At 1800 K, the equilibrium constant is \( K_{eq} = 1.03 \times 10^{-4} \) for the reaction \( \text{N}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{NO}(g) \).**Question:**What is the equilibrium partial pressure of NO in air, which has an initial total pressure of 1.000 atm if the composition of air is 80.0 percent \( \text{N}_2 \) and 20.0 percent \( \text{O}_2 \)?**Answer Options:**- \( \bullet \) 0.004009 atm- ○ 0.0113 atm- ○ 0.403 atm- ○ 0.00202 atm- ○ 0.0406 atmThere are no graphs or diagrams included in this text. The question is formatted as a multiple-choice problem typically found in chemistry practice materials to assess understanding of chemical equilibria and partial pressures.

The equilibrium reaction given is, => N2 (g) + O2 (g) ------------> 2 NO (g) Given : Total…

At 1800 K the equilibrium constant is Keq = 1.03 x 104 for the reaction N2(g) + O2(g) = 2NO(g). What is the equilibrium partial pressure of NO in air, which has an initial total pressure of 1.000 atm if the composition of air is 80.0 percent N2 and 20.0 percent O2? 0.004009 atm O 0.0113 atm O 0.403 atm O 0.00202 atm O 0.0406 atm

At 1800 K the equilibrium constant is Keq = 1.03 x 104 for the reaction N2(g) + O2(g) = 2NO(g). What is the equilibrium partial pressure of NO in air, which has an initial total pressure of 1.000 atm if the composition of air is 80.0 percent N2 and 20.0 percent O2? 0.004009 atm O 0.0113 atm O 0.403 atm O 0.00202 atm O 0.0406 atm

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The equilibrium constant, K, for the following reaction is 6.30 at 723 K. 2NH3(g) ⇒N₂(g) + 3H₂(g) If an equilibrium mixture of the three gases in a 10.9 L container at 723 K contains 0.409 mol of NH3(g) and 0.291 mol of N₂, the equilibrium concentration of H₂ is M.
Suppose a 250. mL flask is filled with 1.2 mol of Br,, 1.4 mol of OCl, and 1.1 mol of BrCl. The following reaction becomes possible: Br, (g) +OCl, (g) - BrOC1 (g) +BrC1(g) The equilibrium constant K for this reaction is 0.483 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places. OM
The equilibrium constant for the reaction shown below is 61.2 H, (g) + Br, (g) = 2HB1(g) Write an expression for the equilibrium constant, K What is the equilibrium concentration of Br2, if [HBr]=0.48 M and [H2] = 0.26 M at equilibrium?
At a certain temperature, the equilibrium constant K for the following reaction is 0.0036: H₂(g) + 1₂(g) → 2 HI(g) Use this information to complete the following table. O There will be very little H₂ and I2. Suppose a 6.0 L reaction vessel is filled with 1.9 mol of H₂ and 1.9 mol of I₂. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little HI. ONeither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 2 HI(g) H₂(9)+1₂(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 2 H₂(g) +21₂(g) 4 HI(g) 0x10 ?
The folllowing reaction is in a state of dynamic chemical equilibrium PCl5(g) ➡ PCl3(g) + Cl2(g) ΔH=+Ve Explain the term dynamic equilibrium and give 2 conditions needed for a system to attain a state of chemical equilibrium. What will be the effect on the position of the above equilibrium if the total pressure on the system was Increased at constant temperature. the numerical value of the equilibrium constant, Kc, of the reaction if the temperature of the reaction is increased. Write the equilibrium constant expression (Kc) giving units for the reaction above.
The equilibrium constant, Kc, for the following reaction is 57.6 at 277 K. 2CH₂Cl₂ (g) CH4 (9) + CCl4 (9) When a sufficiently large sample of CH₂Cl₂ (g) is introduced into an evacuated vessel at 277 K, the equilibrium concentration of CC14 (g) is found to be 0.383 M. Calculate the concentration of CH₂Cl₂ in the equilibrium mixture. [CH₂Cl₂] = M
The following reaction has an equilibrium constant, Kc equal to 3.59 at 900 °C. CH4(g) + 2H₂S(g) — CS2(g) + 4 H2(g) At a particular time during the reaction, the following composition has been found: [CH4(g)] = 1.20 M, [CS2(g)] = 1.15 M, [H₂S(g)] = 1.31 M, [H2(g)] = 1.85. Predict the activity of the reaction during the particular time above. The reaction should go to the left (or reverse) The reaction should go to the right (or forward) The reaction is at a standstill The reaction activity cannot be determined There is no basis for prediction.
Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)
The equilibrium constant, Kc, for the following reaction is 0.00650 at 298 K. 2NOBr(g) ⇒ 2NO(g) + Br₂ (g) If an equilibrium mixture of the three gases in a 15.6 L container at 298 K contains 0.201 mol of NOBr(g) and 0.284 mol of NO, the equilibrium concentration of Br₂ is | M.
Please don't provide handwritten solution ....
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 NO(g) + Cl₂(g) = 2 NOC1 (g) K₁₂=4.×100 He fills a reaction vessel at this temperature with 8.0 atm of nitrogen monoxide gas and 7.5 atm of chlorine gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NOC1, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NOC1 at right. Round your answer to 1 significant digit. O yes O no 0 atm X
The equilibrium constant for the following reaction is 49 at 450 °C. If 0.22 mole of I2 , 0.22 mole of H2 , and 0.66 mole of HI were put into an evacuated 1.00-liter container, would the system be at equilibrium? If not, what must occur to establish equilibrium? H2 (g) + I2 (g) = 2HI (g)