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____ [38]
3 years ago
8

PLEAE HELP! I am stuck on this question.

Chemistry
1 answer:
NikAS [45]3 years ago
7 0
1)general or nonspecific observation- Qaulitative
2)educated guess- hypothesis
4)measured observation- quantitative
5)standard reference data or experiment-control
6)a presently accepted explanation of how something happens-law
8) a curve drawn to average delvations- best fit curve

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SEDIMENTARY ROCK

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What phases can carbon dioxide exist?​
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Carbon dioxide is a gas at room temperature

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Answer fast and I’ll give BRAINLIEST please and thank you!! IT WOULD HELP ALOT IF U DONT RUSH AND ANSWER CORRECTLY
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3 years ago
You are assigned the task of separating a desired granular material, with a density of 3.26 g/cm3, from an undesired granular ma
Svetradugi [14.3K]

Answer:

diiodomethane

Explanation:

The densities of each of the liquids mentioned in the question are stated below;

CCl4- 1.59 g/cm^3

Hexane- 0.672 g/cm^3

Benzene- 0.8765 g/cm^3

Diiodomethane- 3.3 g/cm^3

Clearly, the density of diiodomethane methane is almost the same as that of the desired granular material, hence the undesired granular material having a density of 2.04 g/cm3 will float in diiodomethane thus separating the two granular materials.

5 0
3 years ago
A 0.4657 g sample of a pure soluble bromide compound is dissolved in water, and all of the bromide ion is precipitated as AgBr b
Yanka [14]

Answer:

The mass percentage of bromine in the original compound is 81,12%

Explanation:

<u>Step 1: Calculate moles AgBr</u>

moles AgBr = mass AgBr / molar mass  AgBr

= 0.8878 g / 187.77 g/mol

= 0.00472812 moles AgBr

⇒

Since 1 mol AgBr contains 1 mol Br-

Then the amount of moles Br- in the original sample must also have  been 0.00472812 moles

<u>Step 2:</u> Calculating mass Br-

mass Br- = molar mass Br x moles  Br-

= 79.904 g/mol x 0.00472812 mol

= 0.377796 g Br-

⇒

There were 0.377796 g Br- in the original sample

<u>Step 3:</u> Calculating mass percentage Br-

⇒mass percentage  = actual mass Br- / total mass x 100%

% mass Br = 0.377796 g / 0.4657 g x 100  %

= 81.12%

7 0
3 years ago
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