Math  /  Word Problems

QuestionWhat happens when a 5.0 L5.0 \mathrm{~L} container is expanded to 10.0 L10.0 \mathrm{~L} for this reaction?
51.8 kJ+H2( g)+I2( g)2HI(g) 51.8 \mathrm{~kJ}+\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HI}(\mathrm{g})
A. Shift to the right for fewer moles. B. No change in moles. C. Shift to the left for more moles.

Studdy Solution
When the pressure decreases, the system will shift in the direction that produces more moles of gas to increase the pressure and restore equilibrium.In this reaction, the number of moles of gas is the same on both sides (2 moles). Therefore, the system will not shift to either side because the pressure change does not favor the production of more or fewer moles of gas.
The correct answer is B. There is no change because there are the same number of moles of gas on both sides.

View Full Solution - Free
Was this helpful?

Studdy solves anything!

banner

Start learning now

Download Studdy AI Tutor now. Learn with ease and get all help you need to be successful at school.

ParentsInfluencer programContactPolicyTerms
TwitterInstagramFacebookTikTokDiscord