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3 years ago

Given the reaction below which of the following best describes the energy changes in this reaction?

Chemistry

1 answer:

insens350 [35]3 years ago

8 0

Answer:

first choice

Explanation:

energy is written on the left side is its absorbed

2 elements came together so bonds are formed.

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Confused on this question

kotegsom [21]

Answer:

The second option

Explanation:

Check

2×2Fe = 4Fe. Both sides have 4 Fe's

2x3 O = 3x2 O Both sides have 6 O's

3x1C = 3 C Both sides have 3 C's

3 0

3 years ago

In nature, one common strategy to make thermodynamically unfavorable reactions proceed is to couple them chemically to reactions

padilas [110]

Answer:

$\triangle G= -6.7 KJ/mol$

Explanation:

From the question we are told that:

Chemical Reactions:

X=A⇌B,ΔG= 14.8 kJ/mol

Y=B⇌C,ΔG= -29.7 kJ/mol

Z=C⇌D,ΔG= 8.10 kJ/mol

Since

Hess Law

The law states that the total enthalpy change during the complete course of a chemical reaction is independent of the number of steps taken.

Therefore

Generally the equation for the Reaction is mathematically given by

$T = +1 * X +1 * Y +1 *Z$

Therefore the free energy, ΔG is

$\triangle G=1 * \triangle G*X +1 * \triangle G*Y +1 * \triangle G *Z$

$\triangle G= +1 * (14.9) +1 * (-29.7) +1 * (8.10)$

$\triangle G= -6.7 KJ/mol$

5 0

3 years ago

HELP!!! What is the product of the top reaction?

Fofino [41]

Meso−2,3−butanediol is the product of the top reaction

5 0

3 years ago

Calculate the activation energy (ea in kj/mol for a reaction if the rate constant (k is 2.7 × 10-4 (m−1sec−1 at 600 k and 3.5 ×

djyliett [7]

Below are the choices:

a. −166 kJ/mol
b. 166 kJ/mol 
c. 1.64 kJ/mol 
d. 1.66 × 10^5 kJ/mol

To calculate the activation energy of a reaction, we use the Arrhenius equation. You may want to look it up to see how and why it works. In the problem you posted, there are two temperatures and two rate constants. After some rearranging and substitution of the Arrhenius equation, we have Ea = R T1 T2/(T1-T2) ln(k1/k2) = 8.314 J/mol K (600 K)(650 K)/(600 K-650 K) ln(2.7×10^-4 M^−1sec^−1/3.5×10^−3 M−^1sec^−1) = 166145 J/mol = 166 kJ/mol => choice b

6 0

3 years ago

How many grams of CO2 are produced if 2.09 moles of hydrochloric acid are reacted with

Anit [1.1K]

Answer:

The molar mass of CO2 = 44.01 g/mol

Explanation:

Start with 2.09 moles of HCl and convert to moles of CO2 For every 2 moles of HCl used, 1 mole of CO2 is formed.

2.09 mol HCl •(1 mol CO2/2 mol HCl) = 1.045 mol CO2

Now convert moles of CO2 to grams using the molar mass.

1.045 mol CO2 • 44.01 g/mol = 45.99 grams CO2

3 significant figures = 46.0 grams CO2

Hope This Helped

6 0

2 years ago