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densk [106]
3 years ago
14

Yet another reaction has an equilibrium constant kc=4.32×105 at 25 ∘c. it is an exothermic reaction, giving off quite a bit of h

eat while the reaction proceeds. if the temperature is raised to 200 ∘c , what will happen to the equilibrium constant? the equilibrium constant will yet another reaction has an equilibrium constant at 25 . it is an exothermic reaction, giving off quite a bit of heat while the reaction proceeds. if the temperature is raised to 200 , what will happen to the equilibrium constant?
Chemistry
2 answers:
Tatiana [17]3 years ago
8 0
The equilibrium constant will decrease.
when this reaction is an exothermic reaction, SO we can assume heat as a product of that reaction.

when Kc = concentration of product/concentration of reactants

So when the temperature and heat increase the reaction will go in the direction which decreases the heat and achieves equilibrium again. So it will go leftwards to decrease the products. and when the products decrease the Kc will decrease. 

Kitty [74]3 years ago
4 0
<span><u><em>Answer:</em></u>
The equilibrium constant will decrease

<u><em>Explanation:</em></u>
<u>The equilibriuc constant (Kc) can be calculated as follows:</u>
Kc = </span>\frac{concentration_o_fproducts}{concentration_o_freactants}<span>

Now, the given equation is an exothermic reaction. This means that <u>heat is s product.</u>

If we increase the amount of heat, the system will no longer be at equilibrium. This equilibrium will <u>shift to the left creating more reactants</u> in order to balance the system and be reach equilibrium again.

By this, we can note that the <u>concentration of reactants in the system will increase</u> which means that the equilibrium constant will decrease.

Hope this helps :)</span>
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Balance the following reaction. A coefficient of "1" is understood. Choose option "blank" for the correct answer if the coeffici
irina1246 [14]

Answer:

                     2 C₄H₁₀ + 13 O₂ → 8 CO₂ + 10 H₂O

Explanation:

Step 1: Write the unbalanced chemical equation,

                          C₄H₁₀ + O₂ → CO₂ + H₂O

Step 2: Balance Carbon  Atoms;

As there are 4 carbon  atoms on left hand side and 1 carbon atoms on right hand site therefore, to balance them multiply CO₂ on right hand side by 4 i.e.

                            C₄H₁₀ + O₂ → 4 CO₂ + H₂O

Step 3: Balance Hydrogen Atoms;

There are 10 hydrogen atoms on left hand side and 2 hydrogen atom on right hand site therefore, to balance them multiply H₂O on left hand side by 5 i.e.

                            C₄H₁₀ + O₂ → 4 CO₂ +  5 H₂O

Step 4: Balance Oxygen Atoms:

Now there are 2 oxygen atoms in reactant side and 13 in product side. So, multiply O₂ by 6.5 i.e.

                            C₄H₁₀ + 6.5 O₂ → 4 CO₂ + 5 H₂O

Step 5: Remove fraction coefficients as,

Multiply whole equation by 2 to get rid of fractions i.e.

                            2 C₄H₁₀ + 13 O₂ → 8 CO₂ + 10 H₂O

7 0
2 years ago
During the experiment a student precipitated and digested the BaSO4. After allowing the precipitate to settle, they added a few
OlgaM077 [116]

Answer:

Incomplete precipitation of barium sulfate

Explanation:

The student has precipitated and digested the barium sulfate on his/her side. But on the addition of BaCl_2 in the solution, the solution become cloudy. This happened because incomplete precipitation of barium sulfate by the student. When BaCl_2 is added, there are still sulfate ions present in the solution with combines with BaCl_2 and forms BaSO_4 and the formation of this precipitate makes the solution cloudy.

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3 years ago
Filtration definition 
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Answer:

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8 0
3 years ago
Read 2 more answers
A solution containing 0.102 g of an unknown compound dissolved in 100. mL of water has an osmotic pressure of 28.1 mmHg at 20.°C
IrinaVladis [17]

Answer:

MM = 680g / mol

Explanation:

Hello! To calculate the molar mass of the compound (g / mol), I first have to calculate the molarity.

Molarity can be calculated from the osmotic pressure equation.

op = M * R * T

op = osmotic pressure = 28.1mmHg * (1 atm / 760mmHg) = 0.037atm

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T = temperature (K) = 20 ° C + 273.15 = 293.15K

M (mol / L) = op / R * T

M = 0.037atm / ((0.082 (atm * L) / (K * mol)) * 293.15K) = 0.0015mol / L

As I have the volume = 100ml * (1L / 1000ml) = 0.1L

I can calculate the amount of moles

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4 0
3 years ago
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Black_prince [1.1K]

Answer:

\large \boxed{\text{41.2 cm}^{3}}

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