Simplifying the equation:
P = (6.0 mol * 0.0821 L·atm/mol·K * 273.15 K) / 10.0 L
Calculating:
P = 13.2228 atm
Therefore, the pressure in the 10.0 L flask when the reaction is complete is approximately 13.2 atm.