Question

Suppose a 500. mL flask is filled with 1.4 mole of CO , 0.60 mole of...

Suppose a 500. mL flask is filled with 1.4 mole of CO , 0.60 mole of H20 and 1.8 mol of CO2 the following reaction becomes possible CO (g) + H2O (g) = CO2 (g) + H2 (g) the equilibrium constant K for this reaction 4.89 at the temperature of the flask calculate the equilibrium Molarity of H2 round to two DECIMAL places final answer in Molarity

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
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
Similar Questions
Suppose a 500.mL flask is filled with 0.30mol of I2 and 0.60mol of HI . The...
Suppose a 500.mL flask is filled with 0.30mol of I2 and 0.60mol of HI . The following reaction becomes possible: +H2gI2g 2HIg The equilibrium constant K for this reaction is 0.247 at the temperature of the flask. Calculate the equilibrium molarity of H2 . Round your answer to one decimal place.
Suppose a 500.mL flask is filled with 1.0mol of O2 and 1.8mol of NO . The...
Suppose a 500.mL flask is filled with 1.0mol of O2 and 1.8mol of NO . The following reaction becomes possible: N2g+O2g =2NOg The equilibrium constant K for this reaction is 0.461 at the temperature of the flask. Calculate the equilibrium molarity of N2 . Round your answer to two decimal places. Final answer in molarity M 2 decimal places
Suppose a 250.mL flask is filled with 1.3mol of H2 and 0.30mol of I2 . The...
Suppose a 250.mL flask is filled with 1.3mol of H2 and 0.30mol of I2 . The following reaction becomes possible: H2(g) + I2(g) <--> 2HI(g) The equilibrium constant K for this reaction is 3.99 at the temperature of the flask. Calculate the equilibrium molarity of H2 . Round your answer to two decimal places.
Suppose a 500.mL flask is filled with 1.9mol of Br2 , 0.90mol of OCl2 and 2.0mol...
Suppose a 500.mL flask is filled with 1.9mol of Br2 , 0.90mol of OCl2 and 2.0mol of BrOCl . The following reaction becomes possible: Br2 (g)+OCl2 (g) +BrOCl (g)=BrCl (g) The equilibrium constant K for this reaction is 0.307 at the temperature of the flask. Calculate the equilibrium molarity of BrOCl . Round your answer to two decimal places. final answer in M 2 decimal places
Suppose a 250.mL flask is filled with 0.60mol of I2 and 1.4mol of HI . The...
Suppose a 250.mL flask is filled with 0.60mol of I2 and 1.4mol of HI . The following reaction becomes possible: H2(g) + I2 (g) -> 2HIg The equilibrium constant K for this reaction is 0.644 at the temperature of the flask. Calculate the equilibrium molarity of HI . Round your answer to one decimal place.
Suppose a 250.mL flask is filled with 1.6mol of O2 and 1.2mol of NO The following...
Suppose a 250.mL flask is filled with 1.6mol of O2 and 1.2mol of NO The following reaction becomes possible: N2(g)+O2(g)---2NOg The equilibrium constant K for this reaction is 0.197 at the temperature of the flask. Calculate the equilibrium molarity of N2 Round your answer to two decimal places.
Suppose a 250.mL flask is filled with 1.7mol of O2 and 1.6mol of NO. The following...
Suppose a 250.mL flask is filled with 1.7mol of O2 and 1.6mol of NO. The following reaction becomes possible: +N2g + O2g <-->2NOg The equilibrium constant K for this reaction is 0.628 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. *** must calculate for M first by dividing the moles by Liters before placing in the ICE table.
The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction: CO2(g)...
The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) If 0.65 moles of CO2 and 0.65 moles of H2 are introduced into a 1.0-L flask, what will be the concentration of CO when equilibrium is reached? The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) If 0.65 moles of CO2 and 0.65 moles of...
The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction: CO2(g)...
The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) If 0.35 moles of CO2 and 0.35 moles of H2 are introduced into a 1.0-L flask, what will be the concentration of CO when equilibrium is reached? The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) If 0.35 moles of CO2 and 0.35 moles of...
Consider the reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.21 −L flask at 500 K contains...
Consider the reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.21 −L flask at 500 K contains 9.04 g CO and 0.58 g of H2. At equilibrium, the flask contains 2.34 g CH3OH. Calculate the equilibrium constant at this temperature.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT