Also what happens if you decrease NOCL

Galina-37 [17]

Answer:

The reaction isn't yet at equilibrium. The overall reaction will continue to move in the direction of the products.

Assumption: this system is currently at $\rm 900^{\circ}C$ .

Explanation:

One way to tell whether a system is at its equilibrium is to compare its reaction quotient $Q$ with the equilibrium constant $K_c$ of the reaction.

The equation for $Q$ is quite similar to that for $K_c$ . The difference between the two is that $K_c$ requires equilibrium concentrations, while $Q$ can be calculated even when the system is on its way to equilibrium.

For this reaction,

$\displaystyle Q = \rm \frac{[CS_2]\cdot [H_2]^{4}}{[CH_4]\cdot [H_2S]^{2}}$ .

Given these concentrations,

$\displaystyle Q = \rm \frac{[CS_2]\cdot [H_2]^{4}}{[CH_4]\cdot [H_2S]^{2}} =\frac{1.51\times (1.08)^{4}}{1.15\times (1.20)^{2}} \approx 1.72$ .

The question states that at $\rm 900^{\circ}C$ , $K_c = 3.59$ . Assume that currently this system is also at $\rm 900^{\circ}C$ . (The two temperatures need to be the same since the value of $K_c$ depends on the temperature.)

It turns out that $Q = K_c$ . What does this mean?

First, the system isn't at equilibrium.
Second, if there's no external changes, the system will continue to move towards the equilibrium. Temperature might change. However, eventually $Q$ will be equal to $K_c$ , and the system will achieve equilibrium.

In which direction will the system move? At this moment, $Q < K_c$ . As time proceeds, the value of $Q$ will increase so that it could become equal to $K_c$ . Recall that $Q$ is fraction.

$\displaystyle Q = \rm \frac{[CS_2]\cdot [H_2]^{4}}{[CH_4]\cdot [H_2S]^{2}}$

When the value of $Q$ increases, either its numerator becomes larger or its denominator becomes smaller, or both will happen at the same time. However,

Concentrations on the numerator of $Q$ are those of the products;
Concentrations on the denominator of $Q$ are those of the reactants.

As time proceeds,

the concentration of the products will increase, while
the concentration of the reactants will decrease.

In other words, the equilibrium will move towards the products.

3 0

4 years ago

a weight loss supplement i advertised in several popular beauty and and fashion magazines the advertisements claim that the supp

inessss [21]

to provide scientific evidence and results

8 0

3 years ago

What will happen if you weighed out a quantity of beans

Ostrovityanka [42]

Answer:

When we weigh beans in this mass ratio, we must obtain the same number of beans.Explanation:

Nothing will happen

3 0

3 years ago

Calculate the maximum concentration (in m) of silver ions (ag+) in a solution that contains 0.025 m of co32-. the ksp of ag2co3

Helen [10]

Equilibrium equation is

Ag2CO3(s) <---> 2 Ag+(aq) + CO32-(aq) 

From the reaction equation above, the formula for Ksp: 

Ksp = [Ag+]^2 [CO32-] = 8.1 x 10^-12 
You know [CO32-], so you can solve for [Ag+] as: 
(8.1 x 10^-12) = [Ag+]^2 (0.025) 
[Ag+]^2 = 3.24 x 10^-10 
[Ag+] = 1.8 x 10^-5 M

5 0

3 years ago

Select the statements that are true about electronegativity between elements,

s2008m [1.1K]

Answer:

a

Explanation:

if the difference is over 1.7, an ionic bond will form

4 0

3 years ago