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3 years ago

Place an X next to each action that would most likely increase the reaction rate.

Chemistry

1 answer:

Shtirlitz [24]3 years ago

5 0

Answer:

2.__ Dissolving two solids in water before mixing them together.

4.__ Grinding a solid into fine particles.

5.__ Adding an enzyme catalyst.

Explanation:

The rate of reaction is the measure of the speed of a chemical reaction.

Some factors affects the rate of reactions such as pressure, temperature, concentration, surface area, presence of catalyst.

Reactions in liquid medium are much faster than those between solids because there is a flow of substances. As they come in contact with one another, collision begins to take place.
Grinding a solid into fine particles increases the surface area. An increase in surface area increases the rate of reaction.
Adding an enzyme catalyst lowers the activation energy and reduces the energy barrier that must be overcome before a reaction takes place.

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3 years ago

Read 2 more answers

A sample of hydrogen gas has an initial pressure of 2.86 atm and an initial volume of 8472 mL If the volume of the

Oliga [24]

<h3>Answer:</h3>

Gas law : Boyle's law

New pressure: 66.24 atm

<h3>Explanation:</h3>

Concept tested: Gas laws (Boyle's law)

We are given,

Initial pressure, P₁ = 2.86 atm
Initial volume, V₁ = 8472 mL
New volume, V₂ IS 365.8 mL

We need to determine the new pressure, P₂

According to Boyle's law , the volume of a fixed mass of a gas and the pressure are inversely proportional at constant temperature.

That is, $P\alpha \frac{1}{V}$
This means , PV = k (constant)
Therefore; P₁V₁ = P₂V₂

Rearranging the formula, we can get the new pressure, P₂

P₂ = P₁V₁ ÷ V₂

= (2.86 atm × 8472 mL) ÷ 365.8 mL

= 66.24 atm

Therefore, the new pressure is 66.24 atm

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3 years ago

How moles are in 45.7g of CH3?

miskamm [114]

first find the atomic weight of CH3 which would be

atomic weight: 12.011 (3×1.008) = 36.32 g/mol

then find the moles in the given mass

36.32 ÷ 45.7 = 0.794

I HOPE I'M NOT WRONG I HAVENT DONE CHEM IN SO LONG

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3 years ago