A high school chemistry balance question, high school chemistry balance question, seek detailed expl

The relative molecular mass is equal to the total mass (m) divided by the amount of total matter (n), m is constant, and the amount of matter (n) is constant when the system reaches equilibrium, so the average relative molecular mass is constant. 3。Because it is a transverse container, the volume does not change, and the density = m v, so 3 is false.

4 is also wrong.

Select C for this question

According to the equilibrium constant, the reversible reaction is C(S) H2O(G)--Co(G) H2(G), because C is a solid, if the equilibrium is not reached, the average relative molecular weight of the mixed gas has been changing, and the average relative molecular weight remains unchanged, indicating that the reaction has reached equilibrium, right; v positive (H2O) v inverse (H2), indicating that the reaction has reached equilibrium, right; Although the volume of the container is constant, the mass of the gas is variable, when the density of the gas is constant, it means that the reaction has reached an equilibrium state, right, right; Consume n mol h2 at any time and consume n mol co, false, the correct option is b.

Choose b: The equation is: c(s)+h2o=(reversible)co+h21, n changes before and after the reaction, so 1 is correct.

2. In both directions, the ratio is correct, so 2 is correct.

It is not a pure gas before and after the reaction, so it is all correct.

5. One direction, so 5 is incorrect.

Choose A to join CO, so the balance must be moving in the positive direction.

v = k c(no2)

The reaction rate is only related to the NO2 concentration, and as the reaction progresses, the NO2 concentration decreases, so the positive reaction rate decreases, not increases.

The enthalpy of the product increases, and the enthalpy of the product is not the same as the enthalpy change of the reaction.

Solution: ABCD

From the reaction equation, the mol amount before and after does not change, so the gas pressure before and after the reaction remains unchanged under equilibrium. When CO is added, the amount of reactant increases, but the amount of NO2 does not increase, the reaction speed in the positive direction remains unchanged, and the equilibrium does not move. However, the partial pressure of the CO becomes larger.

Under closed conditions, the pressure of other gases increases. Before and after the reaction, the amount remains the same, the pressure becomes larger, and the equilibrium does not move.

So, ABCD is not right.

The carbon monoxide percentage is not the carbon monoxide concentration, and the concentration will increase as long as it is a gas. After filling Ni(Co)4(g), the percentage will decrease because the reverse reaction will not be 100%.

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.

The relative density of n2 must be h2 (not that I committed suicide), then the average formula is 2*

Next, use the cross method.

no2 (formula) 46

The average N2O4 (formula) is 92

Calculate no2 :n2o4=:

The volume fraction of N2O4 is .

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.