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tensa zangetsu [6.8K]
2 years ago
11

Which of the following statements regarding energy changes during a reaction are true?. 1) If the heat of reaction, ΔH, is negat

ive, the energy of the products is higher than the energy of the reactants, and the reaction is endothermic.2)Two or more atoms must collide, with proper orientation, with energy greater than or equal to the activation energy for a reaction to occur.3)When the activation energy is high, the reaction rate is fast.4) The energy of a collision between atoms or molecules must be greater than the activation energy (Ea) for bonds to be broken.
Chemistry
2 answers:
alexandr1967 [171]2 years ago
7 0

Answer:

2)Two or more atoms must collide, with proper orientation, with energy greater than or equal to the activation energy for a reaction to occur

Explanation:

Activation energy can be defined as the energy needed in order for a reaction to occur. Activation energy helps to also determine the rate of the reaction that is happening.

When the activation energy of a particular reaction is high, the rate or speed of that reaction tends to be slow while when the activation energy of a particular reaction is low, the rate or speed of that reaction in quite fast.

The Collision theory states that the collision of two or more reactants with the appropriate amount of energy (activation energy) and the proper or right orientation is what causes an effective chemical reaction to occur.

sergejj [24]2 years ago
4 0
2.<span>Two or more atoms must collide, with proper orientation, with energy greater than or equal to the activation energy for a reaction to occur</span>
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6 0
2 years ago
Consider four atoms from the second period: lithium, beryllium boron carbon and nitrogen which of these element has the lowest e
bearhunter [10]
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5 0
3 years ago
Read 2 more answers
Together, the protons and neutrons are called what?
mario62 [17]
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3 0
3 years ago
Read 2 more answers
fills a 500.mL flask with 3.6atm of carbon monoxide gas and 1.2atm of water vapor. When the mixture has come to equilibrium she
enot [183]

Answer:

The answer to the question is

The pressure of carbon dioxide after equilibrium is reached the second time is 0.27 atm rounded to 2 significant digits

Explanation:

To solve the question, we note that the mole ratio of the constituent is proportional to their partial pressure

At the first trial the mixture contains

3.6 atm CO

1.2 atm H₂O (g)

Total pressure = 3.6+1.2= 4.8 atm

which gives

3.36 atm CO

0.96 atm H₂O (g)

0.24 atm H₂ (g)

That is

CO+H₂O→CO(g)+H₂ (g)

therefore the mixture contained

0.24 atm CO₂ and the total pressure =

3.36+0.96+0.24+0.24 = 4.8 atm

when an extra 1.8 atm of CO is added we get Increase in the mole fraction of CO we have one mole of CO produces one mole of H₂

At equilibrium we have 0.24*0.24/(3.36*0.96) = 0.017857

adding 1.8 atm CO gives 4.46 atm hence we have

 (0.24+x)(0.24+x)/(4.46-x)(0.96-x) = 0.017857

which gives x = 0.031 atm or x = -0.6183 atm

Dealing with only the positive values we have the pressure of carbon dioxide = 0.24+0.03 = 0.27 atm

7 0
3 years ago
Look up the active ingredient in baking soda. Write a molecular and net ionic equation when that active ingredient is mixed with
Volgvan

Answer:

The active ingredients in baking soda (NaHCO3) are

Na^+ and HCO3^-

when Baking soda reacts with Acetic acid

Molecular equation

 NaHCO3(aq) + CH3COOH(aq) → Na(CH3COO)(aq) + CO2(g) +H2O(l)

Ionic equation

Na^+ + HCO3^-  + CH3COOH →   Na^+ + CH3COO^-  +CO2 + H2O

as Na^+ is present on both sides so it will cancel out and the net ionic equation will be

HCO3^-(aq) + CH3COOH(aq) → CH3COO^-(aq) + CO2(g) + H2O(l)

6 0
3 years ago
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