Question

the reaction between oxygen and nitrogen gases at high temperatures contribute to air pollution: N2(g) +...

the reaction between oxygen and nitrogen gases at high temperatures contribute to air pollution: N2(g) + O2 = 2 NO ; Kc 1.0*10^-5 at 1500 K ; suppose air has [N2] = 0.080 M and [O2] =0.020 M what is the concentration of NO at equilibrium (do it using small x approximation and don't use quadratic formula)

0 0
Add a comment Improve this question Transcribed image text
Answer #1

given, Initial concentration of N2 = 0.08 M Initial concentration of 02 = 0.02 M equilibrium constant = Kc = 1.0x10-= 0.00001

Add a comment
Know the answer?
Add Answer to:
the reaction between oxygen and nitrogen gases at high temperatures contribute to air pollution: N2(g) +...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

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
  • The reaction N2(g) + O2(g) ⇄ 2 NO(g) contributes to air pollution whenever a fuel is...

    The reaction N2(g) + O2(g) ⇄ 2 NO(g) contributes to air pollution whenever a fuel is burned in air at a high temperature, as in a gasoline engine. At 1500 K, Kc = 1.0×10-3. Suppose a sample of air has [N2] = 0.70 mol/L and [O2] = 0.20 mol/L before any reaction occurs. Calculate the equilibrium concentrations of reactants and products after the mixture has been heated to 1500 K. [N2] = M [O2] = M [NO] = M

  • Nitrogen and oxygen react at high temperatures. N2(g) + O2(g) equilibrium reaction arrow 2 NO(g) ΔH...

    Nitrogen and oxygen react at high temperatures. N2(g) + O2(g) equilibrium reaction arrow 2 NO(g) ΔH = 182.6 kJ (a) Write the expression for the equilibrium constant (Kc) for this reversible reaction. (Concentration equilibrium expressions take the general form: Kc = [C]c / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.)

  • Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. 29. N2(g)+O...

    Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. 29. N2(g)+O:(g) 2NO(g) The equilibrium constant Kp for the reaction is 0.0025 at 2127 C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen?

  • Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high...

    Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N2(g) + O2(g) <--> 2NO(g) The equilibrium constant Kp for the reaction is 0.0025 at 2127°C. If a 2.00 L container is charged with 5.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, (i) what will be the equilibrium partial pressure of nitrogen, PN2, and (ii) how many grams of O2(g) are present at equilibrium?...

  • Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high...

    Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N2(g) + O2(g) ⇌ 2NO(g) The equilibrium constant Kp for the reaction is 0.31 at 1200 °C. If a container is charged with 0.344 atm of nitrogen and 0.454 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitric oxide? Report your answer to three significant figures

  • Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases,...

    Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine.CCl4(g) + 1/2O2(g) COCl2(g) + Cl2(g), Kc = 4.4 × 109 at 1,000 KCalculate Kc for the reaction 2CCl4(g) + O2(g) 2COCl2(g) + 2Cl2(g).

  • The rate constant for the reaction of nitrogen with oxygen was determined at four temperatures. N2(g)...

    The rate constant for the reaction of nitrogen with oxygen was determined at four temperatures. N2(g) + O2(g) + 2NO(g) T(K) 250 275 k(cm3/moleculeos) 7.18 x 10-8 1.36 x 10-7 2.31x 10-7 3.46 x 10-7 300 325 Calculate the activation energy of the reaction. kJ/mol Part 2 (2 points) Calculate the frequency factor A for the reaction. x 10 cm3/moleculeos +

  • Nitrogen and oxygen gas react as high temperatures to form nitric oxide, a component of photochemical...

    Nitrogen and oxygen gas react as high temperatures to form nitric oxide, a component of photochemical smog. Net reaction: the net reaction is N2 + O2 --> 2NO Proposed mechanism: O2 <====> 2O   (fast, at equilibrium)                                         N2 + O <-- --> NO + N   (fast, not at equilibrium)                                     N + O2 ----> NO + O    (Slow) a.) Derive the rate law for the proposed mechanism. rate = ____________________________ b.) What is the initial rate law, when very little...

  • Nitric oxide (NO) gas partially decomposes into nitrogen (N2) and oxygen (O2) gases after being placed...

    Nitric oxide (NO) gas partially decomposes into nitrogen (N2) and oxygen (O2) gases after being placed in a closed container. 2NO (8) = N2 (8) + O2 (8) What is true about the reaction? O The rate of the forward reaction is at its maximum when pure NO gas is first placed in the container. O At equilibrium, the concentration of O2 gas is the same as the concentration of NO gas. O All of the NO gas is eventually...

  • The air pollutant NO is produced in automobile engines from the high-temperature reaction N2(g)+O2(g)⇌2NO(g);Kc=1.7×10−3 at 2300...

    The air pollutant NO is produced in automobile engines from the high-temperature reaction N2(g)+O2(g)⇌2NO(g);Kc=1.7×10−3 at 2300 K. If the initial concentrations of N2 and O2 at 2300 K are both 1.58 M, what are the concentrations of NO when the reaction mixture reaches equilibrium? Concentrations of NO= UNITS If the initial concentrations of N2 and O2 at 2300 K are both 1.58 M, what are the concentrations of N2 when the reaction mixture reaches equilibrium? Concentrations of O2=   If the...

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
ADVERTISEMENT