Decreasing the temperature in the reaction vessel keep this reaction from shifting to form more of the product.
As we know that rate of reaction is directly proportional to the concentration of the reactant.
If we increase the concentration of H2 then the rate of reaction increases. So, we keep it constant. Therefore this option is wrong.
By removing the H₂O from the reaction vessel as it almost make no change in the reaction. This can be pursuited the reaction in which product again converted into product.
By increasing the temperature we increases the rate of reaction and equilibrium shift in the forward direction.
Thus, we concluded that by decreasing the temperature in the reaction vessel keep this reaction from shifting to form more of the product.
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<span>An organism that contains chloroplasts is able to produce food by the process of
"Photosynthesis"
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</span>
Answer:
Bohr's model explains the spectral lines of the hydrogen atomic emission spectrum. While the electron of the atom remains in the ground state, its energy in uncharged. When the atom absorbs one or more quanta of energy, the electron moves from the ground state orbit to an excited stats orbit that is further away. Energy levels are designated with the variable n. The ground state is n =1, the first excited state is n = 2, and so on. The energy that is gained by the atom is equal to the difference in energy between the two energy levels. When the atom relaxes back to a lower energy state, it releases energy that is again equal to the difference in energy of the two orbits.
Answer:
( About ) 0.03232 M
Explanation:
Based on the units for this reaction it should be a second order reaction, and hence you would apply the integrated rate law equation "1 / [X] = kt + 1 / [
]"
This formula would be true for the following information -
{ = the initial concentration of X, k = rate constant, [ X ] = the concentration after a certain time ( which is what you need to determine ), and t = time in minutes }
________
Therefore, all we have left to do is plug in the known values. The initial concentration of X is 0.467 at a time of 0 minutes, as you can tell from the given data. This is not relevant to the time needed in the formula, as we need to calculate the concentration of X after 18 minutes ( time = 18 minutes ). And of course k, the rate constant = 1.6
1 / [X] = ( 1.6 )( 18 minutes ) + 1 / ( 0.467 ) - Now let's solve for X
1 / [X] = 28.8 + 1 / ( 0.467 ),
1 / [X] = 28.8 + 2.1413...,
1 / [X] = 31,
[X] = 1 / 31 = ( About ) 0.03232 M
Now for this last bit here you probably are wondering why 1 / 31 is not 0.03232, rather 0.032258... Well, I did approximate one of the numbers along the way ( 2.1413... ) and took the precise value into account on my own and solved a bit more accurately. So that is your solution! The concentration of X after 18 minutes is about 0.03232 M
