Busy. Please wait.
or

show password
Forgot Password?

Don't have an account?  Sign up 
or

Username is available taken
show password

why


Make sure to remember your password. If you forget it there is no way for StudyStack to send you a reset link. You would need to create a new account.
We do not share your email address with others. It is only used to allow you to reset your password. For details read our Privacy Policy and Terms of Service.


Already a StudyStack user? Log In

Reset Password
Enter the associated with your account, and we'll email you a link to reset your password.

Remove Ads
Don't know
Know
remaining cards
Save
0:01
To flip the current card, click it or press the Spacebar key.  To move the current card to one of the three colored boxes, click on the box.  You may also press the UP ARROW key to move the card to the "Know" box, the DOWN ARROW key to move the card to the "Don't know" box, or the RIGHT ARROW key to move the card to the Remaining box.  You may also click on the card displayed in any of the three boxes to bring that card back to the center.

Pass complete!

"Know" box contains:
Time elapsed:
Retries:
restart all cards




share
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.

  Normal Size     Small Size show me how

GCSE Equilibrium

AQA GCSE Chapter 08 (part 2) Equilibrium

QuestionAnswer
The forward reaction producing ammonia is exothermic. Explain what would happen to the YIELD of ammonia at equilibrium if the temperature was increased. use model answer « system will counteract change by » decreasing the temperature; « we know that » forward is exo « so equilibrium moves to » left-hand side/endothermic direction (1) and yield will decrease
Hydrogen reacts with nitrogen to produce ammonia. 3H2(g) + N2(g) <=> 2NH3(g) Give the meaning of <=> in the equation reversible reaction/reaction goes both ways
N2(g) + 3H2(g) <=> 2NH3(g). The pressure used in industry is 250 atmospheres. Explain how the use of a higher pressure would affect the equilibrium YIELD of ammonia. use model answer « system will counteract change by » decreasing the pressure; « we know that » there are less moles on right « so equilibrium moves to » right and yield will increase
The reaction between nitrogen and hydrogen to form ammonia is exothermic. The temperature used in industry is 450°C. Explain how the use of a lower temperature would affect the equilibrium YIELD of ammonia. use model answer « system will counteract change by » increasing the temperature; « we know that » forward is exo « so equilibrium moves to » right-hand side/exothermic direction (1) and yield will increase
N2(g) + 3H2(g) <=> 2NH3(g) Explain the effect on the RATE of attainment of equilibrium, when the process is carried out at a pressure higher than 200 atm increased pressure=more frequent collisions=higher rate (remember to answer the question: do not only say « faster reaction »)
N2(g) + 3H2(g) <=> 2NH3(g). The pressure used in industry is 250 atmospheres. Explain how the use of a LOWER pressure would affect the equilibrium YIELD of ammonia. use model answer « system will counteract change by » increasing the pressure; « we know that » there are less moles on right « so equilibrium moves to » left and yield will decrease
The forward reaction producing ammonia is exothermic. Explain what would happen to the YIELD of ammonia at equilibrium if the temperature was increased. use model answer « system will counteract change by » increasing the temperature; « we know that » forward is exo « so equilibrium moves to » right-hand side/exothermic direction (1) and yield will increase
Hydrogen reacts with nitrogen to produce ammonia. 3H2(g) + N2(g) <=> 2NH3(g). Explain what would happen to the YIELD of ammonia at equilibrium if the Ammonia NH3 was removed. use model answer « system will counteract change by » increasing the CONCENTRATION of NH3; « we know that » Ammonia is on the right hand side « so equilibrium moves to » right-hand side(1) and yield will increase (ensure you use the keyword CONCENTRATION)
What is the model answer for a question on equilibrium? 1) identify the change 2) "system tries to counteract the change by " doing the opposite 3) "we know that" EITHER where the chemical is OR more molecules=more pressure OR forward reaction is endo/exothermic 4)"so the equilibrium shifts" left/right
Created by: ursulinechem2