The table shows the concentration of a reactant, №15229563, 21.12.2022 13:24

Chemistry

The table shows the concentration of a reactant in the reaction mixture over a period of time. reactant concentration time concentration 0 s 1.8 m 210 s 1.2 m 450 s 0.8 m 580 s 0.6 m 720 s 0.4 m what is the average rate of the reaction over the first 580 seconds? a. 1.6 × 10−3 b. 1.9 × 10−3 c. 2.0 × 10−3 d. 2.2 × 10−3

Step-by-step answer

P Answered by PhD

19

C. 2.0 x 10⁻³

Explanation:

The average rate of a reaction is the rate of change of the concentration of the reactants (or products) with time.

The average rate of the reaction = - (ΔC)/(Δt).

∵ The concentration of the reactants changes from 1.8 M to 0.6M for 580 s.

∴ The average rate of the reaction over the first 580 seconds

= - (ΔC)/(Δt) = - [(0.6M) - (1.8 M)]/[(580.0 s) - (0.0 s)] = 2.0 x 10⁻³ M.s⁻¹.

So C. 2.0 x 10⁻³ is the right answer

Chemistry

Question 2(multiple choice worth 3 points) (07.05 mc) the table shows the concentration of a reactant in the reaction mixture over a period of time. reactant concentration time concentration 0 s 1.8 m 210 s 1.2 m 450 s 0.8 m 580 s 0.6 m 720 s 0.4 m what is the average rate of the reaction over the first 580 seconds? 1.6 × 10−3 1.9 × 10−3 2.0 × 10−3 2.2 × 10−3

Step-by-step answer

P Answered by PhD

33

2.0 x 10⁻³ M/s.

Explanation:

The rate of the reaction is the change of the concentration of the reactants or the products with time.

The rate of the reaction = - Δ[reactants]/Δt = - [(0.6 M - 1.8 M)]/(580 s - 0 s) = 2.069 x 10⁻³ M/s.

Mathematics

The table shows the concentration of a reactant in the reaction mixture over a period of time. Reactant Concentration Time Concentration 0 s 1.8 M 210 s 1.2 M 450 s 0.8 M 580 s 0.6 M 720 s 0.4 M What is the average rate of the reaction over the entire course of the reaction? A. 1.6 × 10−3 B. 1.9 × 10−3 C. 2.0 × 10−3 D. 2.2 × 10−3

Step-by-step answer

P Answered by PhD

6

Option CThe average rate of the reaction over the entire course of the reaction is: $2.0 \times 10^{-3}$

Solution:

Average rate is the ratio of concentration change to the time taken for the change

$Average\ rate = \frac{ \triangle c }{\triangle t }$

The concentration of the reactants changes 1.8 M to 0.6 M

here, the time interval given is 0 to 580 sec

Therefore,

$Average\ rate = \frac{1.8-0.6}{580} \\\\Average\ rate = \frac{1.2}{580} \\\\Average\ rate \approx 2.0 \times 10^{-3}$

Thus option C is correct

Mathematics

The table shows the concentration of a reactant in the reaction mixture over a period of time. Reactant Concentration Time Concentration 0 s 1.8 M 210 s 1.2 M 450 s 0.8 M 580 s 0.6 M 720 s 0.4 M What is the average rate of the reaction over the entire course of the reaction? A. 1.6 × 10−3 B. 1.9 × 10−3 C. 2.0 × 10−3 D. 2.2 × 10−3

Step-by-step answer

P Answered by PhD

6

Option CThe average rate of the reaction over the entire course of the reaction is: $2.0 \times 10^{-3}$

Solution:

Average rate is the ratio of concentration change to the time taken for the change

$Average\ rate = \frac{ \triangle c }{\triangle t }$

The concentration of the reactants changes 1.8 M to 0.6 M

here, the time interval given is 0 to 580 sec

Therefore,

$Average\ rate = \frac{1.8-0.6}{580} \\\\Average\ rate = \frac{1.2}{580} \\\\Average\ rate \approx 2.0 \times 10^{-3}$

Thus option C is correct

Chemistry

The table shows the concentration of a reactant in the reaction mixture over a period of time. reactant concentrationtime concentration 0 s 1.8 m 210 s 1.2 m 450 s 0.8 m 580 s 0.6 m 720 s 0.4 m what is the average rate of the reaction over the first 580 seconds? 1.6 × 10−3 1.9 × 10−3 2.0 × 10−3 2.2 × 10−3

Step-by-step answer

P Answered by Master

$2.0*10^{-3}$

Explanation:

average rate is defined as the ratio of concentration change to the time taken for the change.it does not depend on the way in which the concentration change.it depends only on the initial and final concentrations in the given time in which we have to find the average rate.

here, the time interval given is 0 to 580 sec

the concentration change (c) = 1.8 - 0.6 = 1.2 M

time (t) = 580 sec

average rate (r) = $\frac{c}{t}$ = $\frac{1.2}{580}$ ≅ $2.0*10^{-3}$ $\frac{M}{sec}$

Chemistry

The table shows the concentration of a reactant in the reaction mixture over a period of time. reactant concentrationtime concentration 0 s 1.8 m 210 s 1.2 m 450 s 0.8 m 580 s 0.6 m 720 s 0.4 m what is the average rate of the reaction over the first 580 seconds? 1.6 × 10−3 1.9 × 10−3 2.0 × 10−3 2.2 × 10−3

Step-by-step answer

P Answered by Master

$2.0*10^{-3}$

Explanation:

average rate is defined as the ratio of concentration change to the time taken for the change.it does not depend on the way in which the concentration change.it depends only on the initial and final concentrations in the given time in which we have to find the average rate.

here, the time interval given is 0 to 580 sec

the concentration change (c) = 1.8 - 0.6 = 1.2 M

time (t) = 580 sec

average rate (r) = $\frac{c}{t}$ = $\frac{1.2}{580}$ ≅ $2.0*10^{-3}$ $\frac{M}{sec}$

Chemistry

Question 1(multiple choice worth 3 points) (07.05 lc) when zinc reacts with hydrochloric acid, it produces hydrogen gas. as the reaction proceeds, why does the rate of production of hydrogen gas decrease? the concentration of hydrogen gas decreases. the concentration of the reactants decreases. the hydrogen gas formed inhibits the reaction. the hydrogen gas also reacts with the zinc metal. question 2(multiple choice worth 3 points) (07.05 lc) which of the following is true about catalysts? catalysts increase the number of collisions that occur

Step-by-step answer

P Answered by Specialist

10

The concentration of the reactants decreases.

Explanation: Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

k= rate constant

x = order with respect to

y = order with respect to

Thus as the concentration of reactants decrease, the rate of the reaction also decrease and thus the rate of formation of products decrease.

Chemistry

Question 1(multiple choice worth 3 points) (07.05 lc) when zinc reacts with hydrochloric acid, it produces hydrogen gas. as the reaction proceeds, why does the rate of production of hydrogen gas decrease? the concentration of hydrogen gas decreases. the concentration of the reactants decreases. the hydrogen gas formed inhibits the reaction. the hydrogen gas also reacts with the zinc metal. question 2(multiple choice worth 3 points) (07.05 lc) which of the following is true about catalysts? catalysts increase the number of collisions that occur

Step-by-step answer

P Answered by Specialist

10

The concentration of the reactants decreases.

Explanation: Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

k= rate constant

x = order with respect to

y = order with respect to

Thus as the concentration of reactants decrease, the rate of the reaction also decrease and thus the rate of formation of products decrease.

Chemistry

What elements combined with Strontium, St, in a 1:1 ratio?

Step-by-step answer

P Answered by PhD

Answer: chalcogens.
Explanation: Strontium is an alkaline earth metal, it always exhibits a degree of oxidation in its compounds +2.
Chalcogens are a group of 6 chemical elements (oxygen O, sulfur S, selenium se, tellurium te, polonium Po) that have an oxidation state of -2 => Chalcogens will combine with strontium in a ratio of 1:1.

Chemistry

LaToya uses 50 newtons (N) of force to pull a 500 N cart. Which statements are correct about calculating LaToya s mechanical advantage? Select all that apply.A. The input force is 50 N.B. The output force is 50 N.C. The input force is 500 N.D. The output force is 450 N.E. The mechanical advantage is 10.F. The mechanical advantage is 100.

Step-by-step answer

P Answered by Master

Answer:

A

Step-by-step explanation:

The input force is 50 N. But it will not create not any change. No mechanical advantage is observed.

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