When energy changes forms there is always some thermal energy that is produced that cannot be used. what type of energy is it?

dalvyx [7]

The answer is b!!! !!!

7 0

3 years ago

In an experiment, the same mass of magnesium metal reacted with the same amount of two different acids. the acid used in reactio

denpristay [2]

The mole ratio of the reaction shows that equal volumes of hydrogen gas will be produced by the two reactions.

<h3>What is the mole ratio of a reaction?</h3>

The mole ratio of a reaction is the ratio in which the reactants and products of a given reaction occur for the reaction to proceed to completion.

The mole ratio of a reaction is also known as the stoichiometry of the reaction.

The equation of the two reactions are given below:

$Mg + 2HCl \rightarrow MgCl_2 + H_2$

$Mg + 2CH_3COOH \rightarrow (CH_3COO)_2Mg + H_2 \\$

From the equation of the reaction reaction, an equal volume of hydrogen gas will be produced by the two reactions.

Therefore, the mole ratio of the reaction shows that equal volumes of hydrogen gas will be produced by the two reactions.

Learn more about mole ratio at: brainly.com/question/19099163

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6 0

1 year ago

What is the chemical formula of wood?

ad-work [718]

(99% of the total mass). 49% of carbon, 44% of oxygen, 6% of hydrogen, 0.1-0.3% of nitrogen.

3 0

2 years ago

Can anyone pls help!!!!!!1

Kruka [31]

Answer:

Well I know that when the liquid changes from clear to dark blue and small bubbles form and rise to the surface that is a reaction

Explanation:

7 0

3 years ago

The reaction 2NO(g)+O2(g)−→−2NO2(g) is second order in NO and first order in O2. When [NO]=0.040M, and [O2]=0.035M, the observed

Oksanka [162]

Answer:

(a) The rate of disappearance of $O_{2}$ is: $4.65*10^{-5}$ M/s

(b) The value of rate constant is: 0.83036 $M^{-2}s^{-1}$

(c) The units of rate constant is: $M^{-2}s^{-1}$

(d) The rate will increase by a factor of 3.24

Explanation:

The rate of a reaction can be expressed in terms of the concentrations of the reactants and products in accordance with the balanced equation.

For the given reaction:

$2NO(g)+O_{2}->2NO_{2}$

rate = $-\frac{1}{2} \frac{d}{dt}[NO]$ = $-\frac{d}{dt}[O_{2}]$ = $\frac{1}{2}\frac{d}{dt}[NO_{2}]$ -----(1)

According to the question, the reaction is second order in NO and first order in $O_{2}$ .

Then we can say that, rate = k $[NO]^{2}[O_{2}]$ -----(2)

where k is the rate constant.

The rate of disappearance of NO is given:

$-\frac{d}{dt}[NO]$ = $9.3*10^{-5}$ M/s.

(a) From (1), we can get the rate of disappearance of $O_{2}$ .

Rate of disappearance of $O_{2}$ = $-\frac{d}{dt}[O_{2}]$ = (0.5)*( $9.3*10^{-5}$ ) M/s = $4.65*10^{-5}$ M/s.

(b) The rate of the reaction can be obtained from (1).

rate = $-\frac{1}{2} \frac{d}{dt}[NO]$ = (0.5)*( $9.3*10^{-5}$ )

rate = $4.65*10^{-5}$ M/s

The value of rate constant can be obtained by using (2).

rate constant = k = $\frac{rate}{[NO]^{2}[O_{2}]}$

k = $\frac{4.65*10^{-5}}{(0.040)^{2}(0.035)}$ = 0.83036 $M^{-2}s^{-1}$

(c) The units of the rate constant can be obtained from (2).

k = $\frac{rate}{[NO]^{2}[O_{2}]}$

Substituting the units of rate as M/s and concentrations as M, we get:

$\frac{Ms^{-1} }{M^{3}}$ = $M^{-2}s^{-1}$

(d) The reaction is second order in NO. Rate is proportional to square of the concentration of NO.

$rate\alpha [NO]^{2}$

If the concentration of NO increases by a factor of 1.8, the rate will increase by a factor of $(1.8)^{2}$ = 3.24

5 0

3 years ago