8.49

Volume: $\Delta S = nR\ln \frac{V_{2}}{V_{1}}$
Temperature: $\Delta S = nC\ln \frac{T_{2}}{T_{1}}$

Posts: 50
Joined: Fri Sep 29, 2017 7:05 am

8.49

Oxygen Difluoride is colorless, very poisonous gas that reacts rapidly with water vapor to produce 02, HF, and heat:
$OF_{2}(g) + H_{2}0\rightarrow O_{2}(g) + 2HF(g) \bigtriangleup H = -1368kJ$

What is the change in internal energy for the reaction of 1.00 mol OF2?

Merzia Subhan 1L
Posts: 33
Joined: Thu Jul 13, 2017 3:00 am

Re: 8.49

You would use the formula delta U = q + w. q =deltaH. w = delta n*R*T. We assume it is at room temperature so you use 298K for T. n is 1 bc 3 moles of gas are produced and 2 moles of gas were there initially. The enthalpy is in kJ so don't forget to convert it into Joules when adding to the w bc the R is given in Joules

Posts: 50
Joined: Fri Sep 29, 2017 7:05 am

Re: 8.49

Thank You!

Return to “Entropy Changes Due to Changes in Volume and Temperature”

Who is online

Users browsing this forum: No registered users and 1 guest