An inorganic chemistry topic on chemical equilibrium. Freshman year Please advise!! ）

At t = 1073K and 1473K, carbon is solid, so only CO and CO2 are gases.

1) When the total pressure of t = 1073k is 260kpa, with CO2, the CO content is P(CO2)=P(total)*

p(co)=p(total)-p(CO2)=or =p(total)*equilibrium constant kp1=(p(co)p0) 2 (p(co2) p0)=(2)t=1473k, the total pressure is 232kpa, and p(co2)=p(total)* can be obtained with CO2

p(co)=p(total)-p(co2)=

The equilibrium constant kp2=(p(co) p0) 2 (p(co2) p0)=(ln(kp2 kp1)=(δrhm0 r)(1 t1-1 t2)r is the constant =,t1=1073,t2=1473,kp1=,kp2=,δrhm0 refers to the standard molar reaction constant, that is, the molar heat effect of the reaction, which is solved by substituting each value for the above equation.

rhm0=55758j/mol=

This question is about the calculation of the precipitation pH.

After mixing in equal volumes, c(mg2+)=

Ksp= of mg(OH)2

So c(oh-)=

POH = pH = concentration of ammonia added now.

kb=c kb > 500, which can be calculated in a simplified form, c(oh-)=root(ck)=poh=

ph= >

So there is a precipitate of Mg(OH)2

If no precipitation is generated, the addition of NH4Cl makes the solution pH <=, so it is a critical value.

This becomes a buffer solution.

pH = pka-logc (acid) c (base).

Ka=KW KB at this time

So, n(NH4Cl) = ie.

KB= of NH3

Then c(NH4+)*c(oh-)=c(NH3·H2O)*kb=because c(oh-)=

So C(OH-)=C(Mg2+)*C(OH-)*C(OH-)=>ksp(Mg(OH)2).

There is a precipitation generated.

When there is no precipitation precipitation, c(oh-)*c(oh-)=ksp(mg(oh)2) c(mg2+)=

c(oh-)=

c(nh4+)=kb*c(nh3)/c（oh-）=n(nh4cl)=n(nh4+)=c(nh4+)*v=m(nh4cl)=m*n(nh4cl)=

In the case of isotherm of the fiber, p1v1=p2v2

For example, the partial pressure of hydrogen is imitated. p2=

Thermodynamics is expressed in terms of standard equilibrium constants, and gases must be phased.

For the ratio of the standard pressure is brought into the expression:

ph2o p0, instead of the saturated vapor pressure with water, gives the pressure of the water vapor at equilibrium in this reaction, and then with .

The saturation vapor pressure of water at this temperature is smaller.

It's not right-to-right, it's left-to-right. Practical exercises.

The standard equilibrium constant of this question is k0=(ph2o p0) 4, and the partial pressure of water vapor at the time of reaction equilibrium can be calculated ph2o=162pa, which is less than the saturated vapor pressure of water, so the process that occurs should be srcl2·2h2o water absorption deliquescent. I think that the calculated partial pressure of water vapor does not need to be divided by the saturated vapor pressure, and it can be directly compared.

When the acid and salt concentrations are equal, the buffering efficiency of the buffer is the highest, and the greater the difference in the ratio, the lower the buffering efficiency.

According to this principle, the greater the concentration of the buffer solution excluding AB (the general effective buffer range of the buffer is PK 1pH), the stronger the buffering capacity. (It is easy to understand that two solutions of the same volume are naturally strong with more solutes).

So exclude c. Then choose D

There is no calculation process for this question. Just take a look. I can't calculate it.

solution, 1The material ratio at the first equilibrium is: 05, and the equilibrium constant is 5*5 2=decomposition rate of PCL5=

2.Let the decomposition rate of the second time be a, .,At the time of equilibrium, the material ratio is 7-7a: 7a: 7a+1, and the solution is a=

3.If. The decomposition rate of phosphorus pentachloride is 7-7b:7b:7b+1 when the material ratio is balanced

Same as above, b=

Through comparison, it is obtained that at the same temperature, the conversion rate of the gas reaction of a given volume is not related to the process, but only to the proportion of the feeding.