Express the equilibrium constant for the following reaction.

7 N2(g) + 21 H2(g) ⇔ 14 NH3(g)

Question

Express the equilibrium constant for the following reaction.

7 N2(g) + 21 H2(g) ⇔ 14 NH3(g)

BlackTom AI · Accepted Answer

The problem asks for the equilibrium constant expression for the reaction: 7 N2(g) + 21 H2(g) ⇔ 14 NH3(g).
First, recall the general rule: for a balanced gaseous reaction aA + bB ⇌ cC, the equilibrium constant expression (Kc) is given by Kc = [C]^c / ([A]^a [B]^b), using concentrations in mol/L at constant temperature.
In this reaction, the products are NH3 with coefficient 14, and the reactants are N2 with coefficient 7 and H2 with coefficient 21.
Applying the rule, the numerator contains the product concentration raised to its stoichiometric power, and the denominator contains each reactant concentration raised to its stoichiometric power.
Thus, the correct Kc expression is: Kc = [NH3]^{14} / ([N2]^{7} [H2]^{21}).
If one were to use partial pressures instead of concentrations (Kp), the expression would be Kp = (P_NH3)^{14} / ((P_N2)^{7} (P_H2)^{21}), provided the temperature is the same and appropriate unit conventions are applied.
Note about the provided options: the list of answer choices appears to be missing in this prompt, so there are no specific choices to evaluate for correctness here. If options were given, you would compare each to the derived expression, checking that the exponents match the balanced equation and that NH3 appears in the numerator while N2 and H2 appear in the denominator with their respective stoichiometric powers.
In summary, the central idea is assigning NH3 to the numerator with exponent 14, and placing N2 and H2 in the denominator with exponents 7 and 21 respectively to reflect the balanced equation.

Express the equilibrium constant for the following reaction. 7 N2(g) + 21 H2(g) ⇔ 14 NH3(g)

查看解析

登录即可查看完整答案

类似问题

Consider the reaction below: 3C(s) + 3H2(g) ⥫⥬ CH4(g) + C2H2(g) The equilibrium expression for the reaction above is:

Use the data given to calculate the value of Κ for the reaction at 5°C Ag+(aq) + Cl− (aq) AgCl(s) AgCl(s) Ag+(aq) Cl− (aq) S° (J K−1 mol−1) 96.2 72.68 56.4 ΔH°f (kJ/mol) −127.07 105.58 −167.2

Use the data given to calculate the value of Κ for the reaction at 25°C AgCl(s) Ag+(aq) + Cl− (aq) AgCl(s) Ag+(aq) Cl− (aq) S° (J K−1 mol−1) +96.2 +72.68 +56.4 ΔH°f (kJ/mol) −127.07 +105.58 −167.2

The equilibrium constant expression for the reaction shown below is Ag3PO4(s) 3 Ag+(aq) + PO43− (aq)

Express the equilibrium constant for the following reaction. 10 PCl5(g) 10 PCl3(g) + 10 Cl2(g)

Express the reverse equilibrium constant for the following reaction. 3 H2(g) + 3 Br2(g) 6 HBr(g)

Express the equilibrium constant for the following reaction. CsIO3(s) CsIO(s) + O2(g)

Express the equilibrium constant for the following reaction. 3 P4(s) + 15 O2(g) 3 P4O10(s)

更多留学生实用工具

考试浏览器助手

风格化写作助手

论文查重助手

文献引用助手

课堂转译助手

课堂笔记助手

Quiz搜索助手

学校历年真题

智能刷题助手

智能匹配练习

希望你的学习变得更简单