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4 years ago

The ionic equations represent the reactions between four metals, P, Q, R and S, and solutions of the salts of the same metals

Chemistry

1 answer:

EleoNora [17]4 years ago

5 0

Answer:

P + Q2+ -> no reaction

R + P2+ -> R2+ + P

Q + S2+ -> Q2+ + S

S + P2+ -> S2+ + P

S + R2+ -> S2+ + R

S + Q2+ -> no reaction

What is the correct order of reactivity of the metals?

Most -----------------------> least

A. P R S Q

B. Q R S P

C. Q S R P

D. S Q P Rhhgu

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Is the following equation balanced? SO3 + 2H2O H2SO4 no yes

postnew [5]

Answer: No

Explanation: It's not balanced because four oxygen atoms in H2SO4, whereas there are 5 oxygen atoms in the reactants side. Also, there's more hydrogen atoms on the reactants side.

I hope this helps!

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3 years ago

Chlorine radicals perform the first propagation step:

Black_prince [1.1K]

Answer:

b. radicals form easily in the presence of chlorine radicals.

Explanation:

Chlorine radicals perform the first propagation step: because "radicals form easily in the presence of chlorine radicals."

This is because the first propagation step consumes a CHLORINE RADICAL while the second propagation step regenerates a CHLORINE RADICAL. In this way, a chain reaction occurs, whereby one CHLORINE RADICAL can ultimately cause thousands of molecules of methane to be converted into chloromethane with C12 present.

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3 years ago

Hotosynthesis can be represented by 6CO2(g)+6H2O(l)⇌C6H12O6(s)+6O2(g) Which of the following will be false when the photosynthes

antoniya [11.8K]

Answer: Option (b) and (d) are correct.

Explanation:

An equilibrium reaction is defined as the reaction in which rate of forward reaction equals rate of backward reaction.

A photosynthesis reaction is the reaction in which plants in the presence of sunlight, water, and carbon dioxide make their own food.

The amount of carbon dioxide consumed will be equal to the rate of formation of oxygen into the atmosphere.

Hence, the statement rate of formation of $O_{2}$ is equal to the rate of formation of $CO_{2}$ is true.

Concentration of oxygen may remain constant but it will not decrease. Hence, the statement concentration of $O_{2}$ will begin decreasing, is false.

As both oxygen and carbon dioxide are present in an equilibrium reaction, So, their concentration will not change.

Hence, the statement concentrations of $CO_{2}$ and $O_{2}$ will not change, is true.

Concentration of carbon dioxide and oxygen will also depend on the limiting reagent. So, it is not necessary that the concentrations of $CO_{2}$ and $O_{2}$ will be equal.

Some amount of carbon dioxide might escape out into the air.

Hence, the statement concentrations of $CO_{2}$ and $O_{2}$ will be equal, is false.

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3 years ago

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Answer:

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4 years ago

What kind of bonds are hydrogen bonds?

Irina-Kira [14]

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3 years ago