Question

Be sure to answer all parts.The equilibrium constant (Kc) for the formation of nitrosyl chloride, an orange-yellow compound, from nitric oxide and molecular chlorine 2NO(g) + Cl2(g) ⇌ 2NOCl(g) is 2 × 105 at a certain temperature. In an experiment, 6.00 × 10−2 mole of NO, 6.70 × 10−3 mole of Cl2, and 4.00 moles of NOCl are mixed in a 1.30−L flask. What is Qc for the experiment? × 10(Enter your answer in scientific notation.) In which direction will the system proceed to reach equilibrium? The reaction will proceed to the left. The reaction will proceed to the right. The reaction is at equilibrium.

Answer 1

STEP-BY-STEP EXPLANATION*

Given information*

`\begin{gathered} \text{The number of moles of NO = 6.00 }*10^(-2)\text{ moles} \\ \text{The number of moles of Cl2 = 6.7 }*10^(-3)\text{ moles} \\ \text{The number of moles of NOCl = 4.00 moles} \\ K_c\text{ = 2 }*10^5 \end{gathered}`

The first step is to write the balanced equation of the chemical reaction*

`2NO_((g))+Cl_((2)(g))\rightleftarrows2NOCl_((g))`

The next step is to write the chemical equilibrium expression for the above reaction*