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3 years ago

The role of teeth in the digestive system?

Chemistry

2 answers:

GREYUIT [131]3 years ago

5 0

We use our teeth to chew our food and prepare food to travel through the rest of digestive system

USPshnik [31]3 years ago

4 0

Help saliva and makes food soft and easy to swallow

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Does this particle diagram represent an element, compound, or mixture?

valkas [14]

Answer:

Yes, it's a mixture as more than 1 type of molecules are present!!

6 0

3 years ago

An electrode has a potential of 1.201 V with respect to a saturated silver-silver chloride electrode. What would the electrodes

fredd [130]

Answer:

The potential wrt. calomel is 1.254 V

Explanation:

Given:

Potential wrt. silver chloride $E_{Ag} = 1.201$ V

Potential wrt. saturated silver chloride $E = 0.197$ V

Potential wrt. SCE $E_{Hg} = 0.241$ V

Now potential wrt. hydrogen is given by,

$= 1.201- 0.197$

$= 1.004$ V

And we find for potential wrt. calomel,

$=$ potential wrt. hydrogen + potential wrt. SEC

$= 1.004 +0.241$

$= 1.254$ V

Therefore, the potential wrt. calomel is 1.254 V

7 0

3 years ago

Molybdenum can form a wide series of halide compounds, including four different fluoride compounds. The percent by mass of molyb

azamat

The formula and names of the compounds are:

1. Formula of compound => MoF₃

Name of compound => Molybdenum trifluoride

2. Formula of compound => MoF₄

Name of compound => Molybdenum tetrafluoride

3. Formula of compound => MoF₅

Name of compound => Molybdenum pentafluoride

4. Formula of compound => MoF₆

Name of compound => Molybdenum hexafluoride

1. Determination of the name and formula of the molybdenum fluoride having 63.0% of molybdenum.

Molybdenum (Mo) = 63.0%

Fluorine (F) = 100 – 63 = 37%

<h3>Formula =? </h3>

Mo = 63.0%

F = 37%

Divide by their molar mass

Mo = 63.0 / 96 = 0.656

F = 37 / 19 = 1.947

Divide by the smallest

Mo = 0.656 / 0.656 = 1

F = 1.947 / 0.656 = 3

Therefore,

Formula of compound => MoF₃

Name of compound => Molybdenum trifluoride

2. Determination of the name and formula of the molybdenum fluoride having 56.0% of molybdenum.

Molybdenum (Mo) = 56.0%,

Fluorine (F) = 100 – 56 = 44%

<h3>Formula =? </h3>

Mo = 56%

F = 44%

Divide by their molar mass

Mo = 56 / 96 = 0.583

F = 44 / 19 = 2.316

Divide by the smallest

Mo = 0.583 / 0.583 = 1

F = 2.316 / 0.583 = 4

Therefore,

Formula of compound => MoF₄

Name of compound => Molybdenum tetrafluoride

3. Determination of the name and formula of the molybdenum fluoride having 50.0% of molybdenum.

Molybdenum (Mo) = 50.0%,

Fluorine (F) = 100 – 50 = 50%

<h3>Formula =? </h3>

Mo = 50%

F = 50%

Divide by their molar mass

Mo = 50 / 96 = 0.520

F = 50 / 19 = 2.632

Divide by the smallest

Mo = 0.520 / 0.520 = 1

F = 2.632 / 0.520 = 5

Therefore,

Formula of compound => MoF₅

Name of compound => Molybdenum pentafluoride

4. Determination of the name and formula of the molybdenum fluoride having 46.0% of molybdenum.

Molybdenum (Mo) = 46.0%,

Fluorine (F) = 100 – 46 = 54%

<h3>Formula =? </h3>

Mo = 46%

F = 54%

Divide by their molar mass

Mo = 46 / 96 = 0.479

F = 54 / 19 = 2.842

Divide by the smallest

Mo = 0.479 / 0.479 = 1

F = 2.842 / 0.479 = 6

Therefore,

Formula of compound => MoF₆

Name of compound => Molybdenum hexafluoride

Learn more: brainly.com/question/11185156

7 0

3 years ago

2C8H18 (1) + 2502 (g) --> 16CO2 (g) + 18H2O (g)

Makovka662 [10]

Answer:

One gallon of octane produces approximately 7000 L of carbon dioxide.

Note:

I believe that the mass of octane should have been given as 2661 g. However, I understand that your instructor probably gave you this problem, so I will use 4000 g for the approximate mass of one gallon of octane. You can rework the problem on your own, substituting the correct masses of octane if you wish.

Step1. You must first determine the number of moles that are in 4000 g of octane, using the molar mass of octane. Step 2. Then you must determine the number of moles of carbon dioxide that can be produced by that number of moles of octane, based on the mole ratio between octane and carbon dioxide in the balanced equation. Step 3. Then use the ideal gas law to determine the volume in liters of carbon dioxide that can be formed.

5 0

2 years ago

How many moles of H2SO4 are needed to completely neutralize 0.0164 mol KOH

Vanyuwa [196]

0.0082 You have to equal out the amount of concentration with the unknown

8 0

4 years ago

Read 2 more answers