Explanation:
Reaction equation for the given chemical reaction is as follows.
Equation for reaction quotient is as follows.
Q =
=
= 0.256
As, Q > K (= 0.12)
The effect on the partial pressure of as equilibrium is achieved by using Q, is as follows.
First, find the number of moles for each element. The molar mass for nitrogen is 14 g/mol and that of hydrogen is 1 g/mol.
1.40 g N / 14 g/mol = 0.1 mol N
0.20 g H / 1 g/mol = 0.2 mol H
Find the mole ratio. Divide both numbers with the much lower value. In this case, it is 0.1 mol N.
For N: 0.1 ÷ 0.1 = 1
For H: 0.2÷0.1 = 2
Thus, the empirical formula is .
Answer:
1. Hydrogen Iodide
2. 6 molecules of Hydrogen Iodide
3. Iodine is the limiting reagent
Explanation:
The image of the illustration in the question has been attached:
1. The illustration represents a mixture of hydrogen ( light blue ) and iodine ( purple )
H₂ + I₂ ---> 2HI
This forms hydrogen iodide.
2. In the given illustration, 6 product molecules of Hydrogen Iodide. This is indicated in the box on the right side of the illustration.
3. The limiting reagent is the reactant that determines how much of the products are made. It is the substance that is totally consumed when the chemical reaction is completed. In the box on the right side of the illustration, you will see that hydrogen which is indicated by blue is in excess. The limiting reagent is the one that is completely consumed which is the iodine.
