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3 years ago

Below is a diagram showing the chemical energy (Ech) for the formation of water. Is the reaction exothermic or endothermic?

Chemistry

1 answer:

BigorU [14]3 years ago

6 0

Answer: exothermic

Explanation: chemical reactions that release energy is called exothermic, and in this case, more energy is being released. (I THINK)

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To decide on criteria for structure strength to avoid damage from earthquakes, engineers look at ________ to determine _________

N76 [4]

I believe it’s C, it makes the most sense

4 0

3 years ago

Read 2 more answers

Perform the following conversion: 6.1 × 103 K (the surface temperature of the Sun) to °F and °C. Pay attention to the number of

Keith_Richards [23]

Answer:

$\°C=5.8x10^3\°C$

$\°F=1.1x10^4\°F$

Explanation:

Hello,

In this case, for the calculation of the temperature in degree Celsius we subtract 273.15 to the given temperature in kelvins:

$\°C=6100-273.15\\\\\°C=5.8x10^3\°C$

Next, by applying the following equation we compute it in degree Fahrenheit:

$\°F=(5.8x10^{3}*9/5) + 32\\\\\°F=1.1x10^4\°F$

Clearly, since the initial unit has two significant figures the computed units also show two significant figures.

Regards.

5 0

3 years ago

Calculate ΔHo for the following reaction ussing the given bond dissociation energiesCH4(g) + 2O2(g) --> CO2(g) + 2H2O(g)BOND

Mazyrski [523]

Answer:

The ΔH° for the following reaction is -794 kJ, hence exothermic reaction,

Explanation:

$CH_4(g) + 2O_2(g)\rightarrow CO_2(g) + 2H_2O(g) ,$ ΔH° = ?

We are given with:

$\Delta H_{O-O}=142 kJ/mol$

$\Delta H_{O=O}=498 kJ/mol$

$\Delta H_{H-O}=459 kJ/mol$

$\Delta H_{C-H}=411 kJ/mol$

$\Delta H_{C-O}=358 kJ/mol$

$\Delta H_{C=O}=799 kJ/mol$

ΔH° =

(Energies required to break bonds on reactant side) - (Energies released on formation of bonds on product side)

$\Delta H^o=(1 mol\times 4\times \Delta H_{C-H}+2 mol\times 1\times \Delta H_{O=O})-(1 mol\times 2\times \Delta H_{C=O}+2 mol\times 2\times\Delta H_{H-O})$

$\Delta H^o=(1 mol\times 4\times 411 kJ/mol+2 mol\times 1\times 498 kJ/mol)-(1 mol\times 2\times 799 kJ/mol+2 mol\times 2\times 459 kJ/mol)$

$\Delta H^o=-794kJ$

$\Delta H^o>0$ endothermic reaction

$\Delta H^o$ exothermic reaction

The ΔH° for the following reaction is -794 kJ, hence exothermic reaction,

4 0

4 years ago

Explain how the chromatography shows that all three samples have at least one substance common✨

Alinara [238K]

Monkey is good and that is all their it to it

3 0

3 years ago

I wanted known how many of the reaction below is energy released

Tema [17]

Answer:

Explanation:

In two reactions energy is released.

1) C₆H₁₂O₆ + 6O₂ → 6H₂O + 6CO₂ + heat

It is cellular respiration reaction.It involves the breakdown of glucose molecule in the presence of oxygen to yield large amount of energy. Water and carbon dioxide are also produced as a byproduct.

Glucose + oxygen → carbon dioxide + water + 38ATP

2) 2H₂ + O₂ → 2H₂O ΔH = -486 kj/mol

The given reaction is formation of water. In this reaction oxygen and hydrogen react to form water and 486 kj/mol is also released.

The reaction in which heat is released is called exothermic reaction.

Exothermic reaction:

The type of reactions in which energy is released are called exothermic reactions.

In this type of reaction energy needed to break the bonds are less than the energy released during the bond formation.

For example:

Chemical equation:

C + O₂ → CO₂

ΔH = -393 Kj/mol

it can be written as,

C + O₂ → CO₂ + 393 Kj/mol

Endothermic reactions:

The type of reactions in which energy is absorbed are called endothermic reactions.

In this type of reaction energy needed to break the bond are higher than the energy released during bond formation.

For example:

C + H₂O → CO + H₂

ΔH = +131 kj/mol

it can be written as,

C + H₂O + 131 kj/mol → CO + H₂

5 0

3 years ago