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3 years ago

Put the following steps of the scientific method in order. #1 - 6

Chemistry

1 answer:

exis [7]3 years ago

6 0

Answer:

ask a question

research the question

make a hypothesis

do the experiment

collect and record data

arrive at a conclusion

Explanation:

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Tin(IV) sulfide, SnS2, a yellow pigment, can be produced using the following reaction.

Maksim231197 [3]

The theoretical yield of $SnS_2$ will be 4.20 grams while the percent yield will be 7.93%

<h3>How is yield calculated?</h3>

From the equation of the reaction, the mole ratio of $SnBr_4$ to $Na_2S$ is 1:2.

Mole of 48.1 mL, 0.478 M $SnBr_4$ = 0.478 x 48.1/100 = 0.023 mols

Mole of 48.8 mL, 0.160 M $Na_2S$ = 0.160 x 48.8/1000 = 0.0078 moles

$SnBr_4$ $Na_2S$ is the limiting reactant.

Mole ratio of $SnBr_4$ and $SnS_2$ = 1:1

Equivalent mole of $SnS_2$ = 0.023 moles

Mass of 0.023 noles $SnS_2$ = 0.023 x 182.81 = 4.20 grams

With 0.0333 g of $SnS_2$ recovered, percent yield = 0.333/4.2 x 100 = 7.93%

More on yields of reactions can be found here: brainly.com/question/17042787

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Tin(IV) sulfide, SnS2, a yellow pigment, can be produced using the following reaction.

SnBr4(aq)+2Na2S(aq)⟶4NaBr(aq)+SnS2(s)

Suppose a student adds 48.1 mL of a 0.478 M solution of SnBr4 to 48.8 mL of a 0.160 M solution of Na2S.

1) Calculate the theoretical yield of SnS2. ;

2) The student recovers 0.333 g of SnS2. Calculate the percent yield of SnS2 that the student obtained.

7 0

2 years ago

Every Methane molecule looks different. True or false?

Akimi4 [234]

Answer:

False

Explanation:

Molecules of the same substance are made up of the same type of atoms and look exactly alike.

Hence, if I have two molecules of methane having exactly the same atoms of carbon and hydrogen,the both are indistinguishable from each other based on appearance.

Hence all molecules of methane are exactly alike if they are composed of atoms of the same isotope of hydrogen and carbon.

8 0

4 years ago

Calculate the wavelength of the photon emitted when an electron makes a transition from n=6 to n=3. You can make use of the foll

Angelina_Jolie [31]

<u>Answer:</u> The wavelength of light is $1.094\times 10^{-6}m$

<u>Explanation:</u>

To calculate the wavelength of light, we use Rydberg's Equation:

$\frac{1}{\lambda}=R_H\left(\frac{1}{n_f^2}-\frac{1}{n_i^2} \right )$

Where,

$\lambda$ = Wavelength of radiation

$R_H$ = Rydberg's Constant = $1.097\times 10^7m^{-1}$

$n_f$ = Final energy level = 3

$n_i$ = Initial energy level = 6

Putting the values in above equation, we get:

$\frac{1}{\lambda }=1.097\times 10^7m^{-1}\left(\frac{1}{3^2}-\frac{1}{6^2} \right )\\\\\lambda =\frac{1}{914617m^{-1}}=1.094\times 10^{-6}m$

Hence, the wavelength of light is $1.094\times 10^{-6}m$

6 0

4 years ago

Is hydrogen sulfide a heterogeneous mixture solution compound or element?

AleksandrR [38]

Hydrogen sulfide is a <u>compound</u>

<h3>Explanation</h3>

A compound is a substance composed of two or more element in a fixed proportion and it can be separated into simpler substance and element only by chemical method. Hydrogen sulfide is a chemical compound with H2S formula.

7 0

3 years ago

For the reaction of C 2H 4( g) with O 2( g), to form CO 2( g) and H 2O( g), what number of grams of CO 2 could be produced from

maksim [4K]

Answer:

4.58g of CO₂ could be produced

Explanation:

Based on the reaction:

C₂H₄(g) + 3O₂(g) → 2CO₂(g) + 2H₂O(g)

<em>1 mole of C₂H₄ reacts with 3 moles of oxygen to produce 2 moles of CO₂</em>

<em />

To solve this question we must find the moles of each reactant in order to find limiting reactant. With limiting reactant we can find the moles -And the mass- of CO₂ produced:

<em>Moles C₂H₄ -Molar mass: 28.05g/mol-</em>

2.0g * (1mol / 28.05g) = 0.0713moles

<em>Moles O₂ -Molar mass: 32g/mol-</em>

5.0g * (1mol / 32g) = 0.156moles

For a complete reaction of 0.0713 moles of C2H4 are required:

0.0713 moles C₂H₄ * (3 moles O₂ / 1 mol C₂H₄) = 0.214 moles of O₂

As there are just 0.156 moles, O₂ is limiting reactant.

The moles of CO₂ produced are:

0.156 moles O₂ * (2mol CO₂ / 3mol O₂) = 0.104 moles CO₂

The mass is -Molar mass CO₂: 44.01g/mol-

0.104 moles CO₂ * (44.01g / mol) =

<h3>4.58g of CO₂ could be produced</h3>

4 0

3 years ago