On average, tectonic plates move approximately 3 cm per year; about as fast as your fingernails grow

A reaction mixture that consisted of 0.35 molH2and 1.6 mol I2 was introduced into a 2 L flask and heated. At the equilibrium, 60

Ann [662]

Answer:

The equilibrium constant Kc for the reaction is :

<u></u>

Explanation:

The balanced equation is :

$H_{2}(g)+I_{2}(g)\rightleftharpoons 2HI(g)$

First ,

"At the equilibrium, 60% of the hydrogen gas had reacted"

This means the degree of dissociation = 60% = 0.6

Here we are denoting degree of dissociation by ="x" = 0.6

Now , consider the equation again,

$H_{2}(g)+I_{2}(g)\rightleftharpoons 2HI(g)$

H2 I2 2HI

0.35 1.6 0 (Initial Concentration)

0.35(1 - x) 1.6(1 - x) 2x (At equilibrium)

0.35(1 - 0.6) 1.6(1 - 0.6) 2(0.6)

0.14 0.64 1.2

calculate the concentration of each:

$Concentration =\frac{moles}{Volume(L)}$

$C_{H_{2}}=\frac{0.14}{2}$

$C_{H_{2}}=0.07moles/L$

$C_{I_{2}}=\frac{0.64}{2}$

$C_{I_{2}}=0.32moles/L$

$HI=\frac{1.2}{2}$

$HI=0.6moles/L$

The equilibrium constant for this reaction "Kc" can be written as:

$Kc=\frac{[HI]^{2}}{[H_{2}][I_{2}]}$

$Kc=\frac{0.6^{2}}{0.07\times 0.32}$

$Kc=\frac{0.36}{0.0224}$

$Kc=16.07$

3 0

3 years ago

A chemist dissolves 614. mg of pure hydrochloric acid in enough water to make up 400 mL of solution. Calculate the pH of the sol

tatuchka [14]

Answer:

The pH of the solution is 1.38.

Explanation:

Mass of HCl = 614 mg = 0.614 g

Moles of HCl = $\frac{0.614 g}{36.5 g/ mol}=0.01682 mol$

Concentration of HCl :

$Concentration =\frac{Moles}{\text{Volume of solution in L}}$

On adding 0.01682 moles to 400 mL of water that 0.4 L of water.

$[HCl]=\frac{0.01682 mol}{0.4 L}=0.04205 M$

$HCl(s)+H_2O(l)\rightarrow H_3O^+(aq)+Cl^-(aq)$

1 mole of HCl gives 1 mole of hydronium ion and 1 mole of chloride ions in an aqueous solution.

Then 0.04205 mol/L of HCl will give:

$1\times 0.04205 M =0.04205 mol/L$ of hydronium ions.

$[H_3O^+]=0.04205 M$

$pH=-\log [H_3O^+]$

$pH=-\log [0.04205 M]=1.38$

The pH of the solution is 1.38.

7 0

3 years ago

Student added a strip of aluminium metal in aqueous copper(2)Sulfate but no reaction occured. Suggest a reason why.

kari74 [83]

Answer:

See Explanation

Explanation:

It is a common observation that a strip of aluminium metal in aqueous copper(II)Sulfate does not show any visible reaction. Aluminium is normally expected to displace copper in solution since it is higher than copper in the electrochemical series.

The reason for this is that aluminium forms an oxide film around its surface which prevents reaction with aqueous copper(II)Sulfate. This oxides film protects the aluminium surface such that it is now unable to react with the aqueous copper(II)Sulfate

7 0

2 years ago

Which of these statements is true?

Effectus [21]

I think is number 4

8 0

2 years ago

Make a list of silver current industrial uses. Try to include the approximate annual demand if possible. Create a table to displ

r-ruslan [8.4K]

Answer:

Los usos de la plata son cientos, sobre todo en procesos industriales, comerciales y hasta personales. Su resistencia a la corrosión la hace ideal para la elaboración de recipientes especiales o para recubrir otros metales.

Explanation:

3 0

3 years ago

Read 2 more answers