1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
jeka57 [31]
3 years ago
10

Given the redox reaction: Ni + Sn4+ → Ni2+ + Sn2+

Chemistry
2 answers:
Artist 52 [7]3 years ago
5 0
 <span>1. Na 
2. Ni 
3. Na2S 
4. Electrolytic Cell (Galvanic and Voltaic are synonyms, both are electric cells without an external power source. 
5. 3 
6. The first one 
7. Na 
8. Reducing agents are oxidized 
hope this helps you

</span>
Ludmilka [50]3 years ago
5 0

Answer: Ni

Explanation: Oxidation-reduction reaction or redox reaction is defined as the reaction in which oxidation and reduction reactions occur simultaneously.

Oxidation reaction is defined as the reaction in which a substance looses its electrons. The oxidation state of the substance increases.

Ni\rightarrow Ni^{2+}+2e^-

Reduction reaction is defined as the reaction in which a substance gains electrons. The oxidation state of the substance gets reduced.

Sn^{4+}+2e^-\rightarrow Sn^{2+}

The oxidation state of nickel increases from 0 to +2, it is getting oxidized and it undergoes oxidation reaction.

You might be interested in
Which is an unreliable source?
Sunny_sXe [5.5K]

The source that is unreliable is an advertisement for acne medication claims it can clear up acne in less than one week.

<h3>What are citable sources?</h3>

Citable sources are those sources that are gotten from places that are proven to be of good standards and not from mere claims such as:

  • Science journals

  • professional organizations

  • government agencies

Therefore, the source that is unreliable is an advertisement for acne medication claims it can clear up acne in less than one week.

Learn more about citations here:

brainly.com/question/8130130

#SPJ1

5 0
2 years ago
The gas in the piston is at constant temperature. A student increases the pressure on the piston from 2 atm to 3 atm. The observ
Vesna [10]

Answer: row 1, the volume decreases when the pressure increased

Explanation:

7 0
3 years ago
Consider the reaction at 500 ° C 500°C . N 2 ( g ) + 3 H 2 ( g ) − ⇀ ↽ − 2 NH 3 ( g ) K c = 0.061 N2(g)+3H2(g)↽−−⇀2NH3(g)Kc=0.06
Sav [38]

Answer:

Q = 0.061 = Kc

Explanation:

Step 1: Data given

Temperature = 500 °C

Kc=0.061

1.14 mol/L  N2

5.52 mol/L H2

3.42 mol/L NH3

Step 2: Calculate Q

Q=[products]/[reactants]=[NH3]²/ [N2][H2]³

If Qc=Kc then the reaction is at equilibrium.  

If Qc<Kc then the reaction will shift right to reach equilibrium.

If Qc>Kc then the reaction will shift left to reach equilibrium.  

Q = (3.42)² / (1.14 * 5.52³)

Q = 11.6964/191.744

Q = 0.061

Q = Kc the reaction is at equilibrium.  

4 0
3 years ago
Perform the following mathematical operation and report the answer to the appropriate number of significant figures. 5.4-4.21
konstantin123 [22]

Answer:

1.2   ( two significant digits)

Explanation:

5.4 - 4.21        answer should only have the the number of significant digits as the number in the equation with the least number of significant digits... in this case   5.4   is only two significant digits....so the answer should only have two significant digits

5.4 - 4.21 = 1.19     round to two digits = 1.2    

3 0
11 months ago
Sulfur and oxygen react to produce sulfur trioxide. In a particular experiment, 7.9 grams of SO3 are produced by the reaction of
shutvik [7]

Answer:

  • <u>79%</u>

Explanation:

<u>1) Balanced chemical equation:</u>

  • 2S + 3O₂ → 2SO₃

<u>2) Mole ratio:</u>

  • 2 mol S : 3 mol O₂ : 2 mol SO₃

<u>3) Limiting reactant:</u>

  • Number of moles of O₂

        n = 6.0 g / 32.0 g/mol = 0.1875 mol O₂

  • Number of moles of S:

         n = 7.0 g / 32.065 g/mol = 0.2183 mol S

  • Ratios:

        Actual ratio: 0.1875 mol O₂ / 0.2183 mol S =0.859

        Theoretical ratio: 3 mol O₂ / 2 mol S = 1.5

Since there is a smaller proportion of O₂ (0.859) than the theoretical ratio (1.5), O₂ will be used before all S be consumed, and O₂ is the limiting reactant.

<u>4) Calcuate theoretical yield (using the limiting reactant):</u>

  • 0.1875 mol O₂ / x = 3 mol O₂ / 2 mol SO₃

  • x = 0.1875 × 2 / 3 mol SO₃ =  0.125 mol SO₃

<u>5) Yield in grams:</u>

  • mass = number of moles × molar mass = 0.125 mol × 80.06 g/mol =  10.0 g

<u>6) </u><em><u>Percent yield:</u></em>

  • Percent yield, % = (actual yield / theoretical yield) × 100
  • % = (7.9 g / 10.0 g) × 100 = 79%
6 0
3 years ago
Other questions:
  • What is a isotope ?
    15·2 answers
  • Which of these is an acid?
    9·1 answer
  • What would happen if Phosphorus disappeared?
    10·1 answer
  • Which of the following statements is true?
    7·1 answer
  • In the same condition, what happens to the net force acting on the rope?
    7·1 answer
  • 1) The densities of air at −85°C, 0°C, and 100°C are 1.877 g dm−3, 1.294 g dm−3, and 0.946 g dm−3, respectively. From these data
    8·1 answer
  • Which statement would support a merit of the Bronsted-Lowry base theory has over the Arrhenius base theory?
    6·2 answers
  • "in an ionic compound, the size of the ions affects the internuclear distance (the distance between the centers of adjacent ions
    11·2 answers
  • An object's _______ depends on gravity, but an object's _______ does not. A. volume; density B. mass; weight C. weight; mass D.
    7·2 answers
  • What is the pOH of a substance with a Hydrogen concentration of 3.45 x 10-9. suppose to be a small 9
    8·2 answers
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!