Chemistry Calculate the pressure-volume work for the given reaction

AI Thread Summary
The discussion revolves around calculating pressure-volume work for a reaction involving water, noting that water is a liquid and not an ideal gas. Participants mention the ideal gas law (PV=nRT) but recognize its inapplicability to liquids. The focus shifts to the formula for work, emphasizing the need for initial and final volumes to proceed with calculations. There is a call for more specific information about the volumes involved in the reaction. The conversation highlights the necessity of knowing the volume of water produced and the reactants to solve the problem effectively.
anjauk2003
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New user has been reminded to always show their work on schoolwork problems.
Homework Statement
Assume that 2.00 moles of water are formed according to the following reaction at constant
pressure (101.3 kPa) and constant temperature (298 K):
I have to calculate the pressure-volume work for the given reaction and i really dont know how to start or what to use. Can someone help me?
Relevant Equations
2 H2(g) + O2(g) --> 2 H2O(l)
I dont have an solution Attempt. Maybe something with PV=nRT but this is for ideal gas and H2O is liquid. An other formula they introduced us to is: dE=-P*V
 
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anjauk2003 said:
dE=-P*V

If it is about work more like P*dV.

What is the initial volume of the mixture, and what is the final volume?
 
Borek said:
If it is about work more like P*dV.

What is the initial volume of the mixture, and what is the final volume?
That's the problem. I dont have more information. I wrote down everything i got.
 
You have everything you need. What is volume of water produced? What reacted?
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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