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PolarNik [594]
3 years ago
15

Which of the following numbers is in scientific notation?

Chemistry
1 answer:
Paha777 [63]3 years ago
6 0
C is the correct answer
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What is the hydrogen ion (H+) concentration of a solution of pH 8?
fgiga [73]

Answer:

10−8 M.

Explanation:

In this problem we are given pH and asked to solve for the hydrogen ion concentration. Using the equation, pH = − log [H+] , we can solve for [H+] as,

− pH = log [H+] ,

[H+] = 10−pH,

by exponentiating both sides with base 10 to "undo" the common logarithm. The hydrogen ion concentration of blood with pH 7.4 is,

[H+] = 10−7.4 ≈ 0.0000040 = 4.0 × In this problem we are given pH and asked to solve for the hydrogen ion concentration. Using the equation, pH = − log [H+] , we can solve for [H+] as,

− pH = log [H+] ,

[H+] = 10−pH,

by exponentiating both sides with base 10 to "undo" the common logarithm. The hydrogen ion concentration of blood with pH 7.4 is,

[H+] = 10−7.4 ≈ 0.0000040 = 4.0 × 10−8 M.

3 0
3 years ago
Read 2 more answers
Gaseous methane (CH4) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO) and gaseous water (H2O) . Suppo
Leto [7]

Answer:

0 g.

Explanation:

Hello,

In this case, since the reaction between methane and oxygen is:

CH_4+2O_2\rightarrow CO_2+2H_2O

If 0.963 g of methane react with 7.5 g of oxygen the first step is to identify the limiting reactant for which we compute the available moles of methane and the moles of methane consumed by the 7.5 g of oxygen:

n_{CH_4}=0.963gCH_4*\frac{1molCH_4}{16gCH_4}=0.0602molCH_4\\ \\n_{CH_4}^{consumed}=7.5gO_2*\frac{1molO_2}{32gO_2}*\frac{1molCH_4}{2molO_2} =0.117molCH_4

Thus, since oxygen theoretically consumes more methane than the available, we conclude the methane is the limiting reactant, for which it will be completely consumed, therefore, no remaining methane will be left over.

left\ over=0g

Regards.

7 0
3 years ago
Which of the following can form a hydrogen bond with the HF molecule?
Lostsunrise [7]

Answer:

helium

(He)

Explanation:

helium

(He)

6 0
3 years ago
How many moles of carbon dioxide gas should be produced when 10.0 g of C2H6 are combusted at STP?
Finger [1]

Answer:

                    0.665 moles of CO₂

Explanation:

                     The balance chemical equation for the combustion of Ethane is as follow:

                            2 C₂H₆ + 7 O₂ → 4 CO₂ + 6 H₂O

Step 1: <u>Calculate moles of C₂H₆ as;</u>

                              Moles  =  Mass  /  M.Mass

Putting values,

                              Moles  =  10.0 g / 30.07 g/mol

                              Moles  =  0.3325 moles

Step 2: <u>Calculate Moles of CO₂ as;</u>

According to balance chemical equation,

                    2 moles of C₂H₆ produced  =  4 moles of CO₂

So,

             0.3325 moles of C₂H₆ will produce  =  X moles of CO₂

Solving for X,

                      X  =  0.3325 mol × 4 mol ÷ 2 mol

                      X = 0.665 moles of CO₂

3 0
3 years ago
What occurs when Cr^3+ ions are reduced to Cr^2+ ions?
DiKsa [7]
D:

When electrons are gained, the charge of the atom decreases.

When you are given an atom with a charge, the oxidation of that atom is the charge. So by going from a Cr^3+ (Oxidation Number = 3) to a Cr^2+ (Oxidation Number = 2), the Oxidation Number thus decreases.
7 0
3 years ago
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