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Sergio [31]
3 years ago
5

What happens to a catalyst after a chemical reaction has occurred?

Chemistry
2 answers:
Makovka662 [10]3 years ago
8 0

Answer: Option (d) is the correct answer.

Explanation:

A catalyst is defined as the substance that helps in increasing the rate of a chemical reaction by lowering the activation energy. A catalyst never gets consumed in a chemical reaction.

When a catalyst lowers the activation energy then molecules with much less energy are also able to participate in the chemical reaction. Hence, formation of products occur rapidly and thus rate of reaction increases.

Therefore, we can conclude that the catalyst is unchanged and is separate from the products after a chemical reaction has occurred.

Andre45 [30]3 years ago
5 0
After a chemical reaction has occurred, a catalyst remains unchanged and is separate from the products. D
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GIVING 20 POINTS!! Apply Concepts Two chemists each plan an investigation in which they will combine hydrogen gas with chlorine
Montano1993 [528]

Answer:

Yes, the investigations will reach similar conclusions about the reactivity of H2 and Cl2

Explanation:

1. The law of multiple proportions says that when elements form compounds, the proportions of the elements in those chemical compounds can be expressed in small whole number ratios.  This means that regardless of whether 1000 times more of the products are used, the reactivity of the products is established by the chemical reaction

2. The law of multiple proportions is an extension of the law of definite composition, which states that compounds will consist of defined ratios of elements.

3. A reaction with more reactants will need more care because more products are produced, which can be toxic

4. H2 and Cl2 reactivity does not depend on the quantities but the chemical properties of each compound

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3 years ago
Is glass breaking physical or a chemical
serg [7]

Answer:

<h2>physical </h2>

Explanation:

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3 years ago
Hydrogen gas has a density of 0.090 g/L, and at normal pressure and -1.72 C one mole of it takes up 22.4 L. How would you calcul
BlackZzzverrR [31]

Answer:

n= \frac{m}{ \rho }* \frac{1 mol}{22.4 L}

Explanation:

Assuming that all caculations are at normal pressure and -1.72°C :

n= \frac{m}{ \rho }* \frac{1 mol}{22.4 L}

Where

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A 5.00 L sample of helium expands to 12.0 L at which point the
mina [271]

Answer:

1.73 atm

Explanation:

Given data:

Initial volume of helium = 5.00 L

Final volume of helium = 12.0 L

Final pressure = 0.720 atm

Initial pressure = ?

Solution:

"The volume of given amount of gas is inversely proportional to its pressure by keeping the temperature and number of moles constant"

Mathematical expression:

P₁V₁ = P₂V₂

P₁ = Initial pressure

V₁ = initial volume

P₂ = final pressure

V₂ = final volume  

Now we will put the values in formula,

P₁V₁ = P₂V₂

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P₁ = 8.64 atm. L/5 L

P₁ = 1.73 atm

7 0
3 years ago
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