(PH2)(PN2)/(PNH3) Be sure to answer all parts. Write the KP expression for the following reaction: N2(g)...

(P_H₂)(P_N₂)/(P_NH₃)

Be sure to answer all parts.

Write the K_P expression for the following reaction:

N₂(g) + 3H₂(g) ⇌ 2NH₃(g)

Use a format similar to this:

K_P = (PH2O)^2/(PO2)(PH2)^2

K_P =

Expert Solution

queen_honey_blossom answered 11 months ago

Be sure to answer all parts. Consider the following reaction at equilibrium: A(g) ⇆ 2B(g) From...

Be sure to answer all parts. Consider the following reaction at equilibrium: A(g) ⇆ 2B(g) From the data shown here, calculate the equilibrium constant (both KP and Kc) at each temperature. Is the reaction endothermic or exothermic? Temperature (°C) [A] (M) [B] (M) 200 0.0180 0.870 300 0.150 0.790 400 0.240 0.695 Kc(200°C) = KP(200°C) = Kc(300°C) = KP(300°C) = Kc(400°C) = KP(400°C) = Cannot be determined. The reaction is exothermic. The reaction is endothermic

The following reaction N2 (g) + O2 (g) ⇔ 2 NO (g) has a KP =...

The following reaction N2 (g) + O2 (g) ⇔ 2 NO (g) has a KP = 0.032 at a particular temperature. At that temperature, a vessel is filled with 0.040 atm of N2 (g), 0.040 atm of O2 (g) and 0.043 atm of NO (g). What is the pressure of NO (g) at equilibrium?

Be sure to answer all parts. At 430 ° C, the equilibrium constant (KP) for the...

Be sure to answer all parts. At 430 ° C, the equilibrium constant (KP) for the reaction 2NO(g) + O2(g) ⇆ 2NO2(g) is 1.5 × 105. In one experiment, the initial pressures of NO, O2, and NO2 are 7.4 × 10−3 atm, 4.2 × 10−2 atm, and 0.20 atm, respectively. Calculate QP and predict the direction that the net reaction will shift to reach equilibrium. What is QP for the experiment? In which direction will the system proceed to reach equilibrium?...

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Be sure to answer all parts. The equilibrium constant Kc for the Reaction: H2(g) + CO2(g) <--> H2O(g) + CO(g) is 4.2 at 1650 C. Initially 0.87 mol H2 and 0.87 mol CO2 are injected into a 4.9 L flask. Calculate the concentraion of each species at equilibrium Equilibrium concentration of H2: ____ M Equilibrium concentraion of CO2: ___ M Equilibrium concentraion of H2O: _____M Equilibrium concentration of CO: ______M

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Be sure to answer all parts. At 1280°C the equilibrium constant Kc for the reaction Br2(g) ⇌ 2Br(g) is 1.1 ×10−3. If the initial concentrations are [Br2] = 0.0320 M and [Br] = 0.0290 M, calculate the concentrations of these two species at equilibrium. [Br2]eq = [Br]eq =

At a particular temperature Kp = 0.041 for the reaction N2(g) + O2(g) ⇄ 2NO(g) What...

At a particular temperature Kp = 0.041 for the reaction N2(g) + O2(g) ⇄ 2NO(g) What is the equilibrium partial pressure of NO if a flask initially contains 0.12 atm of all three gases? Report the pressure of NO in atm rounded to the nearest hundredth of an atm.

Be sure to answer all parts. Ammonia is produced by the reaction of nitrogen and hydrogen...

Be sure to answer all parts. Ammonia is produced by the reaction of nitrogen and hydrogen according to the equation N2(g) + 3H2(g) → 2NH3(g) 1. Calculate the mass of ammonia produced when 30.0 g of nitrogen react with 11.3 g of hydrogen. 2. Which is the excess reactant and how much of it will be left over when the reaction is complete?

At 850K, the value of the equilibrium constant Kp for the ammonia synthesis reaction: N2(g)+H2(g)--> N2H2(g)...

At 850K, the value of the equilibrium constant Kp for the ammonia synthesis reaction: N2(g)+H2(g)--> N2H2(g) is 0.3290. If a vessel contains an initial reaction mixture in which [N2]= 0.0200 M, [H2]=0.0200 M, and [N2H2]= 0.000150 M, what will the [N2H2] be when equilibrium is reached? The answer is not: 0.000298, .00681, .000172, .000148, .00031, .00471 please help!

Be sure to answer all parts. Write the balanced equations corresponding to the following rate expressions:...

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Consider the equilibrium N2(g)+O2(g)+Br2(g)⇌2NOBr(g) Part A Calculate the equilibrium constant Kp for this reaction, given the...

Consider the equilibrium N2(g)+O2(g)+Br2(g)⇌2NOBr(g) Part A Calculate the equilibrium constant Kp for this reaction, given the following information (at 295 K ): 2NO(g)+Br2(g)⇌2NOBr(g)Kc=2.1 2NO(g)⇌N2(g)+O2(g)Kc=2.2×1030 Express your answer using two significant figures.

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