Reactivity - Reactivity refers to how likely or vigorously an atom is to react with other substances. This is usually determined by how easily electrons can be removed (ionization energy) and how badly they want to take other atom's electrons (electronegativity) because it is the transfer/interaction of electrons that is the basis of chemical reactions.
Metals
Period - reactivity decreases as you go from left to right across a period.
Group - reactivity increases as you go down a group
Why? The farther to the left and down the periodic chart you go, the easier it is for electrons to be given or taken away, resulting in higher reactivity.
Non-metals
Period - reactivity increases as you go from the left to the right across a period.
Group - reactivity decreases as you go down the group.
Why? The farther right and up you go on the periodic table, the higher the electronegativity, resulting in a more vigorous exchange of electron
Answer:
It could be C. Calcuim Chloride.
Explanation:
Answer:
The correct answer to the question is Option E (Strongly retained analytes will give broad peaks).
Explanation:
The other options are true because:
A. Initial temp = 50 °C
Final temp = 270 °C
Differences in temp = 270 - 50 = 220°C
Rate = 10 °C/minute.
So, at 10 °C/minute,
total of 220°C /10 °C = number of minutes required to reach the final temp.
220/10 = 22 minutes
B. A column has a minimum and maximum use temperature. Solutes that are already retained would remain stationary while temperatures are low. This would only change if there is an increase in temperature. Heat transfers more energy to the liquid which would make the solute interact with the column phase.
C. Weakly retained solutes may contain larger molecules, will separate by absorbing into the solvent early in separation making the mobile phase separates out into its components on the stationary phase.
D. Retained solute's vapor pressure is higher at higher temperatures making it possible for particle to escape more from the solute when the temperature is high than when it is low.
of octane had been converted to carbon dioxide CO₂.
<h3>Explanation</h3>
Octane has a molar mass of
1.000 gallon of this fuel would have a mass of 2.650 kilograms or 
, which corresponds to 
of octane.
Octane undergoes complete combustion to produce carbon dioxide and water by the following equation:
An incomplete combustion of octane that gives rise to carbon monoxide and water but no carbon dioxide would consume not as much oxygen:
The mass of the product mixture is 
heavier than that of the octane supplied. Thus 
of oxygen were consumed in the combustion. There are 
of oxygen molecules in 
of oxygen.
Let the number of moles of octane that had undergone complete combustion as seen in the first equation be 
(
). The number of moles of octane that had undergone incomplete combustion through the second equation would thus equal 
.
25 moles of oxygen gas is consumed for every two moles of octane that had undergone complete combustion and 17 moles if the combustion is incomplete.
Therefore 
out of the 23.2 moles of octane had undergone complete combustion to produce carbon dioxide.
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