At 250°C the system below contains 0.0204 mol of H2le), 0.0363 mol of U2(g) , and H2O in a 2.94L container. Calculate the value of the equilibrium constant, K. 2H2() + O2(e) 2H2Og) . O 455 O 5.30 x 106 O 5.30 O 2.09 x 104 O 1.80 x 106 ) 5.54 x 107 2.38 x 103 E 1.89 x 107

For the equilibrium reaction.   2IBr (g) I2 (g) + Br2 (g) Kc=.0085.  If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components.   Consider the decomposition reaction at 555 K   4POCl3 (g)    P4  (g) + 2O2  (g) + 6Cl2  (g)   If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm.  Find Kp and Kc.

Consider the reaction: Important values if I for this question C(s) + O₂(g) → CO₂(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: C(s) + 1/2O₂(g) → CO(g) K₁ CO(g)+1/2O,(g)=CO2(g) K2 For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared. K =

Be sure to answer all parts. The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) = 2NO(g) K = 4.3 x 10-25 2NO(g) + O2(g) == 2NO,(g) K= 6.4 × 10' Determine the value of the equilibrium constant for the following equation at the same temperature: N2(g) + 202(g) = 2NO2(g) K. - x 10 (Enter your answer in scientific notation.)

Part A Estimate K at 120 °C for the reaction 2 SO₂ (g) + O₂(g) 2503 (9). Use Kp = 9.1 x 102 at 800 K, A.H=-1.8 x 10 J/mol. Express your answer using two significant figures. ΠΕ ΑΣΦ X√x √x X Kp 1.3.10-8 X Xxx ? x-10" CXI

Consider the reaction 2 NH3 (g) ⇄ N2 (g) + 3 H2 (g). Suppose 6 moles of pure ammonia are placed in a 1.0 liter flask and allowed to reach equilibrium. If X represents the concentration (in M) of nitrogen present in the system once equilibrium is reached, which of the following will represent the concentration of ammonia in M? Group of answer choices 6–(X/2) 6–X 6–2X 6+2X 6+X

Consider the reaction: SO₂(g) + 1/2O₂(g) ⇒ SO3 (9) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K2, for the reactions below: 2S(s) + 30₂(g) ⇒ 2SO3 (9) K₁ S(s) + O₂(g) → SO₂(g) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared. K= An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer.

Nitric oxide, an important pollutant in air, is formed from the elements nitrogen and oxygen at high temperatures, such as those obtained when gasoline burns in an automobile engine. At 2000°C, K for the reaction N2(g) + O2(g) ⇆  2NO(g) is 0.010. If 0.40 moles of N2, 0.10 moles of O2, and 0.080 moles of NO are placed in a 1.0-liter container, what will be the concentration of O2 at equilibrium?

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Calculate the equilibrium constant (Kc) for the given reaction. Kp = 0.003 and T = 298 K 2C0(6) + O2(e) → 2CO2(8)