The question is incomplete, here is the complete question:
Consider the following chemical reaction: H₂ (g) + I₂ (g) ⇔ 2HI (g) At equilibrium in a particular experiment, the concentrations of H₂, I₂, and HI were 0.15 M, 0.033 M and 0.55 M respectively. The value of Keq for this reaction is
<u>Answer:</u> The value of for the given reaction is 61.11
<u>Explanation:</u>
Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as
For a general chemical reaction:
The expression for is written as:
For the given chemical equation:
The expression of for above equation follows:
We are given:
Putting values in above expression, we get:
Hence, the value of for the given reaction is 61.11
Lithium dichromate - Li2Cr2O7
Answer:
Explanation:
For reaction stoichiometry problems like this, convert given data to moles and set up a ratio expression that relates to the balanced equation. That is ...
Given Rxn => Mg(OH)₂ + 2HCl => 2H₂O + MgCl₂
Given mass => 3.26g = (3.26g)/(58g/mol) = 0.056 mole Mg(OH)₂
If from equation 1 mole Mg(OH)₂ reacts with 2 moles HCl
then, 0.056 mole Mg(OH)₂ reacts with x moles HCl
Setting up ratio and proportion expression ...
=> (1 mole Mg(OH)₂) /(0.056 mole Mg(OH)₂) = (2 moles HCl)/x
=> x = [2(0.056)/(1)] mole HCl neutralized = 0.112mole HCl (36g/mol)
= 4.05 grams of HCl neutralized.