When you are doing a experiment, you are testing if your hypothesis is correct or false. If your hypothesis is false, you have to disgard it. If it is correct, you have to do many more parallels, and if they also confirm your hypothesis, your hypothesis can become a theory.

8 0

3 years ago

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An object has a density that is greater than the density of water. How could you make it float? Explain by giving a real-life ex

vladimir1956 [14]

Answer:

Put it on a ship or an aerogel

Explanation:

You can use an aerogel, a synthetic porous ultralight material. The aerogel can support a mass many times greater than their own.

Even simpler, you can put the object on board a ship. The ship has a smaller density than water, making it float in water.

5 0

3 years ago

Ammonium perchlorate is the solid rocket fuel used by the U.S. Space Shuttle. It reacts with itself to produce nitrogen gas , ch

Zinaida [17]

Answer:

2.9 g

Explanation:

There is some info missing. I think this is the original question.

Ammonium perchlorate is the solid rocket fuel used by the U.S. Space Shuttle. It reacts with itself to produce nitrogen gas, chlorine gas, oxygen gas, water, and a great deal of energy.

What mass of water is produced by the reaction of 9.6 g of ammonium perchlorate?

Step 1: Given data

Mass of ammonium perchlorate: 9.6 g

Step 2: Write the balanced equation

2 NH₄ClO₄(s) → N₂(g) + Cl₂(g) + 2 O₂(g) + 4 H₂O(l)

Step 3: Calculate the moles corresponding to 9.6 g of ammonium perchlorate

The molar mass of ammonium perchlorate is 117.49 g/mol.

$9.6 g \times \frac{1mol}{117.49 g} = 0.082mol$

Step 4: Calculate the moles of water formed from 0.082 moles of ammonium perchlorate

The molar ratio of NH₄ClO₄ to H₂O is 2:4. The moles of water formed are 4/2 × 0.082 mol = 0.16 mol

Step 5: Calculate the mass corresponding to 0.16 moles of water

The molar mass of water is 18.02 g/mol.

$0.16 mol \times \frac{18.02g}{mol} = 2.9 g$

3 0

3 years ago