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Use the reaction and bond information to answer the question. C2H6 → C2H4 H2 Reactant bond energies: H–C = 413 kJ/mol, C–C singl

nlexa [21]

The energy of the reactant has been higher than the energy of the product, Thus, the reaction has been an exothermic reaction.

Bond energy has been defined as the chemical energy possessed by the bonds in the chemical structure. The energy has been conserved in the chemical reaction.

<h3>Is the reaction endothermic or exothermic?</h3>

In the reaction in which bond energy of the reactant has been higher than the product, it has been an exothermic reaction.

In the reaction in which the bond energy of the product is higher than the reactant, it has been an endothermic reaction.

In the given reaction

$\rm C_2H_6\;\rightarrow\;C_2H_4\;+\;H_2$

The bond energies of reactant has been:

H-C bond = 413 kJ/mol
C-C bond = 347 kJ/mol

The total bond energy of the reactant has been:

$\rm Reactant=6\;\times\;H-C\;bond\;+\;C-C\;bond \\Reactant=6\;\times\;413+347\;kJ/mol\\Reactant=2,825\;kJ/mol$

The total bond energy of the reactant has been 2,825 kJ/mol.

The bond energies of product has been:

H-C = 413 kJ/mol
C=C = 614 kJ/mol
H-H = 432 kJ/mol

The total bond energy of the product has been:

$\rm Product=4\;\times\;H-C\;bond\;+\;C=C\;bond\;+\;H-H\;bond\\Product=4\;\times\;413\;+\;614\;+\;432\;kJ/mol\\Product=2,698\;kJ/mol$

The total bond energy of the product has been 2,698 kJ/mol.

The energy of the reactant has been higher than the energy of the product, Thus, the reaction has been an exothermic reaction, as energy can neither be created nor be destroyed. It has been conserved in the chemical reaction.

Learn more about exothermic reaction, here:

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How does a community look after a volcano erupts

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Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is th

kolbaska11 [484]

Answer: When using 645 L /s of O2 in a temperature and pressure of 195°C, 0.88 atm respectively, we will get 0.355Kg /s NO

Explanation:

First we review the equation that represents the oxidation process of the NH3 to NO.

4NH3(g) + 5O2(g) ⟶4 NO(g) +6 H2O(l)

Second we gather the information what we are going to use in our calculations.

O2 Volume Rate = 645 L /s

Pressure = 0.88 atm

Temperature = 195°C + 273 = 468K

NO molecular weight = 30.01 g/mol

Third, in order to calculate the amount of NO moles produced by 645L/ s of O2, we must find out, how many moles (n) are 645L O2 by using the general gas equation PV =n RT

Let´s keep in mind that using this equation our constant R is 0.08205Lxatm/Kxmol

PV =n RT

n= PV / RT

n= [ 0.88atm x 645L/s] / [ (0.08205 Lxatm/Kxmol) x 468K]

n= 14.781 moles /s of O2

Fourth, now by knowing the amount of moles of O2, we can use the equation to calculate how many moles of NO will be produced and then with the molecular weight, we will finally know the total mass per second .

14.781 moles /s of O2 x 4moles NO / 5 moles O2 x 30.01g NO / 1 mol NO x 1Kg NO /1000g NO = 0.355Kg /s NO

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The process in which the nucleus of an atom splits into two lighter atoms, releasing a large amount of energy, is nuclear .

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It's nuclear fission

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