Question

At 1700 C, the equilibrium constant, Kc, for the following reaction is 4.10 x 10^ 4....

At 1700 C, the equilibrium constant, Kc, for the following reaction is 4.10 x 10^ 4. N2(g)+O2(g) --><-- 2NO(g) What percentage of O2 will react to form NO if 0.765 mol of N2 and 0.765 mol of O2 are added to a 0.763-L container and allowed to come to equilibrium at 1700 C?

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
4. At a given temperature, the equilibrium constant Kc for the reaction 2SO2(g) + O2(g) ⇌...
4. At a given temperature, the equilibrium constant Kc for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 3.0x10^9 . If 1.00 mol of SO2 and 2.00 mol of O2 are placed in a 1.00 L container and allowed to react to equilibrium at this temperature, what is the concentration of SO3 at equilibrium? a) 0.500 M b) 1.00 M c) 2.00 M d) 3.87 x10^4 M e) none of these
At 2000 ?C the equilibrium constant for the reaction 2NO(g)???N2(g)+O2(g) is Kc=2.4
At 2000 ?C the equilibrium constant for the reaction 2NO(g)???N2(g)+O2(g) is Kc=2.4
At 2000 degrees celcius, the gas-phase equilibrium 2NO(g)=N2(g)+o2(g) has an equilibrium constant of Kc=2.4X10^3. Use this...
At 2000 degrees celcius, the gas-phase equilibrium 2NO(g)=N2(g)+o2(g) has an equilibrium constant of Kc=2.4X10^3. Use this information to answer the following. a) Determine the relationship between Kc and Kp for this equilibrium. What is the value of Kp? b) Determine the value of Kc for the reaction 1/2N2(g)+1/2O2(g)=NO(g). c) Determine the equilibrium concentrations of NO, N2, O2 when 0.200 mol NO(g) is placed into a (n evacuated) 1.000 L container and heated to 2000 degrees celcius.
The equilibrium constant (Kc) for the following reaction is 6.7 × 10–10 at 630 °C. N2(s)...
The equilibrium constant (Kc) for the following reaction is 6.7 × 10–10 at 630 °C. N2(s) + O2(g) 2 NO(g) What is the equilibrium constant for the reaction below at the same temperature? 1/2 N2(g) + 1/2 O2(g) NO(g) a. 4.5 × 10−19 b. 3.4 × 10−10 c. 1.3 × 10−9 d. 1.8 × 10−5 e. 2.6 × 10−5
The equilibrium constant for the reaction N2 + O2<--> 2NO is 1.69 × 10^?3 at 2300...
The equilibrium constant for the reaction N2 + O2<--> 2NO is 1.69 × 10^?3 at 2300 K. A mixture consisting of 2 mol of nitrogen and 1.0 mol of oxygen is heated to 2300 K at 1 bar and allowed to come to equilibrium. Calculate the mole fraction of NO at equilibrium.
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2(g)...
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2(g) <----> 2HI(g) Kc=53.3 At this temperature, 0.400 mol of H2 and 0.400 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2(g)...
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2(g) <-------> 2 HI(g) Kc=53.3 At this temperature, 0.600 mol of H2 and 0.600 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?
The equilibrium constant, Kc , for the following reaction is 1.80×10-4 at 298 K. NH4HS(s)-----> NH3(g)...
The equilibrium constant, Kc , for the following reaction is 1.80×10-4 at 298 K. NH4HS(s)-----> NH3(g) + H2S(g) If an equilibrium mixture of the three compounds in a 6.21 L container at 298 K contains 3.17 mol of NH4HS(s) and 0.335 mol of NH3, the number of moles of H2S present is ____ moles??
Nitrogen and oxygen gases may react to form nitrogen monoxide. At 1500 °C, Kc equals 1.0...
Nitrogen and oxygen gases may react to form nitrogen monoxide. At 1500 °C, Kc equals 1.0 x 10-5. N2(g) + O2(g) = 2 NO(g) If 0.01 mol N2 and 0.01 mol O2 are sealed in a 1.0 L flask at 1500 °C, the concentration of NO(g) when equilibrium is established is ___ x 10-5 M. Sulfuryl chloride decomposes to sulfur dioxide and chlorine.         SO2Cl2(g) = SO2(g) + Cl2(g) Kc is 0.045 at 648 K. If an initial concentration of...
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H,2(g) + I,2(g)...
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H,2(g) + I,2(g) --> 2HI(g)    Kc=53.3 At this temperature, 0.600 mol of H2 and 0.600 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT