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3 years ago

9

PLEASE HELP!!!

2 answers:

Nataly [62]3 years ago

7 0

1. research question
2. background research
3. hypothesis
4. <span>Controlled experiment
5. data analysis
6. data collection
7. conclusion</span>

Nana76 [90]3 years ago

3 0

Answer:

Step 1. Asking a research question

Step 2. Do background research

Step 3. Propose a hypothesis

Step 4. Perform Controlled experiment

Step 5. Collection of data

Step 6. Analysis of data

Step 7. Conclusion

Explanation:

A scientific method is a systematic approach to understand and explain the natural phenomenon.

The method includes the steps which should be followed in the sequence which begins with making an observation thorough senses, asking questions which could be answered, doing background research and proposing a well-educated guess called hypothesis which could be tested.

Then the experiment is performed to test the hypothesis which provides results which could be collected and analysed. Conclusions, are drawn from the results and must be communicated to the scientific community for verification.

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3 years ago

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3 years ago

A 5.325g sample of methyl benzoate, a compound in perfumes , was found to contain 3.758 g of carbon, 0.316 g of hydrogen, and 1.

Alexxandr [17]

<u>Answer:</u> The empirical and molecular formula of the compound is $C_4H_4O$ and $C_8H_8O_2$ respectively

<u>Explanation:</u>

We are given:

Mass of C = 3.758 g

Mass of H = 0.316 g

Mass of O = 1.251 g

To formulate the empirical formula, we need to follow some steps:

<u>Step 1:</u> Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{3.758g}{12g/mole}=0.313moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.316g}{1g/mole}=0.316moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{1.251g}{16g/mole}=0.078moles$

<u>Step 2:</u> Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.078 moles.

For Carbon = $\frac{0.313}{0.078}=4.01\approx 4$

For Hydrogen = $\frac{0.316}{0.078}=4.05\approx 4$

For Oxygen = $\frac{0.078}{0.078}=1$

<u>Step 3:</u> Taking the mole ratio as their subscripts.

The ratio of C : H : O = 4 : 4 : 1

The empirical formula for the given compound is $C_4H_4O$

For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is:

$n=\frac{\text{Molecular mass}}{\text{Empirical mass}}$

We are given:

Mass of molecular formula = 130 g/mol

Mass of empirical formula = 68 g/mol

Putting values in above equation, we get:

$n=\frac{130g/mol}{68g/mol}=1.9\approx 2$

Multiplying this valency by the subscript of every element of empirical formula, we get:

$C_{(2\times 4)}H_{(2\times 4)}O_{(2\times 2)}=C_8H_8O_2$

Hence, the empirical and molecular formula of the compound is $C_4H_4O$ and $C_8H_8O_2$ respectively

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3 years ago

What is the most basic building block of matter?

Viefleur [7K]

Answer would be A)the atom

7 0

3 years ago

Read 2 more answers

Which element is a liquid at 305 K and 1.0 atm

Svetradugi [14.3K]

Your answer is Gallium.

Hope this helps (:

7 0

4 years ago