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icang [17]
3 years ago
7

How is momentum conserved in a Newton's cradle when one steel ball hits the other?

Chemistry
2 answers:
ycow [4]3 years ago
6 0
Momentum is conserved when you pull one ball bearing back in the air before letting it go to hit the others. Think about it. You lift the bearing in the air with all it's weight, thus leading it to build up momentum and conserve it. Then once you release it, it transfers the energy through the other bearings and out onto the other side repeating it's process.<span />
KatRina [158]3 years ago
5 0

All the momentum starts in one ball, and after the collision, it is all in the other ball.

I took the test

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olya-2409 [2.1K]
The answer is head-to-tail joining of monomers. Monomer used in condensation have  two functional groups that combine to form amide and ester linkages. When this reaction occurs, water molecules is removed and that is why it is called a condensation reaction.
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3 years ago
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Empirical formula of C6H10O6
KiRa [710]

Answer:

I don't know.

Explanation:

I actually don't know the answer so I wrote the answer is "I don't know" or simply "I dunno".

7 0
2 years ago
Iron sulfite has the formula?
Mademuasel [1]
Its FeSO3 or iron(iii)sulfite = Fe2(SO3)3
7 0
3 years ago
Number of grams of hydrogen than can be prepared from 6.80g of aluminum​
Anastaziya [24]

Answer:

0.7561 g.

Explanation:

  • The hydrogen than can be prepared from Al according to the balanced equation:

<em>2Al + 6HCl → 2AlCl₃ + 3H₂,</em>

It is clear that 2.0 moles of Al react with 6.0 mole of HCl to produce 2.0 moles of AlCl₃ and 3.0 mole of H₂.

  • Firstly, we need to calculate the no. of moles of (6.8 g) of Al:

no. of moles of Al = mass/atomic mass = (6.8 g)/(26.98 g/mol) = 0.252 mol.

<em>Using cross multiplication:</em>

2.0 mol of Al produce → 3.0 mol of H₂, from stichiometry.

0.252 mol of Al need to react → ??? mol of H₂.

∴ the no. of moles of H₂ that can be prepared from 6.80 g of aluminum = (3.0 mol)(0.252 mol)/(2.0 mol) = 0.3781 mol.

  • Now, we can get the mass of H₂ that can be prepared from 6.80 g of aluminum:

mass of H₂ = (no. of moles)(molar mass) = (0.3781 mol)(2.0 g/mol) = 0.7561 g.

5 0
3 years ago
The boiling point of an aqueous solution is 102.08 °C. What is the freezing point? Constants can be found here.
enyata [817]

Colligative properties calculations are used for this type of problem. Calculations are as follows:<span>


ΔT(freezing point)  = (Kf)(molality)
ΔT(freezing point)  = 1.86 °C kg / mol (molality)
 </span>Tf - 102.08 = 1.86m

Tf = 1.86m + 102.08

The concetration of the solution is needed in order to obtain a specific value.

7 0
2 years ago
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