HomeworkLib
Question

A student ran the following reaction in the laboratory at 1185 K: 2SO2(g) + O2(g) 2SO3(g)...

A student ran the following reaction in the laboratory at 1185 K:

2SO2(g) + O2(g) 2SO3(g)

When she introduced 8.07×10-2 moles of SO2(g) and 7.94×10-2 moles of O2(g) into a 1.00 liter container, she found the equilibrium concentration of O2(g) to be 5.86×10-2 M.

Calculate the equilibrium constant, Kc, she obtained for this reaction.

Kc=?

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

0 0
Add a comment
Know the answer?
Add Answer to:
A student ran the following reaction in the laboratory at 1185 K: 2SO2(g) + O2(g) 2SO3(g)...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • A student ran the following reaction in the laboratory at 1078 K: 2SO3(g)-> 2SO2(g) + O2(g)...

    A student ran the following reaction in the laboratory at 1078 K: 2SO3(g)-> 2SO2(g) + O2(g) When she introduced 7.35×10-2 moles of SO3(g) into a 1.00 liter container, she found the equilibrium concentration of O2(g) to be 1.53×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

  • 1. A student ran the following reaction in the laboratory at 632 K: 2HI(g) ->H2(g) +...

    1. A student ran the following reaction in the laboratory at 632 K: 2HI(g) ->H2(g) + I2(g)   When she introduced 0.362 moles of HI(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 3.55×10-2 M.   Calculate the equilibrium constant, Kc, she obtained for this reaction.   Kc = 2. A student ran the following reaction in the laboratory at 616 K: CO(g) + Cl2(g) -> COCl2(g) When she introduced 0.131 moles of CO(g) and 0.161 moles...

  • 1) A student ran the following reaction in the laboratory at 306 K: CH4(g) + CCl4(g)...

    1) A student ran the following reaction in the laboratory at 306 K: CH4(g) + CCl4(g) 2CH2Cl2(g) When she introduced 3.94×10-2 moles of CH4(g) and 5.52×10-2 moles of CCl4(g) into a 1.00 liter container, she found the equilibrium concentration of CH2Cl2(g) to be 8.23×10-3 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc= 2) A student ran the following reaction in the laboratory at 333 K: CH4(g) + CCl4(g) 2CH2Cl2(g) When she introduced 3.94×10-2 moles of CH4(g)...

  • A student ran the following reaction in the laboratory at 283 K: 2CH2Cl2(g) -> CH4(g) +...

    A student ran the following reaction in the laboratory at 283 K: 2CH2Cl2(g) -> CH4(g) + CCl4(g) When she introduced 7.85×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CH2Cl2(g) to be 5.26×10-3 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

  • A student ran the following reaction in the laboratory at 230 K: 2NOBr(g) 2NO(g) + Br2(g)...

    A student ran the following reaction in the laboratory at 230 K: 2NOBr(g) 2NO(g) + Br2(g) When she introduced 0.173 moles of NOBr(g) into a 1.00 liter container, she found the equilibrium concentration of Br2(g) to be 1.80×10^-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

  • A student ran the following reaction in the laboratory at 293 K: 2CH2Cl2(g) CH4(g) + CCl4(g)...

    A student ran the following reaction in the laboratory at 293 K: 2CH2Cl2(g) CH4(g) + CCl4(g) When she introduced 6.91×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(g) to be 3.19×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc=?

  • A student ran the following reaction in the laboratory at 283 K: 2CH2Cl2(g) ->CH4(g) + CCl4(g)  ...

    A student ran the following reaction in the laboratory at 283 K: 2CH2Cl2(g) ->CH4(g) + CCl4(g)   When she introduced 7.70×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(g) to be 3.59×10-2 M.   Calculate the equilibrium constant, Kc, she obtained for this reaction.   Kc =

  • A student ran the following reaction in the laboratory at 425 K: PCl5(g) --> PCl3(g) +...

    A student ran the following reaction in the laboratory at 425 K: PCl5(g) --> PCl3(g) + Cl2(g) When she introduced 4.59 moles of PCl5(g) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 3.94×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.

  • A student ran the following reaction in the laboratory at 294 K: 2CH2Cl2(g) ____> CH4(g) +...

    A student ran the following reaction in the laboratory at 294 K: 2CH2Cl2(g) ____> CH4(g) + CCl4(g) When she introduced 7.04×10-2 moles of CH2Cl2(g) into a 1.00 Liter container, she found the equilibrium concentration of CCl4(g) to be 3.25×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.

  • A student ran the following reaction in the laboratory at 380 K: CH4(g) + CCl4(g) 2CH2Cl2(g)...

    A student ran the following reaction in the laboratory at 380 K: CH4(g) + CCl4(g) 2CH2Cl2(g) When she introduced 4.26×10-2 moles of CH4(g) and 5.94×10-2 moles of CCl4(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(g) to be 5.11×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT