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Maslowich
3 years ago
14

Chemical reactions occur when molecules or atoms collide in a way that the bonds between atoms break and new bonds form. Breakin

g the bonds of the reactants requires energy, whereas bond formation releases energy. Select the true statements regarding energy changes during a reaction. Increasing the concentration of reactants increases the number of collisions, and the reaction goes faster. If the heat of reaction, Δ𝻠, is positive, the energy of the products is lower than the energy of the reactants and the reaction is endothermic. When the activation energy is low, the reaction rate is slow. The activation energy, đť¸a , of the forward reaction is the difference between the energy of the products and the energy of the transition state. Decreasing the temperature decreases the kinetic energy of the reactants, and the reaction goes more slowly. Reactants must collide with proper orientation and with energy greater than or equal to the activation energy for a reaction to occur. The energy of a collision between atoms or molecules must be greater than or equal to the activation energy, đť¸a , for bonds to be broken.
Chemistry
1 answer:
lutik1710 [3]3 years ago
6 0

The correct statements are as follows:  

1. Reactants must collide, with proper orientations, with the energy greater than or equal to the activation energy for a reaction to take place. It is a correct statement, as to undergo a chemical reaction, the atoms should exhibit proper orientations and enough energy to reach the activation energy.

2. Increasing the concentration of a reactant increases the number of collisions, and the reaction goes faster. The mentioned statement is true, as when increasing the concentration of reactants, there should be more reactants. Thus, the collision will be more that makes the reaction to go faster.  

3. The energy of a collision between the molecules or atoms must be greater than the activation energy to break the bonds. The given statement is true, as, with the increase in activation energy, the reaction will get slower. Thus, the energy of the reactants is greater in comparison to the activation energy, and then the reaction is faster to break the bond.  

4. Decreasing the temperature decreases the kinetic energy of the reactants, and the reaction goes very slowly. The given statement is true, as when the temperature decreases, the kinetic energy that is required to dissociate the bond, also decreases. This undergoes a slow reaction.  


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3 years ago
The following data were obtained in a kinetics study of the hypothetical reaction A + B + C → products. [A]0 (M) [B]0 (M) [C]0 (
Vladimir [108]

Answer:

B. First order, Order with respect to C = 1

Explanation:

The given kinetic data is as follows:

A + B + C → Products

     [A]₀     [B]₀    [C]₀       Initial Rate (10⁻³ M/s)

1.   0.4      0.4     0.2       160

2.  0.2      0.4      0.4       80

3.   0.6     0.1       0.2       15

4.   0.2     0.1       0.2        5

5.   0.2     0.2      0.4       20

The rate of the above reaction is given as:

Rate = k[A]^{x}[B]^{y}[C]^{z}

where x, y and z are the order with respect to A, B and C respectively.

k = rate constant

[A], [B], [C] are the concentrations

In the method of initial rates, the given reaction is run multiple times. The order with respect to a particular reactant is deduced by keeping the concentrations of the remaining reactants constant and measuring the rates. The ratio of the rates from the two runs gives the order relative to that reactant.

Order w.r.t A : Use trials 3 and 4

\frac{Rate3}{Rate4}= [\frac{[A(3)]}{[A(4)]}]^{x}

\frac{15}{5}= [\frac{[0.6]}{[0.2]}]^{x}

3 = 3^{x} \\\\x =1

Order w.r.t B : Use trials 2 and 5

\frac{Rate2}{Rate5}= [\frac{[B(2)]}{[B(5)]}]^{y}

\frac{80}{20}= [\frac{[0.4]}{[0.2]}]^{y}

4 = 2^{y} \\\\y =2

Order w.r.t C : Use trials 1 and 2

\frac{Rate1}{Rate2}= [\frac{[A(1)]}{[A(2)]}]^{x}[\frac{[B(1)]}{[B(2)]}]^{y}[\frac{[C(1)]}{[C(2)]}]^{z}

we know that x = 1 and y = 2, substituting the appropriate values in the above equation gives:

\frac{160}{80}= [\frac{[0.4]}{[0.2]}]^{1}[\frac{[0.4]}{[0.4]}]^{2}[\frac{[0.2]}{[0.4]}]^{z}

1 = (0.5)^{z}

z = 1

Therefore, order w.r.t C = 1

8 0
3 years ago
What is the mass of aluminum oxide (101.96 g/mol) produced from 1.74 g of manganese(iv) oxide (86.94 g/mol)?
NemiM [27]

the mass of aluminum oxide (101.96 g/mol) produced from 1.74 g of manganese(iv) oxide (86.94 g/mol) is 1.36g

The reaction is 3 MnO2 + 4 Al ------ 2Al2o3+ Mn

3 mole of manganese oxide give 2 moles of aluminum oxide so by the reaction n( MnO2)/3 =n(al203)2

the formula is n= mass/M so, now substituting values

m (Al2O3)= m(MnO2) X 2 X M (Al2O3) / M(MnO2 X3

so, by substituting values, 2 X101.96 X1.74g / 3 X 86.94 =1.36g

so mass of aluminum oxide obtained = 1.36g

To learn more about Mass:

brainly.com/question/19694949

#SPJ4

3 0
2 years ago
I NEED HELP ASAPPPPPPPPPPPPPPPP
RoseWind [281]

Answer:

i wold think it is C

Explanation:

8 0
3 years ago
Read 2 more answers
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