A mole of reacts at a constant pressure of 43.0atm via the reaction
Before the reaction, the volume of the gaseous mixture was 5.00L . After the reaction, the volume was 2.00L . Calculate the value of the total energy change, , in kilojoules.
You didn't provide a reaction.
To calculate the value of the total energy change (∆E) in kilojoules, we can use the equation:
∆E = -P∆V
where ∆V is the change in volume and P is the pressure.
Given:
Initial volume (Vi) = 5.00 L
Final volume (Vf) = 2.00 L
Pressure (P) = 43.0 atm
First, we need to calculate the change in volume (∆V):
∆V = Vf - Vi
∆V = 2.00 L - 5.00 L
∆V = -3.00 L
Negative sign indicates a decrease in volume.
Next, we substitute the values of ∆V and P in the equation ∆E = -P∆V:
∆E = -P∆V
∆E = -(43.0 atm) * (-3.00 L)
Multiply the values:
∆E = 129.0 atm·L
Finally, we convert the units from atm·L to kilojoules. We can use the conversion factor:
1 atm·L = 101.3 J
So, to convert to kilojoules:
∆E = (129.0 atm·L) * (101.3 J / 1000) = 13.05 kJ (rounded to two decimal places)
Therefore, the value of the total energy change (∆E) is approximately 13.05 kilojoules.