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4 years ago

Which law is known as the law of action-reaction

Chemistry

2 answers:

kakasveta [241]4 years ago

6 0

Answer:

Newton's third law

Explanation:

The law of action-reaction (Newton's third law) explains the nature of the forces between the two interacting objects. According to the law, the force exerted by object 1 upon object 2 is equal in magnitude and opposite in direction to the force exerted by object 2 upon object 1.

shusha [124]4 years ago

6 0

Answer:

The law that relates action to reaction is the Newton's third law of motion.

Explanation:

Newton's third law of motion states that for every action there is an equal and opposite reaction.

Action-reaction force pairs make it possible for fishes to swim, birds to fly, cars to move etc,

Furthermore, take for example, While driving down the road, a firefly strikes the windshield of a car (Action) and makes a quite obvious mess in front of the face of the driver (Reaction) i.e The firefly hit the car and the car hits the firefly.

The statement above means that in every interaction, there is a pair of forces acting on the two interacting objects in this case, the car and fly. The size of the force on the car equals the size of the force on the fly. These two forces are called action and reaction forces and are the subject of Newton's third law of motion.

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A major component of gasoline is octane (C8H18). When octane is burned in air, it chemically reacts with oxygen gas (O2) to prod

Molodets [167]

Answers:

8.70 g

Step-by-step explanation:

We know we will need a balanced equation with masses and molar masses, so let’s gather all the information in one place.

M_r: 32.00 44.01

2C₈H₁₈ + 25O₂ ⟶ 16CO₂ + 18H₂O

m/g: 9.88

(a) Calculate the moles of O₂

n = 9.88 g O₂ ×1 mol O₂ /32.00 g O₂

n = 0.3088 mol O₂

(b) Calculate the moles of CO₂

The molar ratio is (16 mol CO₂/25 mol O₂)

n = 0.3088 mol O₂ × (16 mol CO₂/25 mol O₂)

n = 0.1976 mol CO₂

(c) Calculate the mass of CO₂

Mass of CO₂ = 0.1976 mol CO₂ × (44.01 g CO₂/1 mol CO₂)

Mass of CO₂ = 8.70 g CO₂

7 0

3 years ago

In the decomposition of water, why is twice as much hydrogen as oxygen formed?(1 point)

Ugo [173]

Answer:

1. Which statement correctly describes the classification of chemical reactions into different categories?

-Not all reactions fit into a category, and some reactions can fit into more than one category.

2. In a synthesis reaction, two atoms of sodium (Na) combine with one molecule of chlorine gas (Cl2) to produce sodium chloride (NaCl). How many molecules of sodium chloride are produced?

-Two

3. In the decomposition of water, why is twice as much hydrogen as oxygen formed?

- There are two atoms of hydrogen and one atom of oxygen in a water molecule.

4. Which component is transferred between substances in an oxygen-reduction reaction?

-Electrons

5. In a chemical reaction, substance A transfers electrons to substance B. Which statement is correct?

-Substance B is reduced and acts as the oxidizing agent.

5 0

2 years ago

How long does it take long currents to complete their cycle around the world?

monitta

Answer:it takes about a day

Explanation:

7 0

3 years ago

The decomposition of hydrogen peroxide follows first order kinetics and has a rate constant of 2.54 x 10-4 s-1 at a certain temp

Eva8 [605]

Answer:

$[A]_0=0.400M$

Explanation:

Hello.

In this case, since the first-order reaction is said to be linearly related to the rate of reaction:

$r=-k[A]$

Whereas [A] is the concentration of hydrogen peroxide, when writing it as a differential equation we have:

$\frac{d[A]}{dt} =-k[A]$

Which integrated is:

$ln(\frac{[A]}{[A]_0} )=-kt$

And we can calculate the initial concentration of the hydrogen peroxide as follows:

$[A]_0=\frac{[A]}{exp(-kt)}$

Thus, for the given data, we obtain:

$[A]_0=\frac{0.321M}{exp(-2.54x10^{-4}s^{-1}*855s)}$

$[A]_0=0.400M$

Best regards!

3 0

3 years ago

How many molecules of N204 are in 85.0 g of N2O4?

alukav5142 [94]

Answer:

5.56 × 10^23 molecules

Explanation:

The number of molecules in a molecule can be calculated by multiplying the number of moles in that molecule by Avagadro's number (6.02 × 10^23)

Using mole = mass/molar mass

Molar mass of N2O4 = 14(2) + 16(4)

= 28 + 64

= 92g/mol

mole = 85.0/92

= 0.9239

= 0.924mol

number of molecules of N2O4 (nA) = 0.924 × 6.02 × 10^23

= 5.56 × 10^23 molecules

4 0

3 years ago