All categories

2 years ago

1. How much energy must be absorbed to break the bonds of the 2 molecules of HCl?

Chemistry

1 answer:

IRISSAK [1]2 years ago

6 0

Bond energy refers to the energy that must be taken in to break a bond. It is also the energy required to form the bond.

<h3>What is Bond energy?</h3>

The term bond energy refers to the energy that must be taken in to break a bond. It is also the energy required to form the bond.

The energy that must be supplied to break the bonds in two molecules of HCl is 862 J. The energy released is obtained from; 862J - [436 +262] = 164J.

The total energy of the reaction is 164J, this is called the enthalpy change. Based on this value of the total energy, the reaction is endothermic. Hence, it is true that; "It takes more energy to break the two H–Cl bonds than is released when forming the H–H and Cl–Cl bonds."

Learn more about bond energy:brainly.com/question/16754172?

#SPJ1

You might be interested in

How are flagella and cilia alike?

Hoochie [10]

Answer: Both store of celluar materials

Explanation:

I have the same question here is proof:

3 0

2 years ago

If 16.00 g of O₂ reacts with 80.00 g NO, how many the excess reactant are left over? (enter only the value, round to whole numbe

pishuonlain [190]

Answer:

Explanation:

We will need a balanced equation with masses, moles, and molar masses of the compounds involved.

1. Gather all the information in one place with molar masses above the formulas and masses below them.

Mᵣ: 30.01 32.00 46.01

2NO + O₂ ⟶ 2NO₂

Mass/g: 80.00 16.00

2. Calculate the moles of each reactant

$\text{moles of NO} = \text{80.00 g NO} \times \dfrac{\text{1 mol NO}}{\text{30.01 g NO}} = \text{2.666 mol NO}\\\\\text{moles of O}_{2} = \text{16.00 g O}_{2} \times \dfrac{\text{1 mol O}_{2}}{\text{32.00 g O}_{2}} = \text{0.5000 mol O}_{2}$

3. Calculate the moles of NO₂ we can obtain from each reactant

From NO:

The molar ratio is 2 mol NO₂:2 mol NO

$\text{Moles of NO}_{2} = \text{2.333 mol NO} \times \dfrac{\text{2 mol NO}_{2}}{\text{2 mol NO}} = \text{2.333 mol NO}_{2}$

From O₂:

The molar ratio is 2 mol NO₂:1 mol O₂

$\text{Moles of NO}_{2} = \text{0.5000 mol O}_{2}\times \dfrac{\text{2 mol NO}_{2}}{\text{1 mol Cl}_{2}} = \text{1.000 mol NO}_{2}$

4. Identify the limiting and excess reactants

The limiting reactant is O₂ because it gives the smaller amount of NO₂.

The excess reactant is NO.

5. Mass of excess reactant

(a) Moles of NO reacted

The molar ratio is 2 mol NO:1 mol O₂

$\text{Moles reacted} = \text{0.500 mol O}_{2} \times \dfrac{\text{2 mol NO}}{\text{1 mol O}_{2}} = \text{1.000 mol NO}$

(b) Mass of NO reacted

$\text{Mass reacted} = \text{1.000 mol NO} \times \dfrac{\text{30.01 g NO}}{\text{1 mol NO}} = \text{30.01 g NO}$

(c) Mass of NO remaining

Mass remaining = original mass – mass reacted = (80.00 - 30.01) g = 50 g NO

5 0

3 years ago

What is the oxidation number for iodine in Mg(IO3)2 ?

mestny [16]

The oxidation number of iodine is 5 in Mg(IO3)2 which can be calculated as
Mg(IO3)2
MgI2O6
As we know that
Mg has +2
O has -2
So,
(+2) + 2I + 6 (-2)=0
2 + 2I - 12 =0
10+ 2I =0
10 = 2I
I =5

6 0

3 years ago

Read 2 more answers

Chemistry

madam [21]

Answer: 1. 3.914 × ^10-4 | 2. 4.781 × ^10-1

Explanation:

7 0

3 years ago

(02.01 MC)

Rina8888 [55]

Answer:

C. Particle size

Explanation:

The sand, which has smaller particles, will go through the sieve, while the rice (with a larger particle size) will not

4 0

2 years ago