For the next two questions: A chemist mixes 0.200 atm N2O4, and 0.100 atm NO2 in a closed flask. The compounds form an equilibrium of 2NO2(g) ? N2O4(g). The Kp is 1.52 at 319K. 45. You calculate the equilibrium expression to obtain -0.1848 + 1.608x + 6.08x² = 0, where x is concentration change of N2O4. The equilibrium partial pressure of NO2 (in atm) at 319K is: a) 0.273 atm b) 0.0866 atm c) 0.113 atm d) 0.551 atm e) There is more than one possible partial pressure.
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Step 1: Write the balanced chemical equation for the reaction: 2 NO2 ⇌ N2O4 Show more…
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At a particular temperature, $K_{\mathrm{p}}=0.25$ for the reaction $$ \mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g) $$ a. A flask containing only $\mathrm{N}_{2} \mathrm{O}_{4}$ at an initial pressure of 4.5 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. b. A flask containing only $\mathrm{NO}_{2}$ at an initial pressure of 9.0 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. c. From your answers to parts a and b, does it matter from which direction an equilibrium position is reached? d. The volume of the container in part a is decreased to one-half the original volume. Calculate the new equilibrium partial pressures.
At a particular temperature, $K_{\mathrm{p}}=0.25$ for the reaction $$\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)$$ a. A flask containing only $\mathrm{N}_{2} \mathrm{O}_{4}$ at an initial pressure of 4.5 $\mathrm{atm}$ is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. b. A flask containing only $\mathrm{NO}_{2}$ at an initial pressure of 9.0 $\mathrm{atm}$ is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. c. From your answers to parts a and b, does it matter from which direction an equilibrium position is reached?
At a particular temperature, $K_{\mathrm{p}}=0.25$ for the reaction $$\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)$$. a. A flask containing only $\mathrm{N}_{2} \mathrm{O}_{4}$ at an initial pressure of 4.5 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. b. A flask containing only $\mathrm{NO}_{2}$ at an initial pressure of 9.0 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. c. From your answers to parts a and b, does it matter from which direction an equilibrium position is reached?
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