All of the reactions shown are oxidationreduction reactions except A) N2(g) + O2 (g) → 2...

All of the reactions shown are oxidationreduction reactions except

A) N2(g) + O2 (g) → 2 NO(g)

B) 2 Fe2O3 (s) → 4 Fe(s) + 3 O2 (g)

C) Zn(s) + 2 HCl(aq) → ZnCl2 (aq) + H2 (g)

D) CH4(g) + 2 O2 (g) → CO2(g) + 2 H2O(l)

E) K2SO4(aq) + BaCl2(aq) → BaSO4(s) + 2 KCl(aq)

Expert Solution

queen_honey_blossom answered 2 years ago

PART A.Identify the proper form of the equilibrium-constant expression for the equation N2(g)+O2(g)⇌2NO(g) 1.K=[NO][N2][O2] 2.K=[NO]2[N2][O2] 3.K=[N2][O2][NO]2...

PART A.Identify the proper form of the equilibrium-constant expression for the equation N2(g)+O2(g)⇌2NO(g) 1.K=[NO][N2][O2] 2.K=[NO]2[N2][O2] 3.K=[N2][O2][NO]2 4.K=2[NO][N2][O2] PART B. The equilibrium-constant of the reaction NO2(g)+NO3(g)⇌N2O5(g) is K=2.1×10−20. What can be said about this reaction? 1.At equilibrium the concentration of products and reactants is about the same. 2.At equilibrium the concentration of products is much greater than the concentration of reactants. 3.At equilibrium the concentration of reactants is much greater than that of products. 4.There are no reactants left over once...

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

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Given the data N2(g) + O2(g) → 2 NO(g) ΔH = +180.7 kJ 2 NO(g) +...

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Consider the equilibrium N2(g) + O2(g) ⇄ 2 NO(g) At 2300 K the equilibrium constant K = 1.7 × 10-3. Suppose that 0.0150 mol NO(g), 0.250 mol N2(g), and 0.250 mol O2(g) are placed into a 10.0-L flask and heated to 2300 K. The system is not at equilibrium. Determine the direction the reaction must proceed to reach equilibrium and the final equilibrium concentrations of each species. to the right to the left [N2] =____ mol/L [O2] = ____mol/L [NO]...

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At 3748°C, K = 0.093 for the following reaction. N2(g) + O2(g) equilibrium reaction arrow 2...

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