At a particular temperature, a 2.00-L flask at equilibrium contains

$$2.80 \times 10 ^ { - 4 } \text { mole of } N _ { 2 }, 2.50 \times 10 ^ { - 5 } \text { mole of } \mathrm { O } _ { 2 } , \\ \text { and } 2.00 \times 10 ^ { - 2 } \text { mole of } \mathrm { N } _ { 2 } \mathrm { O }$$

Calculate K at this temperature for the reaction

$$2 \mathrm { N } _ { 2 } ( g ) + \mathrm { O } _ { 2 } ( g ) \rightleftharpoons 2 \mathrm { N } _ { 2 } \mathrm { O } ( g )$$

If

$$\left[ \mathrm { N } _ { 2 } \right] = 2.00 \times 10 ^ { - 4 } \mathrm { M } , \left[ \mathrm { N } _ { 2 } \mathrm { O } \right] = 0.200 \mathrm { M } , \mathrm { and } \left[ \mathrm { O } _ { 2 } \right] =0.00245 M$$

does this represent a system at equilibrium?

Explain the following statement: The smallest particles unique to a compound cannot be atoms.

How can you use probability to make decisions$?$

Solve the equation. Check your solution. 44 = t - 72

Write equilibrium constant expression for the following reaction N$_2$(g) + 3H$_2$ $\rightleftharpoons$ 2NH$_3$(g)

At

$$327^\circ C,$$

the equilibrium concentrations are

$$| \mathrm { CH } _ { 3 } \mathrm { OH } ] =0.15 M,$$

[CO] = 0.24 M, and

$$\left[ \mathrm { H } _ { 2 } \right] = 1.1\ \mathrm { M }$$

for the reaction

$$\mathrm { CH } _ { 3 } \mathrm { OH } ( g ) \rightleftharpoons \mathrm { CO } ( g ) + 2 \mathrm { H } _ { 2 } ( g )$$

Calculate

$$K_p$$

at this temperature.

A sample of solid ammonium chloride was placed in an evacuated chamber and then heated, causing it to decompose according to the following reaction: $\mathrm { NH } _ { 4 } \mathrm { Cl } ( s ) \rightleftharpoons \mathrm { NH } _ { 3 } ( g ) + \mathrm { HCl } ( g ).$ In a particular experiment, the equilibrium partial pressure of $\mathrm { NH } _ { 3 } ( g )$ in the container was 2.9 atm. Calculate the value of $K _ { \mathrm { p } }$ for the decomposition of $\mathrm { NH } _ { 4 } \mathrm { Cl } ( s )$ at this temperature.

At

$$1285 ^ { \circ } \mathrm { C }$$

the equilibrium constant for the reaction

$$\mathrm { Br } _ { 2 } ( g ) \rightleftharpoons 2 \mathrm { Br } ( g ) \text { is } K _ { c } = 1.04 \times 10 ^ { - 3 }$$

A 0.200-L vessel containing an equilibrium mixture of the gases has 0.245 g

$$\mathrm { Br } _ { 2 } ( g )$$

in it. What is the mass of Br(g) in the vessel?

Explain the difference between K, $K_p,$ and Q.

Evaluate the limit of the following sequences or state that the limit does not exist.

$$a _ { n } = \cos \left( 0.99 ^ { n } \right) + \frac { 7 ^ { n } + 9 ^ { n } } { 63 ^ { n } }$$

At a particular temperature, K = 3.75 for the reaction

$$\mathrm { SO } _ { 2 } ( g ) + \mathrm { NO } _ { 2 } ( g ) \rightleftharpoons \mathrm { SO } _ { 3 } ( g ) + \mathrm { NO } ( g )$$

If all four gases had initial concentrations of 0.800 M, calculate the equilibrium concentrations of the gases.

For the reaction

$$\mathrm { H } _ { 2 } ( g ) + \mathrm { Br } _ { 2 } ( g ) \rightleftharpoons 2 \mathrm { HBr } ( g )$$

$$K _ { \mathrm { p } } = 3.5 \times 10 ^ { 4 }$$

at 1495 K. What is the value of

$$K_p$$

for the following reactions at 1495 K?

$$2 \mathrm { HBr } ( g ) \rightleftharpoons \mathrm { H } _ { 2 } ( g ) + \mathrm { Br } _ { 2 } ( g )$$

Answer the following.

Consider the following generic reaction:

$$2 \mathrm{~A}_2 \mathrm{~B}(g) \rightleftharpoons 2 \mathrm{~A}_2(g)+\mathrm{B}_2(g)$$

Some molecules of $\mathrm{A}_2 \mathrm{~B}$ are placed in a 1.0-L container. As time passes, several snapshots of the reaction mixture are taken as illustrated below.

Which illustration is the first to represent an equilibrium mixture? Explain. How many molecules of $\mathrm{A}_2 \mathrm{~B}$ were initially placed in the container?

Describe why it is important to take measurements that are both accurate and precise: