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dezoksy [38]
3 years ago
6

Yvus UVILLE auuuulll

Chemistry
2 answers:
vfiekz [6]3 years ago
5 0

Answer:

The 20 kg stone traveling at 10m/s

Explanation:

Hi, the kinetic energy is the energy available of the objects in movement.

That energy can be calculated be the next formula:

ec=0.5*m*v^2

Where:

  • ec is the kinetic energy [J]
  • m is the mass of the object [kg]
  • v is the velocity of the object [m/s]

Case A:

ec=0.5*20kg*(10m/s)^2

ec=1000 J

Case B:

ec=0.5*40kg*(4m/s)^2

ec=320 J

Case C:

ec=0.5*30kg*(6m/s)^2

ec=540 J

Case D:

ec=0.5*50kg*(2m/s)^2

ec=100 J

sveta [45]3 years ago
3 0

Answer: A 20kg Stone traveling an 10 m/s

Explanation:

The Formula for Kinetic Energy is KE = 0.5 x mv², using this equation you can then find the item with the most Kinetic Energy in Joules (J) 0.5 x 20 x 10 = 200 Joules.

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Consider the reaction Mg₂Si(s) + 4 H₂O(ℓ) → 2 Mg(OH)₂(aq) + SiH₄(g). How many grams of silane gas (SiH₄) are formed if 25.0 g of
Neko [114]

Answer:

10.60 grams of silane gas are formed.

Explanation:

From the reaction:

Mg₂Si(s) + 4H₂O(l) → 2Mg(OH)₂(aq) + SiH₄(g)          

We know that the limiting reactant is Mg₂Si, so to find the mass of SiH₄ formed we need to calculate the number of moles of Mg₂Si:

\eta_{Mg_{2}Si} = \frac{m_{Mg_{2}Si}}{M_{Mg_{2}Si}}

Where:

m: is the mass of Mg₂Si = 25.0 g

M: is the molar mass of Mg₂Si = 76.69 g/mol

\eta_{Mg_{2}Si} = \frac{m_{Mg_{2}Si}}{M_{Mg_{2}Si}} = \frac{25.0 g}{76.69 g/mol} = 0.33 moles

Now, the stoichiometric relation between Mg₂Si and SiH₄ is 1:1 so:

\eta_{Mg_{2}Si} = \eta_{SiH_{4}} = 0.33 moles

Finally, the mass of SiH₄ is:

m_{SiH_{4}} = \eta_{SiH_{4}}*M_{SiH_{4}} = 0.33 moles*32.12 g/mol = 10.60 g

Therefore, 10.60 grams of silane gas are formed.

I hope it helps you!    

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3 years ago
Why do some transition metals have multiple oxidation states? Select the correct answer from each drop down menu
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Answer:

Option b. 22 g of He will have the greatest volume at STP

Explanation:

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R, T and P are the same in all the situation we must define n (number of moles).

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