<u>Answer:</u> The partial pressure of carbon dioxide at equilibrium is 0.0056 atm
<u>Explanation:</u>
The given chemical equation follows:
<u>Initial:</u> 4.00
<u>At eqllm:</u> 4.00-2x x x
The expression of 
for above reaction follows:
The partial pressure of pure solids and liquids are taken as 1 in the equilibrium constant expression.
We are given:
Putting values in above expression, we get:
Neglecting the value of x = 718.28 because equilibrium pressure cannot be greater than initial pressure
Partial pressure of 
= 0.0056 atm
Hence, the partial pressure of carbon dioxide at equilibrium is 0.0056 atm
Answer: 8.0 moles
Explanation:
0.6661 moles×12 H≈8.0 moles
Answer:
Option A, 931 Kg
Explanation:
As we know that weight is equal to the product of mass and acceleration due to gravity.
Thus,
m/s2
Substituting the given values in above equation, we get -
Kg
Hence, option A is correct
In a chemical change, the atoms in the reactants rearrange themselves and bond together differently to form one or more new products with different characteristics than the reactants. When a new substance is formed, the change is called a chemical change.
<span>www.middleschoolchemistry.com/lessonplans/chapter6/lesson1</span>
This set up of a conversion table should show you that if you multiply
the grams of BeI2 times .02 moles, it equals <span>5.256 g (your answer) </span>
