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1 year ago

The reaction

Chemistry

1 answer:

Aliun [14]1 year ago

7 0

From he calculations, we can see that the total pressure at equilibrium is 21 atm.

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

The term equilibrium constant commonly describes the constant that that shows the extent of conversion of reactants to products.

We have to find the pressure of each gas as follows;

For H2

P = nRT/V = 4.553 /2 × 0.082 × 1000/8.89 L = 21 atm

Using the ICE table;

C(s) + 2H2(g) ⇌ CH4(g)

I 21 atm 0

C -x +x

E 21 - x x

0.263= x/(21 - x )^2

0.263(21 - x )^2 = x

38 - 11x - 0.263x^2 = x

0.263x^2 + 12x - 38 = 0

x=2.97 atm

At equilibrium, we have;

(21 - 2.97) + 2.97 = 21 atm

Learn more about equilibrium constant: brainly.com/question/17960050

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A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O 3 ( g ) + NO ( g )

Aleksandr [31]

Answer:

(a) 7.11x10⁻⁴ M/s

(b) 2.56 mol.L⁻¹.h⁻¹

Explanation:

(a) The reaction is:

O₃(g) + NO(g) → O₂(g) + NO₂(g) (1)

The reaction rate of equation (1) is given by:

$rate = k*[O_{3}][NO]$ (2)

k: is the rate constant of reaction = 3.91x10⁶ M⁻¹.s⁻¹

[O₃]₀ = 2.35x10⁻⁶ M

[NO]₀ = 7.74x10⁻⁵ M

Hence, to find the inital reacion rate we will use equation (2):

$rate = k*[O_{3}]_{0}[NO]_{0} = 3.91 \cdot 10^{6} M^{-1}s^{-1}*2.35\cdot 10^{-6} M*7.74 \cdot 10^{-5} M = 7.11 \cdot 10^{-4} M/s$

Therefore, the inital reaction rate is 7.11x10⁻⁴ M/s

(b) The number of moles of NO₂(g) produced per hour per liter of air is:

t = 1 h

V = 1 L

$\frac{\Delta[NO_{2}]}{\Delta t} = rate$

$\frac{\Delta[NO_{2}]}{\Delta t} = 7.11 \cdot 10^{-4} M/s*\frac{3600 s}{1 h} = 2.56 mol.L^{-1}.h{-1}$

Hence, the number of moles of NO₂(g) produced per hour per liter of air is 2.56 mol.L⁻¹.h⁻¹

I hope it helps you!

5 0

2 years ago

the equilibrium concentration of hydroxide ion in a saturated iron(ii) hydroxide solution is 1.2 x 10^-5 M at a certain temperat

Anit [1.1K]

From the calculation as shpwn in the procedure below, the equilibrium constant of the substance is 6.9 * 10^-15.

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

The equilibrium constant for the solubility of aa solid in solution is called the solubility product Ksp. The Ksp shows the extent to which a solid is dissolved in solution.

Given that;

Fe(OH)2 ⇄Fe^2+ + 2(OH)^-

Ksp = s(2s)^2

We have s as 1.2 x 10^-5 M

Ksp = 4s^3

Ksp = 4( 1.2 x 10^-5 )^3

Ksp = 6.9 * 10^-15

Learn more about Ksp:brainly.com/question/27132799

#SPJ1

8 0

1 year ago

HELPPP!! Which describes one feature of the image formed by a convex mirror?

notka56 [123]

Answer:

The correct answer is - right-side up.

Explanation:

A diverging mirror is a curved mirror that can be bulge outside towards the source of light called a convex mirror or inward away from the source of light called a concave mirror.

A convex mirror is a mirror that forms an image bigger and but right side up or exact as the object direction also called a virtual image. It appears to be bigger than the real object and not upside down as concave mirrors.

8 0

2 years ago

Read 2 more answers

Combustion of 9.511 grams of c4h10 will yield ____ grams of CO2

Flauer [41]

Answer:

$\boxed{28.81}$

Explanation:

We know we will need an equation with masses and molar masses, so let’s gather all the information in one place.

M_r: 58.12 44.01

2C₄H₁₀ + 13O₂ ⟶ 8CO₂ + 10H₂O

m/g: 9.511

1. Moles of C₄H₁₀

$\text{Moles of C$_{4}$H$_{10} $} = \text{ 9.511 g C$_{4}$H$_{10} $} \times \dfrac{\text{1 mol C$_{4}$H$_{10} $}}{\text{ 58.12 g C$_{4}$H$_{10} $}} = \text{0.1636 mol C$_{4}$H$_{10}$}$

2. Moles of CO₂

The molar ratio is 8 mol CO₂:2 mol C₄H₁₀

$\text{Moles of CO}_{2} =\text{0.1636 mol C$_{4}$H$_{10} $} \times \dfrac{\text{8 mol CO}_{2}}{\text{2 mol C$_{4}$H$_{10}$}} = \text{0.6546 mol CO}_{2}$

3. Mass of CO₂

$\text{Mass of CO}_{2} = \text{0.6546 mol CO}_{2} \times \dfrac{\text{44.01 g CO}_{2}}{\text{1 mol CO}_{2}} = \textbf{28.81 g CO}_{2}\\\\\text{The combustion will form $\boxed{\textbf{28.81 g CO}_{2}}$}$

8 0

2 years ago

In a galvanic cell, a spontaneous redox reaction occurs. however, the reactants are separated such that the transfer of electron

jek_recluse [69]

Oxidation is the loss of electrons and corresponds to an increase in oxidation state. Reduction is the gain of electrons and corresponds to a decrease in oxidation state. Balancing redox reactions can be more complicated than balancing other types of reactions because both the mass and charge must be balanced. Redox reactions occurring in aqueous solutions can be balanced by using a special procedure called the half-reaction method of balancing. In this procedure the overall equation is broken down into two half-reactions: one for oxidation and the other for reduction. The half-reactions are balanced individually and then added together so that the number of electrons generated in the oxidation half reaction is the same as the number of electrons consumed in the reduction half-reaction.

4 0

2 years ago