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Tasya [4]
3 years ago
9

What is generally true about rate over the course of a reaction?. Rate decreases because there are more collisions as the reacti

on progresses.. . Rate increases because there are more collisions as the reaction progresses.. . Rate decreases because the concentration of reactants decreases.. . Rate increases because the concentration of products increases.. . @chmvijay
Chemistry
2 answers:
Vlad1618 [11]3 years ago
8 0
The best answer among the choices listed is the third option. The rate over the course of a reaction <span>decreases because the concentration of reactants decreases. As the concentration of the reactants decreases, there is less particles to form the products therefore less rate.</span>
alisha [4.7K]3 years ago
4 0

Answer: Option (c) is the correct answer.

Explanation:

Rate of reaction is defined as the speed of a chemical reaction.

When there is more number of collisions between reactant molecules then there will be increase in rate of a chemical reaction.

Also, when we increase the concentration of reactant molecules then it means there will be more number of molecules. This will lead to more number of collisions and as a result, there will be increase in the rate of a chemical reaction. Similarly, on decreasing the concentration of reactants there will be decrease in rate of reaction.

Also, when a chemical reaction progresses then it is not necessary that number of collisions will also increase.

Therefore, we can conclude that generally it is true about rate over the course of a reaction that rate decreases because the concentration of reactants decreases.

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Investigate why some element’s symbols derived from their old names.
Gekata [30.6K]

Answer:

you know just in order to bring that nostalgia into chemists minds

Explanation:

3 0
3 years ago
What is the total mass of products formed when 16 grams of ch4?
AlekseyPX
When CH₄ is burnt in excess O₂ following products are formed,

                           CH₄  +  2 O₂     →     CO₂  +  2 H₂O

According to equation 1 mole of CH₄ (16 g) reacts with 2 moles of O₂ to produce 1 mole of CO₂ and 2 moles of H₂O. Hence the products are,

                          1 mole of CO₂  and  2 moles of H₂O

Converting 1 mole CO₂ to grams;
As,
                           Mass  =  Moles × M.mass

                           Mass  =  1 mol ×  44 g.mol⁻¹

                           Mass  =  40 g of CO₂

Converting 2 moles of H₂O to grams,

                           Mass  =  2 mol ×  18 g.mol⁻¹
                         
                           Mass  =  36 g of H₂O

Total grams of products;

                           Mass of CO₂  =  44 g
                    +     Mass of H₂O  =  36 g
                                                  -------------
                           Total              =   80 g of Product

Result:
            80 grams of product
is formed when 16 grams of CH₄ is burnt in excess of Oxygen.
3 0
3 years ago
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Ede4ka [16]

Answer:

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Explanation:

8 0
3 years ago
How molecules of N2 gas can be present in a 2.5 L flask at 50°C and 650 mmHg?
ratelena [41]

Answer:

0.482 ×10²³ molecules

Explanation:

Given data:

Volume of gas = 2.5 L

Temperature of gas = 50°C (50+273 = 323 k)

Pressure of gas = 650 mmHg (650/760 =0.86 atm)

Molecules of N₂= ?

Solution:

PV= nRT

n = PV/RT

n = 0.86 atm × 2.5 L /0.0821 atm. mol⁻¹. k⁻¹. L × 323 k

n = 2.15 atm. L /26.52 atm. mol⁻¹.L

n = 0.08 mol

Number of moles of N₂ are 0.08 mol.

Number of molecules:

one mole = 6.022 ×10²³ molecules

0.08×6.022 ×10²³ = 0.482 ×10²³ molecules

5 0
3 years ago
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Llana [10]

Answer: northern hemisphere

Explanation: I looked it up. Plus I took a test with this question and when the teacher went over the answer i got it right.

3 0
3 years ago
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