if the pressure of a gas at constant volume is 3.5 atm at 100°c, what will the pressure be if the tempature is changed to 250°c?

natka813 [3]

It represents a chemical change

4 0

3 years ago

Consider an equilibrium (K1) that is established after 10 mL of compound A and 10 mL of compound B are mixed. Now, imagine the e

WARRIOR [948]

The equilibrium constant K₁ = Equilbrium constant K₂.

The equilibrium constant, K, of a reaction, is defined as:

"The ratio between concentration of products powered to their reaction quotient and concentration of reactants powered to thier reaction quotient".

For the reaction:

aA + bB ⇄ cC + dD

The equilibrium constant, K, is:

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

Now, assuming the reaction of the problem is 1:1:

A + B ⇄ C + D

$K = \frac{[C][D]}{[A][B]}$

The concentrations of the reactants are directly proportional to the volume added. Thus, we can assume that concentration = Volume. Replacing for K₁ and K₂:

$K_1 = \frac{[C][D]}{[10mL][10mL]} = K_1 = \frac{[C][D]}{100mL^2}$

In the same way:

$K_2 = \frac{[C][D]}{[1mL][100mL]} = K_2 = \frac{[C][D]}{100mL^2}$

Thus, we can say:

Learn more about chemical equilibrium in:

brainly.com/question/4289021?referrer=searchResults

8 0

3 years ago

For which of the following reactions is ΔH∘rxn equal to ΔH∘f of the product(s)?

nexus9112 [7]

<span>The correct answers are A, B, and D. The ΔHrxn is equal to the ΔHf when the ΔHf of the reactants is zero, and this can only occur when the reactants are pure elements (not compounds) in their natural phase at ambient temperature.

c) Chlorine's natural phase is gaseous, but since it is a liquid in this reaction, ΔHf ≠ 0.

e) CO is a compound, not a pure element.

f) BaCO3 is a compound, not a pure element.</span>

6 0

3 years ago

Read 2 more answers

Contrast the three types of intermolecular forces.

Virty [35]

Answer: The three major types of intermolecular interactions are dipole–dipole interactions, London dispersion forces (these two are often referred to collectively as van der Waals forces), and hydrogen bonds.

Hope this helps............ Stay safe and have a Merry Christmas!!!!!!! :D

4 0

3 years ago

The following redox reaction is conducted with [Al3+] = 0.12 M and [Mn2+] = 1.5 M.

Ronch [10]

Answer:

0.47V

Explanation:

2 Al(s) + 3 Mn2+(aq) → 2 Al3+(aq) + 3 Mn(s)

n= 6 ( six moles of electrons were transferred)

Q= [Red]/[Ox] but [Red]= 1.5M, [Ox] = 0.12 M

Q= 1.5/0.12= 12.5

From Nernst equation:

E= E°cell- 0.0592/n log Q

E°cell= 0.48 V

E= 0.48 - 0.0592/6 log (12.5)

E= 0.47V

6 0

4 years ago