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Andru [333]
4 years ago
6

one of the isotopes of sulfur is represented as sulfur -35 or S-35. what does the number 35 signify?

Chemistry
2 answers:
Temka [501]4 years ago
6 0
35 is equal to it's mass number
SpyIntel [72]4 years ago
4 0

Answer: If using plato the answer is D Mass number

Explanation:

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Which atom has a change of oxidation number of +4 in the pictured redox reaction?
SpyIntel [72]

Answer:

The answer to your question is the letter d. S

Explanation:

Data

Change of +4 in the oxidation number

Chemical reaction

               K₂Cr₂O₇  +  H₂O  +  S  ⇒   KOH  +  Cr₂O₃  +  SO₂    

Process

1.- Calculate the oxidation numbers following the rules.

Some rules

  H = +1       O = -2    Alkali metals = + 1    Alkali earth metals = +2    

K₂⁺¹Cr₂⁺⁶O₇⁻²  +  H₂⁺¹O⁻²  +  S⁰  ⇒   K⁺¹O⁻²H⁺¹  +  Cr₂⁺³O₃⁻²  +  S⁺⁴O₂⁻²    

Elements that changed their oxidation numbers

                       Cr₂⁺⁶   ---------------- Cr₂⁺³

                       S⁰       --------------- S⁺⁴

                     

 

3 0
3 years ago
Which particle has the most energy? A) ice Eliminate B) water C) steam D) there is no difference in particle energy
d1i1m1o1n [39]
Steam, being in gas form, has the highest energy as particles have more kinetic energy and they move more vigorously than in ice or water that are in solid and liquid form respectively.
3 0
3 years ago
Read 2 more answers
Iron(II) sulfide has a molar mass of 87.91 g/mol. 50 grams of
dimaraw [331]

Answer:

true

Explanation:

7 0
3 years ago
Read 2 more answers
What is the frequency of light with an energy of 124 kJ/mol?
Charra [1.4K]

Answer: = 3.11 x 10^14 s^-1

Explanation:

Use the formula E = hv

This formula uses the assumption that the unit for energy is in Joules/photon.

124 kJ = 124000J

To get 124000J/mol into a unit of J/photons, we need to divide by the number of photons in a mole, which is 6.022 x 10^23.

And thus, we need

124000/6.022 x 10^23 = 2.06 x 10^-19J/photon

We can plug it in to E = hv by

2.06 x 10^-19J = (6.63 x 10^-34 J s)(v) Isolate v by

v = (2.06 x 10^-19J)/(6.63 x 10^-34 J s)

= 3.11 x 10^14 s^-1

6 0
3 years ago
1. Perform calculations to determine the amount of 6.00x10-5 M stock solution needed to prepare 20.00 mL of 2.00x10-5 M dye solu
zhannawk [14.2K]

Answer:

1a. 6.70 ml of stock dye solution is required

1b. 10.0 ml of stock dye solution is required

1c. 4.00 ml of stock dye solution is required

Explanation:

1a. Using m₁v₁ = m₂v

6.00 * 10⁻⁵ * v₁ = 20.0 * 2.00 * 10⁻⁵

v₁ = 4 * 10⁻⁴/6.00 * 10⁻⁵

v₁ = 6.70 mL of stock solution

Therefore, 6.70 ml of stock dye solution is required

b. Using m₁v₁ = m₂v

2.00 * 10⁻⁵ * v₁ = 20.0 * 1.00 * 10⁻⁵

v₁ = 2 * 10⁻⁴/2.00 * 10⁻⁵

v₁ = 10.0 mL of stock solution

Therefore, 10.0 ml of stock dye solution is required

c. Using m₁v₁ = m₂v

1.00 * 10⁻⁵ * v₁ = 20.0 * 2.00 * 10⁻⁶

v₁ = 4 * 10⁻⁵/1.00 * 10⁻⁵

v₁ = 4.00 mL of stock solution

Therefore, 4.00 ml of stock dye solution is required

The procedure is then followed as in steps 2 to 4.

4 0
3 years ago
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