Question

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.

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 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.
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 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 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 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
At a given temperature the gas phase reaction: N2 + O2 2NO has an equilibrium constant...
At a given temperature the gas phase reaction: N2 + O2 2NO has an equilibrium constant of4.00x10-2 . What will be the concentration of NO at equilibrium, if1.00 moles of nitrogen and 1.00 moles of oxygen are allowed to cometo equilibrium in a 250 mL flask?
Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.63 L flask at a certain...
Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.63 L flask at a certain temperature initially contains 0.767 g H2 and 97.0 g I2. At equilibrium, the flask contains 90.6 g HI. Calculate the equilibrium constant (Kc) for the reaction at this temperature. Express your answer using two significant figures.
A flask is filled with PCl5 to a pressure of 2.00 atm at 300°C and allowed...
A flask is filled with PCl5 to a pressure of 2.00 atm at 300°C and allowed to come to equilibrium according to the reaction: PCl5(g) ⇄ PCl3(g) + Cl2(g) Analysis shows the total pressure in the flask at equilibrium is 3.96 atm. Calculate the equilibrium constant Kp for the reaction. A)49.0 B)3.96 C)96.0 D)0.886 E)7.84
When N2O5(g) is heated, it dissociates into N2O3(g) and O2(g) according to the following reaction: N2O5(g)...
When N2O5(g) is heated, it dissociates into N2O3(g) and O2(g) according to the following reaction: N2O5(g) ⇌ N2O3(g)+O2(g) Kc=7.75 at a given temperature. The N2O3(g) dissociates to give N2O(g) and O2(g) according the following reaction: N2O3(g)⇌N2O(g)+O2(g) Kc=4.00 at the same temperature. When 4.00 mol of N2O5(g) is heated in a 1.00-L reaction vessel to this temperature, the concentration of O2(g) at equilibrium is 4.50 mol/L. Part A Find the concentration of N2O5 in the equilibrium system. Express your answer using...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT