Which description explains the role of activation energy in a chemical reaction? A .It provides useful energy that is released in an exothermic reaction.
B. It stops the products from being formed from the intermediate state.
C. It slows down the overall chemical reaction so it does not happen too quickly.
D. It provides reactants with sufficient energy for bonds to break and reform.

Answers

Answer 1

Answer:

Answer: The description it provides reactants with sufficient energy for bonds to break and reform best explains the role of activation energy in a chemical reaction.

Explanation:

Activation energy is defined as the minimum amount of required energy so that a chemical reaction can initiate.

As a result, it provides the reactants with certain amount of energy so that they will get the necessary amount of energy to break their bond and then form new bonds.

Thus, we can conclude that the description it provides reactants with sufficient energy for bonds to break and reform best explains the role of activation energy in a chemical reaction.

Answer 2

Answer: D. Activation energy is the energy that is required in order for a reaction to occur, i.e. break and form new bonds

Related Questions

According to the arrhenius theory an acid is a substance that
The molar mass of I2 is 253.80 g/mol, and the molar mass of NI3 is 394.71 g/mol. How many moles of I2 will form 3.58 g of NI3?
What proof did you see in the experiment that a chemical reaction took place?
What determines the order of placement of the elements on the modern Periodic Table?(1) atomic number(2) atomic mass(3) the number of neutrons, only(4) the number of neutrons and protons
7 Which element has atoms that can form halide ions?(1) iodine (3) strontium(2) silver (4) xenon

The heat of formation of Fe2O3(s) is –826.0 kJ/mol. Calculate the heat of the reaction 4Fe(s) + 3O2(g) → 2Fe2 O3(s) when a 53.99-g sample of iron is reacted.

Answers

Final answer:

The heat of the reaction can be calculated using the enthalpy of formation. For a 53.99-g sample of iron, the heat of the reaction is approximately -798.9 kJ.

Explanation:

To calculate the heat of the reaction, we need to use the concept of enthalpy of formation. The enthalpy of formation of Fe2O3(s) is -826.0 kJ/mol. We can use this value as a conversion factor to find the heat produced when 1 mole of Fe2O3(s) is formed. Since we have a 53.99-g sample of iron, we can calculate the moles of iron and use the conversion factor to find the heat of the reaction.

The molar mass of iron (Fe) is 55.845 g/mol. Therefore, the moles of iron in the sample can be calculated as:

(53.99 g) / (55.845 g/mol) = 0.9662 mol

Now, using the conversion factor:

0.9662 mol Fe × (826.0 kJ/mol) = -798.9 kJ

Therefore, the heat of the reaction 4Fe(s) + 3O2(g) → 2Fe2O3(s) when a 53.99-g sample of iron is reacted is approximately -798.9 kJ.

Learn more about Enthalpy of Formation here:

brainly.com/question/34177147

#SPJ12

Final answer:

The problem is solved by first converting the given mass of Fe to moles, then determining the amount of Fe2O3 formed using the stoichiometry of the reaction. With the heat formation of Fe2O3 given, the heat released in the reaction is calculated to be -399.8 kJ, indicating an exothermic reaction.

Explanation:

To solve the given problem, we first need to calculate the number of moles of Fe in the 53.99-g sample. The molar mass of Fe is about 55.85 g/mol, so 53.99 grams will represent approximately 0.967 moles of iron. Given the reaction 4Fe + 3O2 → 2Fe2O3, the formation of 2 moles of Fe2O3 requires 4 moles of Fe; hence a ratio of 2:4= 0.5:1 is formed. So, from 0.967 moles of iron, we get 0.967*0.5 = 0.484 moles of Fe2O3 formed.

From the problem, we know that the heat of formation of Fe2O3 is -826.0 kJ/mol. Therefore, the heat of reaction or released heat from the formation of 0.484 moles will be 0.484*-826.0 kJ/mol = -399.8 kJ. Because the value is negative, this is an exothermic reaction, releasing heat.

Learn more about Heat of Reaction here:

brainly.com/question/30464598

#SPJ3

Which compound is a saturated hydrocarbon?

Answers

Saturated hydrocarbons are organic compounds that contain only single bonds between the carbon atoms. They are known to be the simplest organic compounds. They are termed as such because they are saturated with water. Examples are the alkanes (ethane, methane, propane, butane, etc.).

Regarding the vaporization of water, which of the following is true? A. A great deal of heat must be lost by water to form hydrogen bonds and allow molecules to move farther apart. B. A great deal of heat must be absorbed by water to break hydrogen bonds and allow molecules to move farther apart. C. Vaporization of water is an exothermic process. D. Water must lose a great deal of heat before it will vaporize.

Answers

Answer: B. A great deal of heat must be absorbed by water to break hydrogen bonds and allow molecules to move farther apart.

Explanation:

Vaporization is a physical process where liquid state changes to gaseous state.

$H_2O(l)\rightarrow H_2O(g)$

Water molecules are bonded by strong hydrogen bonding between the hydrogen atom and the electronegative oxygen atom. Thus water molecules present on the surface are strongly attracted by the molecules present below the surface.

Thus as liquid state has to be changed to gaseous state, the heat must be supplied and the reaction will be endothermic.The heat is used to break the inter molecular forces or the hydrogen bonds present in water to convert them to randomly moving gaseous state.

B. A great deal of heat must be absorbed by water to break hydrogen bonds and allow molecules to move farther apart.

Which statements about hydrogen bonding in water are true?a. The hydrogen atoms of a water molecule have a partial positive charge.
b. The oxygen atom of a water molecule is more electronegative than a hydrogen atom.
c. The hydrogen atoms of a water molecule have a partial negative charge.
d. The hydrogen atom of one water molecule is attracted to the oxygen atom of a different water molecule.
e. The hydrogen atom of a water molecule is attracted to the oxygen atom of the same water molecule.
f. The oxygen atom of a water molecule has a partial positive charge.
g The oxygen atom of a water molecule has a partial negative charge.

Answers

Answer:

The answer to your question is below

Explanation:

a. The hydrogen atoms of a water molecule have a partial positive charge. True.

b. The oxygen atom of a water molecule is more electronegative than a hydrogen atom. True

c. The hydrogen atoms of a water molecule have a partial negative charge. False

d. The hydrogen atom of one water molecule is attracted to the oxygen atom of a different water molecule. True

e. The hydrogen atom of a water molecule is attracted to the oxygen atom of the same water molecule. False,

f. The oxygen atom of a water molecule has a partial positive charge. True

g The oxygen atom of a water molecule has a partial negative charge. True

6X, Y and Z are all gases that behave ideally and react according to the equation shown.
X(g) + 2Y(g) → 2Z(9)
When 3.0 mol of X and 3.0 mol of Y are placed inside a container with a volume of 1.0 dmº, they
react to form the maximum amount of Z.
The final temperature of the reaction vessel is 120°C.
What is the final pressure inside the reaction vessel?
А
4.49 x 10 Pa
B
9.80 x 106 Pa
C
1.47 x 10' Pa
D
1.96 x 10' Pa