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Sergio039 [100]
3 years ago
7

Convert 55.6 km to m show equation

Chemistry
2 answers:
Lisa [10]3 years ago
8 0

Answer:

55,600 meters

Explanation:

1km=1,000 meters

55.6km= 55,600 meters

crimeas [40]3 years ago
5 0

Explanation:

1 km = 1000m

55.6 km = x m

x = 55.6*1000

x = 55600m

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3 years ago
Consider the reaction below. 2Al2O3 4Al + 3O2 What is the mole ratio of oxygen to aluminum?
DiKsa [7]
The answer is 3/4.

The coefficient next to each reactant represents the amount of moles. The compound for oxygen is O2 and the compound for aluminum is 4. We can see that the number next to O2 is 3 and the number next to aluminum is 4.
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3 years ago
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Calculate the density of sulfuric acid from the information that 35.4 mL of the acid masses 65.14 g.
vladimir1956 [14]

Answer:

<h3>The answer is 1.84 g/mL</h3>

Explanation:

The density of a substance can be found by using the formula

density =  \frac{mass}{volume}  \\

From the question we have

density =  \frac{65.14}{35.4}  \\  = 1.840112994...

We have the final answer as

<h3>1.84 g/mL</h3>

Hope this helps you

3 0
2 years ago
What is the pH of a solution with a 3.8 × 10−4 M hydronium ion concentration?
mamaluj [8]

Answer:

3.4

Explanation:

The pH scale is used to express the acidity or basicity of a solution.

  • If the pH < 7, the solution is acid.
  • If the pH = 7, the solution is neutral.
  • If the pH > 7, the solution is basic.

Given the hydronium ion concentration [H₃O⁺] = 3.8 × 10⁻⁴ M, we can calculate the pH using the following expression.

pH = -log [H₃O⁺]

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8 0
2 years ago
Bromine has two isotopes 79Br and 81Br, whose masses (78.9183 and 80.9163 amu) and abundances (50.69% and 49.31%, respectively)
Reika [66]

Answer:

Average atomic mass = 79.9034 amu

Explanation:

The formula for the calculation of the average atomic mass is:

Average\ atomic\ mass=(\frac {\%\ of\ the\ first\ isotope}{100}\times {Mass\ of\ the\ first\ isotope})+(\frac {\%\ of\ the\ second\ isotope}{100}\times {Mass\ of\ the\ second\ isotope})

Given that:

<u>For first isotope: </u>

% = 50.69 %

Mass = 78.9183 amu

<u>For second isotope: </u>

% = 49.31 %

Mass = 80.9163 amu

Thus,  

Average\ atomic\ mass=\frac{50.69}{100}\times {78.9183}+\frac{49.31}{100}\times {80.9163}\ amu

Average\ atomic\ mass=40.0036+39.8998\ amu

<u>Average atomic mass = 79.9034 amu</u>

4 0
3 years ago
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