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2 years ago

1. Which processes are taking place in the system represented by the following equation?

Chemistry

1 answer:

dimaraw [331]2 years ago

4 0

For the first question:
The double directional arrow (<span>→←) shows that the equation is moving at both directions (forward and reverse) simultaneously (at the same time).
So for the equation, two processes are happening at the same time:
1- Carbon monoxide combines with oxygen to form carbon dioxide
2CO2 + O2 ..........> 2CO2
2- Carbon dioxide dissociates to give carbon monoxide and oxygen
2CO + O2 <........ 2CO2

For the second question:
The equilibrium constant can be calculated as shown in the attached picture.
Applying this rule to the given equation, we find that:
k= [(0.01^1)(0.01^1)] / [(0.8^2)] = 1.5625 x 10^-4</span>

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Suppose that in an equilibrium mixture of HCl, Cl2, and H2, the concentration of H2 is 1.0 x 10-11 mol-L-1and that of Cl2 is 2.0

bekas [8.4K]

Considering the definition of Kc, the equilibrium molar concentration of HCl at 500 K is 0.0894 $\frac{mol}{L}$ .

The balanced reaction is:

H₂(g) +Cl₂(g) ⇆ 2 HCl(g)

Equilibrium is a state of a reactant system in which no changes are observed as time passes, despite the fact that the substances present continue to react with each other. In other words, reactants become products and products become reactants and they do so at the same rate.

In other words, chemical equilibrium is established when there are two opposite reactions that take place simultaneously at the same speed.

The concentration of reactants and products at equilibrium is related by the equilibrium constant Kc. Its value in a chemical reaction depends on the temperature and the expression of a generic reaction aA + bB ⇄ cC is

$K_{c} =\frac{[C]^{c} x[D]^{d} }{[A]^{a} x[B]^{b} }$

That is, the constant Kc is equal to the multiplication of the concentrations of the products raised to their stoichiometric coefficients by the multiplication of the concentrations of the reactants also raised to their stoichiometric coefficients.

In this case, the constant Kc can be expressed as:

$K_{c} =\frac{[HCl]^{2} }{[H_{2} ]x[Cl_{2} ] }$

You know that in an equilibrium mixture of HCl, Cl₂, and H₂:

the concentration of H₂ is 1.0×10⁻¹¹ $\frac{mol}{L}$
the concentration of Cl₂ is 2.0×10⁻¹⁰ $\frac{mol}{L}$
Kc=4×10¹⁸

Replacing in the expression for Kc:

$4x10^{18} =\frac{[HCl]^{2} }{[1x10^{-11} ]x[2x10^{-10} ] }$

Solving:

$4x10^{18} =\frac{[HCl]^{2} }{2x10^{-21} }$

$4x10^{18} x 2x10^{-21}=[HCl]^{2}$

$8x10^{-3} =[HCl]^{2}$

$\sqrt[2]{8x10^{-3}} =[HCl]$

0.0894 $\frac{mol}{L}$ = [HCl]

Finally, the equilibrium molar concentration of HCl at 500 K is 0.0894 $\frac{mol}{L}$ .

Learn more:

3 0

2 years ago

The pressure caused by a sample of gas is 2.25 atm. 1 atm is

nexus9112 [7]

Answer:

$0.326\frac{N}{cm^2}$

Explanation:

Hello.

In this case, considering that 1 atm equals 1.01 kPa, we can compute the pressure in kPa first as shown below:

$2.25atm*\frac{1.01kPa}{1atm} =3.26kPa$

Now, we convert kPa to Pa, considering 1 kPa equals 1000 Pa:

$3.26kPa*\frac{1000Pa}{1kPa}=3260Pa$

Now, since Pa is equal to N/m², and 1 m equals 100 cm, the pressure in newton per square centimeter turns out:

$3260\frac{N}{m^2}*(\frac{1m}{100cm})^2 \\\\0.326\frac{N}{cm^2}$

Best regards.

4 0

3 years ago

The second-order rate constant for the dimerization of a protein (P) P + P → P2 is 6.2 × 10−3/M · s at 25°C. Part 1 out of 2 If

siniylev [52]

Answer:

$r=1.59\times 10^{-10}\ M/s$

Explanation:

According to the law of mass action:-

The rate of the reaction is directly proportional to the active concentration of the reactant which each are raised to the experimentally determined coefficients which are known as orders. The rate is determined by the slowest step in the reaction mechanics.

Order of in the mass action law is the coefficient which is raised to the active concentration of the reactants. It is experimentally determined and can be zero, positive negative or fractional.

The order of the whole reaction is the sum of the order of each reactant which is raised to its power in the rate law.

From the reaction given that:-

$P+P\rightarrown P_2$

The expression for the rate is:-

$r=k[P]^2$

Given that;- k= $6.2\times 10^{-3}$ /Ms

[P] = $1.6\times 10^{-4}$ M

Thus,

$r=6.2\times \:10^{-3}\times \:\left(1.6\times \:\:10^{-4}\right)^2\ M/s=1.59\times 10^{-10}\ M/s$

8 0

2 years ago

At 1 atm, how much energy is required to heat 39.0 g of h2o(s at –24.0 °c to h2o(g at 121.0 °c?

earnstyle [38]

Q = mcΔt, q = energy [J] m = mass (of water) [g]; c = specific heat capacity of water [J g⁻¹ K⁻¹/°C⁻¹]; Δt = change in temperature [K/°C]
Δt = 121 - -24 = 145
q = 39 × 4.18 × 145
q = 23637.9 J

4 0

2 years ago

The heat released by one mole of sugar from a bomb calorimeter experiment is 5648 kJ/mol. The balanced chemical reaction equatio

Bogdan [553]

Answer:

The answer to your question is the letter C) 5648 kJ/mol

Explanation:

Data

C₁₂H₂₂O₁₁ + 12 O₂ ⇒ 12 CO₂ + 11 H₂O

H° C₁₂H₂₂O₁₁ = -2221.8 kJ/mol

H° O₂ = 0 kJ / mol

H° CO₂ = -393.5 kJ/mol

H° H₂O = -285.8 kJ/mol

Formula

ΔH° = ∑H° products - ∑H° reactants

Substitution

ΔH° = 12(-393.5) + 11(-285.8) - (-2221.8) - (0)

ΔH° = -4722 - 3143.8 + 2221.8

Result

ΔH° = -5644 kJ/mol

6 0

2 years ago