For an ideal gas, evaluate the volume occupied by 0.3 mole of gas.

How many molecules of carbon dioxide and how many molecules of water would be produced from 4 molecules of methane (CH4) reactin

77julia77 [94]

Answer:

4

Explanation:

water would be produced from 4 molecules of methane (CH4) reacting with 8 molecules of oxygen (O2)

7 0

3 years ago

FILL IN THE BLANKWORD BANK (can use more than once): less, increases, decreases, greaterNO2Cl(g)+NO(g)⇌NOCl(g)+NO2(g)1.Disturbin

Jlenok [28]

Explanation:

If we have the following reaction at equilibrium:

aA + bB ⇄ cC + dD

where a, b, c, and d are the stoichiometric coefficients for the reacting species A, B, C, and D. For the reaction at a particular temperature:

Kc=([C]^c *[D]^d)/([A]^a *[B]^b)

where Kc is the equilibrium constant, which holds that for a reversible reaction at equilibrium and a constant temperature, a certain ratio of reactant and product concentrations has a constant value, Kc (the equilibrium constant). Note that although the concentrations may vary, as long as the reaction in in equilibrium and temperatura don't change, the value of K remains constant.

For reactions that have not reached equilibrium, we obtain the reaction quotient (Qc), instead of the equilibrium constant by substituting the initial concentrations into the equilibrium constant expression.

Qc=([Co]^c *[Do]^d)/([Ao]^a *[Bo]^b)

To determine the direction in wich the net reaction will proceed to reach equilibrium, que compare the values of Qc and Kc.

Qc < Kc: To reach equilibrium, reactants must be converted to products (→)
Qc = Kc: The initial concentrations are equilibrium concentrations. The system in at equilibrium.
Qc > Kc: To reach equilibrium, products must be converted to reactants (←)

Solution:

We have the following reaction:

NO2Cl(g)+NO(g)⇌NOCl(g)+NO2(g)

So:

Kc=([NOCl]^1*[NO2]^1)/([NO2Cl]^1 *[NO]^1)

=([NOCl][NO2])/([NO2Cl][NO])

1. In the equation above, [NO2Cl] it's in the denominator, so if we increase it's numericall value by adding NO2Cl decreases Qc to a value less than Kc.

(From the chemical point of view, if we disturb the equilibrium adding NO2Cl (a reactant), to reach equilibrium again the system proceeds from left to right (→) consuming this reactant.)

2. To reach a new state of equilibrium (where Qc = Kc), Qc therefore increases wich means that the denominator of the expression for Qc decreases (in order to increase the denominator as mention above).

3. To accomplish this, the concentration of reageants decreases (reagents are being consumed), and the concentration of prodcuts increases (products are being formed).

4 0

3 years ago

At 218°C, Keq=1.2 x 10^-4 for the equilibrium NH4SH(s) ⇋ NH3(g) + H2S(g). Calculate the equilibrium concentrations of NH3 and H2

maksim [4K]

At 218 °C, solid NH₄SH decomposes to form 0.011 M NH₃ and H₂S, as given by its equilibrium constant.

<h3>What is the equilibrium constant?</h3>

The equilibrium constant (Keq) is the ratio of the product of the concentrations of the products to the product of the concentrations of the reactants, all raised to their stoichiometric coefficients.

Only gases and aqueous species are included.

Step 1. Make an ICE chart.

NH₄SH(s) ⇋ NH₃(g) + H₂S(g)

I 0 0

C +x +x

E x x

Step 2. Write the equilibrium constant.

Keq = 1.2 × 10⁻⁴ = [NH₃] [H₂S] = x²

x = 0.011 M

At 218 °C, solid NH₄SH decomposes to form 0.011 M NH₃ and H₂S, as given by its equilibrium constant.

Learn more about equilibrium here: brainly.com/question/5081082

#SPJ1

3 0

2 years ago

Which grouping of circles, when considered in order from the top to the bottom, best represents the relative size of the atoms o

Nimfa-mama [501]

Answer:

answers number 1

Explanation:

6 0

3 years ago

Are acids harmful to work with.

Yanka [14]

YES. Do I get brainliest now?

8 0

3 years ago

Read 2 more answers