I need someone to answer this ASAP please!

The order of the layers from the inside of the Earth outwards is:

Ulleksa [173]

I agree with this person

8 0

3 years ago

Suppose that 0.1000 mole each of H2and I2are placed in a 1.000-L flask, stoppered, and the mixture is heated to 425oC. At equili

Katen [24]

Answer: The value of equilibrium constant for the given reaction is 56.61

Explanation:

We are given:

Initial moles of iodine gas = 0.100 moles

Initial moles of hydrogen gas = 0.100 moles

Volume of container = 1.00 L

Molarity of the solution is calculated by the equation:

$\text{Molarity of solution}=\frac{\text{Number of moles}}{\text{Volume}}$

$\text{Molarity of iodine gas}=\frac{0.1mol}{1L}=0.1M$

$\text{Molarity of hydrogen gas}=\frac{0.1mol}{1L}=0.1M$

Equilibrium concentration of iodine gas = 0.0210 M

The chemical equation for the reaction of iodine gas and hydrogen gas follows:

$H_2+I_2\rightleftharpoons 2HI$

Initial: 0.1 0.1

At eqllm: 0.1-x 0.1-x 2x

Evaluating the value of 'x'

$\Rightarrow (0.1-x)=0.0210\\\\\Rightarrow x=0.079M$

The expression of $K_c$ for above equation follows:

$K_c=\frac{[HI]^2}{[H_2][I_2]}$

$[HI]_{eq}=2x=(2\times 0.079)=0.158M$

$[H_2]_{eq}=(0.1-x)=(0.1-0.079)=0.0210M$

$[I_2]_{eq}=0.0210M$

Putting values in above expression, we get:

$K_c=\frac{(0.158)^2}{0.0210\times 0.0210}\\\\K_c=56.61$

Hence, the value of equilibrium constant for the given reaction is 56.61

6 0

3 years ago

HELP PLEASE PLEAES PLAESE

mamaluj [8]

Explanation:

Filter the sand and sea salt from water.

Add water and wait for sea salt to dissolve.

Filter sand from salt water.

Heat and evapourate salt water for salt.

7 0

3 years ago

Read 2 more answers

15.

Vladimir [108]

Answer:

Mass = 1.84 g

Explanation:

Given data:

Total pressure = 3.44 atm

Volume of flask = 9.62 L

Temperature = 63°C = 63+273.15K = 336.15 K

Mass of CO₂ = 12.5 g

Mass of hydrogen = ?

Solution:

Number of moles of CO₂:

Number of moles = mass/molar mass

Number of moles = 12.5 g/ 44 g/mol

Number of moles = 0.28 mol

Pressure of CO₂:

PV = nRT

R = general gas constant = 0.0821 atm.L/mol.K

P = 0.28 mol × 0.0821 atm.L/mol.K × 336.15 K / 9.62 L

P = 7.73 atm.L/ 9.62 L

P = 0.8 atm

Total pressure = Partial pressure of CO₂ + Partial pressure of H₂

3.44 atm = 0.8 atm + P(H₂)

P(H₂) = 3.44 atm - 0.8 atm

P(H₂) = 2.64 atm

Number of moles of hydrogen:

PV = nRT

2.64 atm × 9.62 L = n × 0.0821 atm.L/mol.K × 336.15 K

25.39 atm.L = n × 27.59atm.L/mol

n = 25.39 atm.L / 27.59atm.L/mol

n = 0.92 mol

Mass of hydrogen:

Mass = number of moles × molar mass

Mass = 0.92 mol × 2 g/mol

Mass = 1.84 g

5 0

3 years ago

3. Hexane (C6H-2) is combusted in oxygen

Lapatulllka [165]

Answer:

a) 9.5 moles of Oxygen

b) 1.029 × 10²⁵ Molecules

Explanation:

The balance chemical equation for said reaction is as follow:

2 C₆H₁₄ + 19 O₂ → 12 CO₂ + 14 H₂O

A)

According to equation,

2 moles of C₆H₁₄ are reacted with = 19 moles of O₂

So,

1 moles of C₆H₁₄ will react with = X moles of O₂

Solving for X,

X = 19 moles × 1 mole / 2 moles

X = 9.5 moles of Oxygen

B)

For this part first calculate moles of hexane as;

Moles = Mass / M.Mass

Moles = 245.5 g / 86.18 g/mol

Moles = 2.84 mole of Hexane

Secondly, find the number of moles of CO₂ as,

According to equation,

2 moles of C₆H₁₄ produced = 12 moles of CO₂

So,

2.84 moles of C₆H₁₄ will produce = X moles of CO₂

Solving for X,

X = 12 moles × 2.84 mole / 2 moles

X = 17.09 moles of CO₂

Lastly, calculate the number of molecules of CO₂ as,

Number of Molecules = Moles × 6.022 × 10²³ molecules/mole

Number of Molecules = 17.09 moles × 6.022 × 10²³ molecules/mole

Number of Molecules = 1.029 × 10²⁵ Molecules

4 0

3 years ago