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jekas [21]
3 years ago
11

6PbO + O2 → 2Pb304 a. How many grams of Pb304 are produced from 8.50 grams of lead(II) oxide?

Chemistry
1 answer:
AlladinOne [14]3 years ago
7 0

Answer:

8.70g of Pb3O4

Explanation:

6PbO + O2 → 2Pb3O4

Molar Mass of PbO = 207 + 16 = 223g/mol

The mass of the PbO from the balanced equation = 6 x 223 = 1338g

Molar Mass of Pb3O4 = (3x207) +(16x4) = 621 + 64 = 685g/mol

Mass of Pb3O4 from the balanced equation = 2 x 685 = 1370g

From the equation,

1338g oh PbO produced 1370g of Pb3O4.

Therefore, 8.50g of PbO will produce = (8.5 x 1370)/1338 = 8.70g of Pb3O4

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Calculate [H3O+] and [OH−] for each of the following solutions at 25 ∘C given the pH. pH= 8.74, pH= 11.38, pH= 2.81
Gnom [1K]

Answer:

Explanation:

Given parameters;

pH  = 8.74

pH = 11.38

pH = 2.81

Unknown:

concentration of hydrogen ion and hydroxyl ion for each solution = ?

Solution

The pH of any solution is a convenient scale for measuring the hydrogen ion concentration of any solution.

It is graduated from 1 to 14

      pH = -log[H₃O⁺]

      pOH = -log[OH⁻]

 pH + pOH = 14

Now let us solve;

   pH = 8.74

             since  pH = -log[H₃O⁺]

                           8.74 =  -log[H₃O⁺]

                           [H₃O⁺] = 10⁻^{8.74}

                             [H₃O⁺]  = 1.82 x 10⁻⁹mol dm³

       pH + pOH = 14

                 pOH = 14 - 8.74

                  pOH = 5.26

                  pOH = -log[OH⁻]

                     5.26  = -log[OH⁻]

                     [OH⁻] = 10^{-5.26}

                      [OH⁻] = 5.5 x 10⁻⁶mol dm³

2.  pH = 11.38

             since  pH = -log[H₃O⁺]

                           11.38 =  -log[H₃O⁺]

                           [H₃O⁺] = 10⁻^{11.38}

                             [H₃O⁺]  = 4.17 x 10⁻¹² mol dm³

           pH + pOH = 14

                 pOH = 14 - 11.38

                  pOH = 2.62

                  pOH = -log[OH⁻]

                     2.62  = -log[OH⁻]

                     [OH⁻] = 10^{-2.62}

                      [OH⁻] =2.4 x 10⁻³mol dm³

3. pH = 2.81

             since  pH = -log[H₃O⁺]

                           2.81 =  -log[H₃O⁺]

                           [H₃O⁺] = 10⁻^{2.81}

                             [H₃O⁺]  = 1.55 x 10⁻³ mol dm³

           pH + pOH = 14

                 pOH = 14 - 2.81

                  pOH = 11.19

                  pOH = -log[OH⁻]

                     11.19  = -log[OH⁻]

                     [OH⁻] = 10^{-11.19}

                      [OH⁻] =6.46 x 10⁻¹²mol dm³

5 0
3 years ago
g This plot shows the rate of the decomposition of SO2Cl2 into SO2 and Cl2 as a function of the concentration of SO2Cl2. What is
scoundrel [369]

Answer:

When n = 1, the reaction is of the First Order

Explanation:

Find attach the solution

5 0
3 years ago
How do you do this?
Alona [7]
It would be Atom 2 because the proton and neutron are both nine and the election is 8 which is -1 to nine <span />
7 0
3 years ago
If a plant produces 8.46 mol C6H12O6, how many moles of H2O are needed?
Ierofanga [76]

Answer:

50.76 mol H2O.

Explanation:

The photosynthesis follows the equation:

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

This means that 6 mol of H2O are needed to obtain 1 mol of C6H12O6 (see the numbers that precedes every molecule to know how many mols are in game).

So we can say that:

1 mol C6H12O6 --------- 6 mol H2O

8.46 mol C6H12O6 -----x= 8.46 x 6 : 1 = 50.76 mol H20

8 0
3 years ago
Which chemical formula shows two atoms of iron (Fe) and three atoms of oxygen (O)?
Taya2010 [7]
Fe  O
 2    3 is what i would put
5 0
3 years ago
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