Answer:
It is necessary because Trans-cinnamic is a limiting reagent in the mixture reaction while Bromine is the excess reagent
Explanation:
It is necessary to maintain excess bromine in the reaction mixture because Bromine is the excess reagent in the reaction mixture and if it's quantity is less it would consume the limiting reagent ( Trans-cinnamic ) completely . hence Bromine should maintain excess quantity in the reaction mixture
Lines in one spectral series can overlap lines in another is rydberg
In several chemical elements, the Rydberg formula is used to compute the wavelengths of spectral lines.
<h3>
What causes lines in a line spectrum?</h3>
A spectral line is similar to a fingerprint in that it can be used to identify the atoms, elements, or molecules in a star, galaxy, or cloud of interstellar gas. When we use a prism to split incoming light from a heavenly source, we often observe a rainbow of colours crossed by definite lines. It's worth noting that spectral lines can appear in other parts of the electromagnetic spectrum, however we can't use a prism to assist us identify them.
Emission lines are distinct coloured lines that appear on a black backdrop and correspond to certain wavelengths of light emitted by an item.
Absorption lines are visible as black bars.
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Relative means you take the required amount from the actual amount which gives you the excess or abundance, its relative because you compare it to the required amount.
The percent abundance is the relative abundance as a percentage of the required amount.
Therefore % abundance= (abundance/required amount) X 100
The key difference is that percentages are standardised as a number out of 100 which allows you to compare them with other percentages without any calculations.
Hope that helps.
The balanced chemical
reaction will be:
2H2O = 2H2 + O2
<span>We are given the amount of water used in the decomposition reaction. This will be our
starting point.</span>
<span>17.0 g H2O</span> (1 mol H2O/ 18.02 g H2O) (1 mol O2/2
mol <span>H2O</span>) ( 32.00 g O2/1mol O2) = 15.09 g O2
Percent yield = actual yield / theoretical yield x 100
<span>Percent yield =10.2 g / 15.09 g
x 100</span>
Percent yield = 67.58%
A. As pressure on the gas increases, the volume and temperature will both decrease
