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wolverine [178]
3 years ago
11

If you could place a piece of solid silver into a container of liquid silver, would it float or sink? Explain your answer.

Chemistry
1 answer:
8_murik_8 [283]3 years ago
7 0
Liquid silver is less dense than solid silver, so the solid silver would sink
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How much energy (kJ) is required to change 0.18 mole of ice (s) at 0 C to water (l) at 0 C?
Dmitriy789 [7]

Answer:25,06 kJ of energy must be added to a 75 g block of ice.

ΔHfusion(H₂O) = 6,01 kJ/mol.

T(H₂O) = 0°C.

m(H₂O) = 75 g.

n(H₂O) = m(H₂O) ÷ M(H₂O).

n(H₂O) = 75 g ÷ 18 g/mol.

n(H₂O) = 4,17 mol.

Q = ΔHfusion(H₂O) · n(H₂O)

Q = 6,01 kJ/mol · 4,17 mol

Q = 25,06 kJ.

Explanation:

6 0
2 years ago
An object has a total mechanical energy of 150 J. At point A, the object has a kinetic energy
nika2105 [10]

Answer:

60 J

Explanation:

The law of conservation of energy states that energy is neither created nor destroyed, just converted into different forms. This means the total mechanical energy of the object at point A will be the same as the total mechanical energy at point B, and the question tells us the total of that mechanical energy is 150 J. Note we are assuming no energy is lost from the system as heat.

At point B, if the potential energy is 90 J, the remainder of the 150 J total must be kinetic energy. KE = 150 J - 90 J = 60 J.

8 0
3 years ago
The main goal of developing technology is to___?
sammy [17]

I believe the correct answer is C, but I'm 100% on this.  Hope this helped though!

-TTL

8 0
3 years ago
Read 2 more answers
How many kj of heat are needed to completely vaporize 1.30 moles of h2o? the heat of vaporization for water at the boiling point
Cerrena [4.2K]
The Kj of heat that  are needed to completely vaporize 1.30  moles of H2O  if  the heat of vaporization  for water is 40.6 Kj/mole  is calculated as  below

Q(heat) = moles x heat  of vaporization)

=1.30 mol  x40.6 kj/mol= 52.78 Kj  is needed
6 0
3 years ago
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Choose the best answer please .
STALIN [3.7K]

Answer:

B

Explanation:

3 0
2 years ago
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