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The Answer rounded with significant figures is:
1.5*10^24 atoms
Answer:
Reaction equilibrium will shift to the left (higher molar volume side of process).
Explanation:
For gas phase reactions, changes in pressure-volume conditions cause a stress on the process equilibrium shifting away from the applied pressure-volume change.
LeChatlier's Principle states for a gas phase reaction at equilibrium ...
if the pressure is increased (volume decreased) the reaction will shift toward the lower molar volume side of the process.
if the pressure is decreased (volume increased) the reaction will shift toward the higher molar volume side of the process.
if the sum of molar volumes of reactants equals the sum of molar volumes of products, changes in pressure-volume conditions will NOT affect the equilibrium stability. Example => H₂(g) + Cl₂(g) ⇄ 2HCl(g) will not be affected by P-V changes as ∑Vm(reactants) = ∑Vm(products).
Explanation:
Generally in normal phase column, inside the column silica gel present is in normal phase and it strongly reacts or combine with more polar ferrocene compounds. Whereas, less polar ferrocene compounds weakly interact with this silica gel.
Hence, on starting with least polar solvent or solvent-mixture the less polar ferrocene compounds will tend to elute first of all because these will weakly interact with the silica gel. Therefore, readily able to move away from the gel.
On increasing the polarity of solvent or solvent mixture, more polar ferrocene compounds will start to elute first. As a result, on changing the solvent polarity we can (from least to more polar) it is possible to get pure products.
But if we start with more polar solvent at first then almost all of the ferrocene compounds will elute leading to poor separation from the column due to which you will end up having a mixture of ferrocene compounds.
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