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notsponge [240]
3 years ago
6

Which describes a speed?

Chemistry
1 answer:
Tanya [424]3 years ago
8 0
Its A or B... Correct me if im wrong. :)
You might be interested in
Complete and balance the following redox equation using the set of smallest whole– number coefficients. Now sum the coefficients
Elena L [17]

Answer : The balanced chemical equation in a acidic solution is,

BrO_3^-(aq)+6H^+(aq)+3Sb^{3+}(aq)\rightarrow Br^-(aq)+3H_2O(l)+3Sb^{5+}(aq)

The sum of the coefficients is, 17

Explanation :

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.

Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.

Rules for the balanced chemical equation in acidic solution are :

First we have to write into the two half-reactions.

Now balance the main atoms in the reaction.

Now balance the hydrogen and oxygen atoms on both the sides of the reaction.

If the oxygen atoms are not balanced on both the sides then adding water molecules at that side where the less number of oxygen are present.

If the hydrogen atoms are not balanced on both the sides then adding hydrogen ion (H^+) at that side where the less number of hydrogen are present.

Now balance the charge.

The given chemical reaction is,

BrO_3^-(aq)+Sb^{3+}(aq)\rightarrow Br^-(aq)+Sb^{5+}(aq)

The oxidation-reduction half reaction will be :

Oxidation : Sb^{3+}\rightarrow Sb^{5+}

Reduction : BrO_3^-\rightarrow Br^-

  • First balance the main element in the reaction.

Oxidation : Sb^{3+}\rightarrow Sb^{5+}

Reduction : BrO_3^-\rightarrow Br^-

  • Now balance oxygen atom on both side.

Oxidation : Sb^{3+}\rightarrow Sb^{5+}

Reduction : BrO_3^-\rightarrow Br^-+3H_2O

  • Now balance hydrogen atom on both side.

Oxidation : Sb^{3+}\rightarrow Sb^{5+}

Reduction : BrO_3^-+6H^+\rightarrow Br^-+3H_2O

  • Now balance the charge.

Oxidation : Sb^{3+}\rightarrow Sb^{5+}+2e^-

Reduction : BrO_3^-+6H^++6e^-\rightarrow Br^-+3H_2O

The charges are not balanced. Now multiplying oxidation reaction by 3 and then adding both equation, we get the balanced redox reaction.

Oxidation : 3Sb^{3+}\rightarrow 3Sb^{5+}+6e^-

Reduction : BrO_3^-+6H^++6e^-\rightarrow Br^-+3H_2O

The balanced chemical equation in acidic medium will be,

BrO_3^-(aq)+6H^+(aq)+3Sb^{3+}(aq)\rightarrow Br^-(aq)+3H_2O(l)+3Sb^{5+}(aq)

The sum of the coefficients = 1 + 6 + 3 + 1 + 3 + 3

The sum of the coefficients = 17

7 0
3 years ago
Add a constant temperature when the volume of the gas is decreased what happens to its pressure
Margaret [11]

Answer:

<h2>Pressure will increase</h2>

Explanation:

At a constant temperature, the pressure of gas will increase proportional to the decrease in volume of the gas.

P1V1= P2V2

Decrease in volume result in increase in pressure as the equation has to hold true.

8 0
2 years ago
A 65.0-gram sample of some unknown metal at 100.0° C is added to 100.8 grams of water at 22.0° C. The temperature of the water r
vampirchik [111]
We do a heat balance to solve this:
(m cp ΔT)water = -(m cp ΔT)metal
100.8 (4.18) (27 - 22) = -65 (cp)(27-100)
cp = 100.8 (4.18) (27 - 22) / (-65 (27-100))
cp = 0.44 J/ (°C × g)

The specific heat of the metal is 0.44 J/ (°C × g)
5 0
3 years ago
What would be the oxidation and reduction half reactions for this equation?
Sedbober [7]

Answer:

Fe(s) → Fe²⁺(aq) + 2e⁻   OXIDATION

Mg²⁺(aq) + 2e⁻ → Mg(s)   REDUCTION

Explanation:

The redox reaction is: MgCl₂(aq) + Fe(s) → FeCl₂(aq) + Mg(s)

We need to know that elements in ground state have 0 as the oxidation state.

Iron in the reactants, and Mg in the products

In the magnessium chloride, the Mg acts with+2, so the oxidation state has decreased → REDUCTION

In the iron(II) chloride, the Fe acts with +2, so the oxidation statehas increased → OXIDATION

The half reactions are:

Fe(s) → Fe²⁺(aq) + 2e⁻   OXIDATION

Mg²⁺(aq) + 2e⁻ → Mg(s)   REDUCTION

5 0
3 years ago
In the boxes below, draw three particle diagrams representing the sample
Alexxandr [17]

Answer: 2

Explanation: bencause they are changing

5 0
3 years ago
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