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ELEN [110]
3 years ago
10

Which of these equations best summarizes photosynthesis?

Chemistry
1 answer:
elena-14-01-66 [18.8K]3 years ago
7 0

Answer: C

Explanation:

                                              Sunlight

6 CO2       +          6 H2O   -------------->            C6H12O6    +        6 O2

                                            Chlorophyll

Carbon(IV)oxide   Water                               Glucose              Oxygen

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Rust is a compound with the formula F e 2 O 3 . Which elements combine to form rust?
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Remembering the periodic table, Fe is iron and O is oxygen. The elements that combine to create rust are iron and oxygen, with the chemical compound being (Iron)2(Oxygen)3.
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in this cut-away image of an atom, where is the red arrow most likely pointed at the greatest probability of locating an electro
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Answer:

c

Explanation:

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How many grams of sulfuric acid is needed to neutralize 380 ml of solution with pH = 8.94
erma4kov [3.2K]

Answer : The mass of sulfuric acid needed is 16.23\times 10^{-5}g.

Solution : Given,

pH = 8.94

Volume of solution = 380 ml = 380\times 10^{-3}      (1ml=10^{-3}L)

Molar mass of sulfuric acid = 98.079 g/mole

As we know,

pH+pOH=14\\pOH=14-8.94=5.06

pOH=-log[OH^-]

5.06=-log[OH^-]

[OH^-]=0.00000871=8.71\times 10^{-6}mole/L

Now we have to calculate the moles of OH^-.

Formula used : Moles=Concentration\times Volume

\text{ Moles of }[OH^-]=\text{ Concentration of }[OH^-]\times Volume\\\text{ Moles of }[OH^-]=(8.71\times 10^{-6}mole/L)\times (380\times 10^{-3}L)=3309.8\times 10^{-9}moles

For neutralization, equal number of moles of H^+ ions will neutralize same number of OH^- ions.

\text{ Moles of }[OH^-]=\text{ Moles of }[H^+]=3309.8\times 10^{-9}moles

As, H_2SO_4\rightarrow 2H^++SO^{2-}_4

From this reaction, we conclude that

2 moles of H^+ ion is given by the 1 mole of H_2SO_4

3309.8\times 10^{-9} moles of H^+ ion is given by \frac{3309.8\times 10^{-9}}{2}=1654.9\times 10^{-9} moles of H_2SO_4

Now we have to calculate the mass of sulfuric acid.

Mass of sulfuric acid = Moles of H_2SO_4 × Molar mass of sulfuric acid

Mass of sulfuric acid = (1654.9\times 10^{-9}moles)\times (98.079g/mole)=162310.94\times 10^{-9}=16.23\times 10^{-5}g

Therefore, the mass of sulfuric acid needed is 16.23\times 10^{-5}g.

3 0
3 years ago
Zirconium has an atomic number of 40, And an atomic mass of 91. How many electrons does zirconium have?
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Answer: 40

Explanation: Whatever the atomic number is, that’s also the number of electrons and protons.
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Caffeine, a stimulant found in coffee, tea, and certain soft drinks, contains C, H, O, and N. Combustion of 1.000 mg of caffeine
Yuliya22 [10]

Answer:

  • <u>194 g/mol</u>

Explanation:

<u>1) Content of C:</u>

All the C atoms in the 1.000 mg of caffeine will be found in the 1.813 mg of CO₂.

  • Mass of C in 1.813 mg of CO₂

       Since the atomic mass of C is 12.01 g/mol and the molar of of CO₂ is 44.01, there are 12 mg of C in 44 mg of CO₂ and you can set the proporton:

       12.01 mg C / 44.01 mg CO₂ = x / 1.813 g CO₂

        ⇒ x = 1.813 × 12.01 / 44.01 g of C = 0.49475 mg of C

  • Number of moles of C

      number of moles = mass in g / atomic mass = 0.49475×10⁻³ g / 12.01 g/mol = 4.1195×10⁻⁵ moles = 0.041195 milimol

<u>2) Content of H</u>

All the H atoms in the 1.000 mg of caffeine will be found in the 0.4639 mg of H₂O

  • Mass of H in 0.4639 mg of H₂O

       Since the atomic mass of H is 1.008 g/mol and the molar of of H₂O is 18.015 g/mol, there are 2×1.008 mg of H in 18.015 mg of H₂O and you can set the proporton:

       2×1.008 mg H / 18.015 mg H₂O = x / 0.4639 mg H₂O

        ⇒ x = 0.4639 mg H₂O × 2 × 1.008 mg H / 18.015 mg H₂O = 0.051913 mg H

  • Number of moles of H

      number of moles = mass in g / atomic mass = 0.051913 ×10⁻³ g / 1.008 g/mol = 5.1501× 10⁻⁵ moles = 0.051501 milimol

<u>3) Content of N</u>

All the N atoms in the 1.000 mg of caffeine will be found in the 0.2885 mg of N₂

  • Mass of N in 0.2885 mg of N₂ is 0.2885 mg

  • Number of moles of N

      number of moles = mass in g / atomic mass = 0.2885 ×10⁻³ g / 14.007 g/mol = 2.0597× 10⁻⁵ moles = 0.020597 milimol

<u>4) Content of O</u>

The mass of O is calculated by difference:

  • Mass of O = mass of sample - mass of C - mass of H - mass of N

       Mass of O = 1.000 mg - 0.49475 mg C - 0.051913 mg H - 0.2885 mg N

     Mass of O = 0.1648 mg

  • Moles of O =  0.1648 × 10 ⁻³ g / 15.999 g/mol = 1.0303×10⁻⁵ mol = 0.01030 milimol

<u>5) Ratios</u>

Divide every number of mililmoles by the smallest number of milimoles:

  • C:  0.041195 / 0.01030 = 4
  • H: 0.051501 / 0.01030 = 5
  • N: 0.020597 / 0.01030 = 2
  • O: 0.01030 / 0.01030 = 1

  • C: 4
  • H: 5
  • N: 2
  • O: 1

<u>6) Empirical formula:</u>

  • C₄H₅N₂O₁

<u>7) Calculate the approximate mass of the empirical formula:</u>

  • 4 × 12 + 5 × 1 + 2 × 14 + 1 × 16 =  97 g/mol

So, since that number is not between 150 and 200 g/mol, multiply by 2: 97 × 2 = 194, which is between 150 and 200.

Thus, the estimate is 194 g/mol

7 0
3 years ago
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