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?

Expert Solution

queen_honey_blossom answered 1 year ago

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.

Consider the following reaction at 173 K: 2 N2O (g) → 2 N2 (g) + O2...

Consider the following reaction at 173 K: 2 N2O (g) → 2 N2 (g) + O2 (g) In one of your laboratory experiments, you determine the equilibrium constant for this process, at 173 K, is 6.678E+57. You are given a table of data that indicates the standard heat of formation (ΔHoform) of N2O is 82.0 kJ/mol. Based on this information, what is the standard entropy change (ΔSorxn) for this reaction at 173 K? ΔSorxn(J/K)=

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

At 3748°C, K = 0.093 for the following reaction. N2(g) + O2(g) equilibrium reaction arrow 2 NO(g) Calculate the concentrations of all species at equilibrium for each of the following cases. (a) 1.6 g N2 and 3.0 g O2 are mixed in a 1.3-L flask. (b) 2.0 mol pure NO is placed in a 2.1-L flask.

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.

A.) For which reaction will Kp = Kc? 2 H2O(l) ↔ 2 H2(g) + O2(g) 2...

A.) For which reaction will Kp = Kc? 2 H2O(l) ↔ 2 H2(g) + O2(g) 2 HgO(s) ↔ Hg(l) + O2(g) S(s) + O2(g) ↔ SO2(g) H2CO3(s) ↔ H2O(l) + CO2(g) CaCO3(s) ↔ CaO(s) + CO2(g) B.) How does an increase in the pressure within the container by the addition of the inert gas E affect the amount of C present at equilibrium for the following reaction? A(g) + 3 B(g) ↔ 2 C(g) + D(g) ΔH° = -65 kJ...

The reaction 2NO(g) + O2(g) ⇌ 2NO2(g) has Kp = 1.65 × 1011 at 25°C. To...

The reaction 2NO(g) + O2(g) ⇌ 2NO2(g) has Kp = 1.65 × 1011 at 25°C. To a 1.00 L flask, 1.03 g of NO and 532 mL of O2 measured at 29°C and 772 torr are mixed. When the mixture comes to equilibrium at 25°C, what is the concentration of NO(g)? If needed, use “E” for scientific notation. Do not enter units as part of your answer. Report your answer to the correct number of significant figures.

The reaction 2NO(g) + O2(g) ⇌ 2NO2(g) has Kp = 1.65 × 1011 at 25°C. To...

The reaction 2NO(g) + O2(g) ⇌ 2NO2(g) has Kp = 1.65 × 1011 at 25°C. To a 1.00 L flask, 1.03 g of NO and 532 mL of O2 measured at 29°C and 772 torr are mixed. When the mixture comes to equilibrium at 25°C, what is the concentration of NO(g)? If needed, use “E” for scientific notation. Do not enter units as part of your answer. Report your answer to the correct number of significant figures.

Consider the first order reaction 2 N2O(g) ⟶ 2 N2 (g) + O2(g). What will [N2O]...

Consider the first order reaction 2 N2O(g) ⟶ 2 N2 (g) + O2(g). What will [N2O] be after 3 half lives when 0.25 moles N2O is placed in a 1.00-L reaction vessel?

For the reaction: N2(g) + 2 O2(g) ↔ 2 NO2(g), Kc = 8.3 × 10-10 at...

For the reaction: N2(g) + 2 O2(g) ↔ 2 NO2(g), Kc = 8.3 × 10-10 at 25°C. What is the concentration of N2 gas at equilibrium when the concentration of NO2 is twice the concentration of O2 gas?

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...

Question

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

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

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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...