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1 year ago

Given the following reaction: 2O3---->3O2. DeltaH of reaction=-286kJ/mol

Chemistry

1 answer:

soldi70 [24.7K]1 year ago

4 0

The enthalpy of reaction (ΔH) of the above chemical reaction is equal to -143 kJ/mol.

<h3>What is a chemical reaction?</h3>

A chemical reaction can be defined as a chemical process that involves the continuous transformation (rearrangement) of the ionic, atomic or molecular structure of a chemical element by breaking down and forming chemical bonds, in order to produce a new chemical compound while new bonds are formed.

<h3>What is a balanced equation?</h3>

A balanced chemical equation can be defined as a chemical equation wherein the number of atoms on the reactant (left) side is equal to the number of atoms on the product (right) side.

Next, we would write the properly balanced chemical equation for this chemical reaction:

3/2O₂ -----> 2/2O₃

Therefore, the enthalpy of reaction (ΔH) of the above chemical reaction is half the enthalpy of reaction (ΔH) of the initial chemical reaction:

Enthalpy of reaction (ΔH) = ½ × -286 kJ/mol

Enthalpy of reaction (ΔH) = -143 kJ/mol.

Read more on enthalpy here: brainly.com/question/12993630

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What type of energy is stored within a chemical substance?

s2008m [1.1K]

Chemical Energy is energy stored in the bonds of chemical compounds (atoms and molecules). It is released in a chemical reaction, often producing heat as a by-product (exothermic reaction). Batteries, biomass, petroleum, natural gas, and coal are examples of stored chemical energy and NO i didnt get this off google

4 0

3 years ago

Read 2 more answers

How much energy (heat) is required to convert 248 g of water from 0oC to 154oC? Assume that the water begins as a liquid, that t

Arturiano [62]

Answer: The amount of heat required is 775.7 kJ

Explanation:

The processes involved in the given problem are:

$1.)H_2O(s)(0^oC,273K)\rightarrow H_2O(l)(0^oC,273K)\\2.)H_2O(l)(0^oC,273K)\rightarrow H_2O(l)(100^oC,373K)\\3.)H_2O(l)(100^oC,373K)\rightarrow H_2O(g)(100^oC,373K)\\4.)H_2O(g)(100^oC,373K)\rightarrow H_2O(g)(154^oC,427K)$

Now, we calculate the amount of heat released or absorbed in all the processes.

For process 1:

$q_1=m\times L_f$

where,

$q_1$ = amount of heat absorbed = ?

m = mass of water or ice = 248 g

$L_f$ = latent heat of fusion = 334 J/g

Putting all the values in above equation, we get:

$q_1=248g\times 334J/g=84832J$

For process 2:

$q_2=m\times C_{p,l}\times (T_{2}-T_{1})$

where,

$q_2$ = amount of heat absorbed = ?

$C_{p,l}$ = specific heat of water = 4.184 J/g°C

m = mass of water = 248 g

$T_2$ = final temperature = $100^oC$

$T_1$ = initial temperature = $0^oC$

Putting all the values in above equation, we get:

$q_2=248g\times 4.184J/g^oC\times (100-0)^oC=103763.2J$

For process 3:

$q_3=m\times L_v$

where,

$q_3$ = amount of heat absorbed = ?

m = mass of water or ice = 248 g

$L_v$ = latent heat of vaporization = $40.79kJ/mol\times \frac{1000}{18}=2266.1J/g$ (Conversion factor used: 1 kJ = 1000 J and molar mass of water = 18 g/mol)

Putting all the values in above equation, we get:

$q_3=248g\times 2260J/g=560480J$

For process 4:

$q_4=m\times C_{p,g}\times (T_{2}-T_{1})$

where,

$q_4$ = amount of heat absorbed = ?

$C_{p,g}$ = specific heat of steam = 1.99 J/g°C

m = mass of water = 248 g

$T_2$ = final temperature = $154^oC$

$T_1$ = initial temperature = $100^oC$

Putting all the values in above equation, we get:

$q_4=248g\times 1.99J/g^oC\times (154-100)^oC=26650.1J$

Calculating the total heat absorbed, we get:

$Q=q_1+q_2+q_3+q_4$

$Q=[84832+103763.2+560480+26650.1]J=775,725.3J=775.7kJ$

Hence, the amount of heat required is 775.7 kJ

5 0

4 years ago

_Al(s) + - 02(g) → _Al2O3 (s) Balance equation

AfilCa [17]

Explanation:

Chemical reaction

When two or more substances react and form some new substance it is called as chemical reaction .

For example :

Al (s) + O₂ (g)----> Al₂O₃(s)

Chemical equation

It is the representation of chemical reaction in terms of symbols ,molecular formulas ,moles , states etc .

As we know all chemical reaction obeys law of chemical combination therefore chemical reaction need to be balanced .

Law of conservation of mass

Mass can neither be created nor be destroyed in a chemical reaction , it is always conserved .That is why reactions need to be balanced .

Let us balance

Al (s) + O₂ (g)----> Al₂O₃(s)

After balancing , it becomes :

2Al (s) + 3/2O₂ (g)----> Al₂O₃(s)

6 0

3 years ago

It takes 45.0 J to raise the temperature of an 8.10 g piece of unknown metal from 13.0∘C to 24.3 ∘C. What is the specific heat f

hodyreva [135]

Answer:

0.492 J/g °C

General Formulas and Concepts:

Thermodynamics

Specific Heat Formula: q = mcΔT

q is heat (in J0
m is mass (in g)
c is specific heat (in J/g °C)
ΔT is change in temperature (in °C)

Explanation:

Step 1: Define

Identify variables

[Given] q = 45.0 J

[Given] m = 8.10 g

[Given] ΔT = 24.3 °C - 13.0 °C = 11.3 °C

[Solve] c

Step 2: Solve for c

Substitute in variables [Specific Heat Formula]: 45.0 J = (8.10 g)c(11.3 °C)
Multiply: 45.0 J = (91.53 g °C)c
Isolate c: 0.491642 J/g °C = c
Rewrite: c = 0.491642 J/g °C

Step 3: Check

Follow sig fig rules and round. We are given 3 sig figs.

0.491642 J/g °C ≈ 0.492 J/g °C

5 0

3 years ago

Which element will only gain one electron during a chemical reaction?

Gelneren [198K]

Halogens

Explanation:

Halogens are a group of non-metals located in the seventh group on the periodic table. The will only gain one electron during a chemical reaction.

Halogens have a seven electrons in their outermost shell.
To complete the number of electrons in this shell, they need to gain an additional electron.
One more electron makes the halogen similar to the corresponding noble gas which is very stable.
Halogens are very reactive groups of elements and are highly electronegative.
They have a high affinity for electrons.
These elements are fluorine, chlorine, bromine, iodine and Astatine.

learn more:

Halogens brainly.com/question/6324347

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7 0

3 years ago