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3 years ago

PLEASE HELP ME WITH A COUPLE OF QUESTIONS!!! Thank You :)

1 answer:

5 0

Hey there!

1. A chemical reaction is, B). Any time different substances combine to form a new substance, or when a substance breaks up into different substances

2. Balancing chemical equations is called, C). Equivalentry

3. Sulfuric acid is made of two hydrogen atoms (H), one sulfur atom (5), and four oxygen atoms (0). What is its formula? C). H2S04

Hope this helps!

-Much love, Makayla

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Match each item to its proper disposal method. Answers to be used more than once.

salantis [7]

Answer:

1. a)

2. a)

3. b)

4. d)

Explanation:

The disposal method is how we throw away the wastes. In a chemical lab, the correct disposal method guarantees the security of the environment and the humans and animals that may be in contact with the materials.

So:

1. Excess chemical: Because it can be toxic, it may be disposed of in the appropriate waste container, which will depend on the characteristics of the material;

2. Reaction mixture: As the excess chemical, it can be toxic, so it must be disposed of at an appropriate waste container;

3. Used filter paper: Generally, the solids in the filter paper is not toxic, so it can be thrown away in the trash can;

4. Cracked or chipped beaker: Because the beaker is made of glass, it can cut when broken, so it must go to a broken glass box, that will protect the people that will deal with it.

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3 years ago

Some hidden evidence can be seen with this type of light

Tatiana [17]

You Would Need A(n) Blacklight Or AKA UV Light

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3 years ago

Determine the percent yield forthe reaction between 82.4 g of Rband 11.6 g of O2 if 39.7 g of Rb2Ois produced

Mazyrski [523]

Step 1

The reaction is written and balanced:

4 Rb + O2 =>2 Rb2O

-----------

Step 2

Define % yield of product (Rb2O) = (Actual yield/Theoretical yield) x 100

The actual yield is provided by the exercise = 39.7 g

----------

Step 3

Determine the limiting reactant. The molar masses are needed to solve this:

For Rb) 85.4 g/mol

For O2) 32 g/mol

Procedure:

4 Rb + O2 =>2 Rb2O

4 x 85.4 g Rb ----- 32 g O2

82.4 g Rb ----- X = 7.72 g O2 are needed

For 82.4 g Rb, 7.72 g O2 is needed, but there is 11.6 g O2. Therefore, O2 is the excess agent. Rb is the limiting reactant.

--------

Step 4

Determine the theoretical yield from the limiting reactant:

The molar mass Rb2O) 187 g/mol

Procedure:

4 x 85.4 g Rb ------ 2 x 187 g Rb2O

82.4 g Rb ------ X = 90.2 g Rb2O = Theoretical yield

---------

Step 5

% yield = Actual y./Theoretical y. x 100 = (39.7 g/90.2 g) x 100 = 44 % approx.

Answer: % yield = 44 %

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1 year ago

Which compound does a plant absorb during photosynthesis?

andrey2020 [161]

Answer:

B. all the above no wrong answer

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3 years ago

Read 2 more answers

Write a method that could be used to produce pure crystals of copper chloride from copper oxide and hydrochloric acid.

joja [24]

- Describe how you would make the salt from the reactants.

CuO + 2 HCl → CuCl₂ + H₂O

- Describe how you would purify the salt from the reaction mixture.

Filter the solution and let the product crystallize.

Explanation:

The reaction between copper oxide (CuO) and hydrochloric acid (HCl) will produce copper chloride (CuCl₂) and water:

CuO + 2 HCl → CuCl₂ + H₂O

-Describe how you would make the salt from the reactants

In a beaker which contain cooper oxide add the hydrochloric acid. To avoid working with concentrated hydrochloric acid, the acid may be diluted with water but make sure the add the stoechiometric amount (and a little bit of excess) in respect with the copper oxide.

-Describe how you would purify the salt from the reaction mixture.

Let the reaction proceed and then filter the solution to remove the unreacted cooper oxide.

Let the filtered solution, which contain copper chloride, water and unreacted hydrochloric acid, to stand undisturbed for several days. You may see the crystals growing from the solution. To speed up the process you may reduce the temperature.

Learn more about:

purifying compounds

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#learnwithBrainly

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3 years ago