What is usually released as a product in a combustion reaction?

Consider the following balanced thermochemical equation for a reaction sometimes used for H₂S production: 1/8 S₈(s) + H₂(g) → H₂

castortr0y [4]

ΔH = -15.78 KJ when 25.0 g of S₈ reacts.

<h3>What is Balanced Chemical Equation ?</h3>

The balanced chemical equation is the equation in which the number of atoms on the reactant side is equal to the number of atoms on the product side in an equation.

The given reaction balanced equation is:

1/8 S₈(s) + H₂(g) → H₂S(g) ΔH = -20.22kj

Now,

When 1 mol will react, then ΔH = -20.2 × 8

= -161.6 KJ

When 1 mol of S8 = 8 × 32 g

= 256 g

When 256g of S8 react ΔH = -161.6 KJ

When 1 g reacts, ΔH = $\frac{-161.6}{256}$

=- 0.63125 KJ

When 25 g reacts, ΔH = - 0.63125 × 25

= -15.78 KJ

Thus from the above conclusion we can say that ΔH = -15.78 KJ when 25.0 g of S₈ reacts.

Learn more about the Balanced chemical equation here: brainly.com/question/26694427

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4 0

2 years ago

Chemistry!! Please help asap!! Will mark brainiliest!!

Whitepunk [10]

<h2>Answer:</h2><h3>Part 1. </h3>

Option B is correct option.

The half-reaction 2MnO2 + H2O + 2e- Mn2O3 is missing OH- ions.

Explanation:

Full equation:

2MnO2 + H2O + 2e- → Mn2O3 + 2OH-

The option B which is Mg is stronger reducing agent than Ag is correct option.

Explanation:

Equation:

Mg(s) + 2Ag+ (aq) → Mg2+ (aq) + 2Ag(s)

According to equation Mg converts to Mg+2 which means it gives to electron to reduce Ag. So it act as an reducing agent.

The correct option is B. Which is 5, 1, 8, 5, 1, 4.

Explanation:

Full equation :

5 Fe²⁺ (aq) + MnO₄⁻ (aq) + 8 H⁺ (aq) --> 5 Fe³⁺ (aq) + Mn²⁺ (aq) + 4 H₂O (l)

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5 0

3 years ago

Write a balanced overall reaction from these unbalanced half-reactions. ln->ln3+ cd2+->cd

DochEvi [55]

Oxidation reaction
In ---> In³⁺ + 3e ---1)
reduction reaction
Cd²⁺ + 2e ---> Cd ---2)
when balancing the reactions, electrons have to be balanced. to balance the electrons multiple 1st reaction by 2 and 2nd reaction by 3
1) x 2
2) x 3
2In ---> 2In³⁺ + 6e
3Cd²⁺ + 6e ---> 3Cd
add the 2 equations to obtain the overall reaction

2In + 3Cd²⁺ ---> 2In³⁺ + 3Cd

5 0

3 years ago

Chris the chemist was working in the and he wanted to sou what would happen he put copper chloride into a Bunsen flameAs soon as

Reptile [31]

The question is incomplete, the complete question is;

Chris the Chemist was working in the lab, and he wanted to see what would happen if he put copper chloride into a Bunsen burner flame. As soon as he put it in the flame, it began to emit a green color. Which of these BEST describes this outcome?

A) The heat split the nucleus and created a new element.

B) As the copper chloride was heated, electrons were turned into neutrons.

C) As the electrons moved to a higher energy level, a photon of light is emitted.

D) When excited electrons return back to the ground state, a photon of light is emitted.

Answer:

D) When excited electrons return back to the ground state, a photon of light is emitted.

Explanation:

According to Bohr's model of the atom, electrons may absorb energy and move up to higher energy levels.

These electrons quickly return to ground state from such higher energy excited states thereby emitting the excess energy absorbed during excitation.

If the higher energy level is E2 and the ground state is E1 then the energy of the photon emitted when the electron descends from energy level E2 to E1 is;

ΔE = E2 - E1

This photon emitted accounts for the green colour of the copper salt observed when it was heated.

4 0

3 years ago

What is the molar mass of an element?

Vesnalui [34]

The answer is: the mass of 6.02 x 1023 representative particles of the element.

The base SI unit for molar mass is kg/mol, but chemist more use g/mol (gram per mole).

For example, molar mas of ammonia is 17.031 g/mol.

M(NH₃) = Ar(N) + 3 · Ar(H) · g/mol.

M(NH₃) = 14.007 + 3 · 1.008 · g/mol.

M(NH₃) = 17.031 g/mol.

The molar mass (M) is the mass of a given substance (in this example ammonia) divided by the amount of substance.

8 0

3 years ago