Metals is found on the left side of the table and the nonmetals is on the top right.
To identify why a metal measurement was different in the experiments look for the variable that was different in the experiment and analyze how this change affected the results.
<h3>What is an experiment?</h3>
An experiment is a procedure that aims at probing or discovering something. For example, you can test if a plant grows faster/slower by using an experiment.
<h3>What causes different results in similar experiments?</h3>
The most common cause for this situation is that one of the factors or variables is slightly different. For example, if I add 50mL of water to a plant rather than 20mL of water every day this might cause different results.
Based on this, if the metal content was different you should analyze if any of the factors changed in this experiment and find out how this change affected the general results.
Note: This question is incomplete because there is limited information about the experiment; due to this, I answered it based on general knowledge.
Learn more about experiments in: brainly.com/question/13270830
62.5 mL is prepare .
What is molarity?
Molar concentration is a unit of measurement for the concentration of a chemical species, specifically a solute, in a solution, expressed as the amount of substance per unit volume of solution. The most often used unit for molarity in chemistry is the number of moles per litre, denoted by the unit symbol mol/L or mol/dm3 in SI units.
Molarity of the stock solution as 0.100 M
Volume of the dilute solution as 250 mL
Molarity of dilute solution as 0.0250 M
We are required to calculate the Volume of the stalk solution.
Taking the volume and molarity of the stock solution to be V₁ and M₁ respectively, and volume and molarity of the dilute solution to be V₂ and M₂ respectively.
We are going to use the dilution formula;
According to the dilution formula, M₁V₁ = M₂V₂
Rearranging the formula;
V₁ = M₂V₂ ÷ M₁
= (0.025 M × 0.25 L) ÷ 0.100 M
= 0.0625 L
But, 1 L = 1000 mL
V₁ = 62.5 mL
Therefore, the volume of the stock solution is 62.5 mL
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Moles= mass divided by molar mass
Molar mass= 12.01(4) + 1.01(10)
= 58.14g/mol
Moles=14.5g / 58.14g/mol
=0.249
Therefore there are approx 0.249 moles in a 14.5g sample of C4H10