A chemistry question for sophomore chemical equilibrium, a question for sophomore chemical equilibri

The answer is B2SO2(G) + O2(G) = 2SO3(G) at some point:

The positive direction reacts exactly 0 0

The reverse direction completely reacts to 0

We all know that the reversible reaction cannot be carried out completely, first of all, when the SO3 in A and DC is 2SO2(g)+O2(G) = 2SO3(G), the SO3 has a reverse reaction, so the SO2 increases accordingly.

b 2SO2(G) + O2(G) = 2SO3(G) at some time:

The positive direction reacts exactly 0 0

The reverse direction completely reacts to 0

So the option for a complete reaction to occur is denied, a d

Option C is also rejected because it does not meet the amount and concentration of the substance in its initial state.

B can be ruled out first because this reaction is a reversible reaction, and it is impossible for a complete reaction to occur in a certain direction, so AD can be ruled out first

However, it is not possible to reduce the concentration of reactants and products in C at the same time!

a, d is wrong, because the reaction is reversible, and the reaction cannot be carried out to the end c, false, according to the number of atoms before and after the reaction, the number of atoms should be conserved, that is, the amount of their matter should be the same, at a certain time: n(s) (v (the container is in volume) according to the conservation principle: the equilibrium should also be x v, but the answer in c is only x v

b Correct.

As the temperature increases, the conversion rate of b increases; It can be obtained that the mass fraction of C in the mixed system decreases when the pressure is reduced. M+N>P can be obtained If B is added (keeping the volume of the system unchanged), the conversion rate of A increases, the conversion rate of B decreases, and the moment B is added, due to the increase of B concentration, the forward reaction rate becomes larger, the reverse reaction rate remains unchanged, and the equilibrium moves positively, so that the concentration of A decreases, and the concentration of B is still greater than the original concentration. So the conversion rate of A increases, and the conversion rate of B decreases.

If B is a colored substance, and both A and C are colorless, the color of the mixture becomes darker when C is added (the volume is unchanged).

Because the addition of C causes the equilibrium to move in reverse, the concentration of B is increased, and the color becomes darker.

While maintaining the constant pressure in the container, the equilibrium shifts to the left (left, right, or unchanged) when neon gas is flushed.

Because the pressure in the container is kept constant, the total volume of neon gas will increase, and the partial pressure of each gas will decrease (equivalent to reducing the pressure), so the equilibrium will move in the direction of the expansion of the gas volume.

A should be greater than B, because A is constant pressure, N2O4=2NO2, the pressure of A is unchanged, so the volume becomes larger, so the concentration of N2O4 in A is smaller, but N2O4 in B is only consumed, so the change is small.

The concentration of N2O4 is small.

Because the degree of reaction is smaller, the energy absorbed by A is also small.

It should be right. We are also new to the +1 class.

Because A is constant pressure, nitrogen tetroxide will be converted into nitrogen dioxide, the pressure will become larger, the volume of nail will become larger, and the concentration of nitrogen tetroxide will become smaller, so that the reaction time will increase, so it is greater than 60s.

Because the volume increases, the reaction proceeds in the direction of the positive reaction, and the concentration of nitrogen dioxide becomes larger and the concentration of nitrogen tetroxide decreases.

3a(g)+b(g) == 4c(g) start 3 1

Transform balance. Equivalent to 4c(g) == 3a(g)+b(g) starting with 4

Transform balance. The conversion rate is:

Then add AMOLC and transform 80%, and the remaining 20% is plus the original is.

a.It can be assumed that the first reaction generates x mol co, and the second reflects that y mol co is consumed

x-y=x+y=

Solving the equation yields that the first reaction generates 1mol co, which consumes another mol and the conversion rate is 90%.

b.From the above option, c(CO2)= mol is obviously incorrect.

c.There is no information about water vapor and the relative molecular mass of the gas cannot be solved.

d.By Le Chatle's principle, the volume is reduced, and the first equilibrium is shifted to the left (the direction of volume reduction) so that the second equilibrium is also shifted to the left (the direction of reactant increase).