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jasenka [17]
3 years ago
6

Upon which moon does mars exert a stronger gravitational force

Chemistry
2 answers:
Katena32 [7]3 years ago
4 0

Answer:

Deimos

Explanation:

riadik2000 [5.3K]3 years ago
3 0

Answer:

deimos

Explanation:

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Helpppp pleaseee ill give brainliest
Studentka2010 [4]

Answer:

The answers are in the explanation.

Explanation:

The energy required to convert 10g of ice at -10°C to water vapor at 120°C is obtained per stages as follows:

Increasing temperature of ice from -10°C - 0°C:

Q = S*ΔT*m

Q is energy, S specific heat of ice = 2.06J/g°C, ΔT is change in temperature = 0°C - -10°C = 10°C and m is mass of ice = 10g

Q = 2.06J/g°C*10°C*10g

Q = 206J

Change from solid to liquid:

The heat of fusion of water is 333.55J/g. That means 1g of ice requires 333.55J to be converted in liquid. 10g requires:

Q = 333.55J/g*10g

Q = 3335.5J

Increasing temperature of liquid water from 0°C - 100°C:

Q = S*ΔT*m

Q is energy, S specific heat of ice = 4.18J/g°C, ΔT is change in temperature = 100°C - 0°C = 100°C and m is mass of water = 10g

Q = 4.18J/g°C*100°C*10g

Q = 4180J

Change from liquid to gas:

The heat of vaporization of water is 2260J/g. That means 1g of liquid water requires 2260J to be converted in gas. 10g requires:

Q = 2260J/g*10g

Q = 22600J

Increasing temperature of gas water from 100°C - 120°C:

Q = S*ΔT*m

Q is energy, S specific heat of gaseous water = 1.87J/g°C, ΔT is change in temperature = 20°C and m is mass of water = 10g

Q = 1.87J/g°C*20°C*10g

Q = 374J

Total Energy:

206J + 3335.5 J + 4180J + 22600J + 374J =

30695.5J =

30.7kJ

5 0
2 years ago
What is the molariity of a 50.0 mL aqueous solution containing 10.0 grams of table salt, NaCl?
tia_tia [17]

Answer:

3 mol/L

Explanation:

You should know or have the equation to solve for Molarity which is;

M = n/v           (M: Molarity) (n: moles of solute) (v: Liters of solute)

You can start off differently but I would start by converting the mL to L. This is your "v" value.

50.0 mL/ 1000 mL = 0.05 L

Now, you have to convert grams to moles in order to solve for molarity (M).

1.) On the periodic table find the molecular weights of Na and Cl.

Na= 22.99 g/mol         Cl= 35.45g/mol

2.) Add them together to have their combined molecular weights.

22.99 + 35.45= 58.44 g/mol

3.) Now, you're going to use the "picket fence method" or whichever your teacher taught you to convert from grams to moles. This will be your "n" value. (I cannot show it on here without it looking weird, so my sincere apologies.)

10.0 g/ 58.44 g = 0.17111 mol

4.)You are now going to plug in your answers into the equation for Molarity.

M= 0.17111 mol / 0.05 L = 3.4222

5.) I am sure your professor might be a stickler so for sig figs sake when you multiply or divide use the smallest amount of sig figs you see which is 1. Round 3.4222 to 3 mol/L

Sorry this explanation is long let me know if you need a better more written out sample.

3 0
3 years ago
Why do some athletes use anabolic steroid and what are the side effects of using anabolic steroids
Galina-37 [17]
Some athletes use anabolic steroids in order to make their performance better, but the side effects are destroyed testicles, bad vision, bad sleeping habits, bald head.
hope this loves.
7 0
3 years ago
What does the subscript tell you?
OverLord2011 [107]
B. The number of atoms of each element in a formula
8 0
2 years ago
A certain amount of H2S was added to a 2.0 L flask and allowed to come to equilibrium. At equilibrium, 0.072 mol of H2 was found
SIZIF [17.4K]

Answer:

0.098 moles H₂S

Explanation:

The reaction that takes place is

  • 2H₂(g) + S₂(g) ⇄ 2H₂S(g)  keq = 7.5

We can express the equilibrium constant as:

  • keq = [H₂S]² / [S₂] [H₂]² = 7.5

With the volume we can <u>calculate the equilibrium concentration of H₂</u>:

  • [H₂] = 0.072 mol / 2.0 L = 0.036 M

<em>The stoichiometric ratio</em> tells us that <u>the concentration of S₂ is half of the concentration of H₂</u>:

  • [S₂] = [H₂] / 2 = 0.036 M / 2 = 0.018 M

Now we <u>can calculate [H₂S]</u>:

  • 7.5 = [H₂S]² / (0.018*0.036²)
  • [H₂S] = 0.013 M

So 0.013 M is the concentration of H₂S <em>at equilibrium</em>.

  • This would amount to (0.013 M * 2.0 L) 0.026 moles of H₂S
  • The moles of H₂ at equilibrium are equal to the moles of H₂S that reacted.

Initial moles of H₂S - Moles of H₂S that reacted into H₂ = Moles of H₂S at equilibrium

Initial moles of H₂S - 0.072 mol = 0.026 mol

Initial moles of H₂S = 0.098 moles H₂S

8 0
3 years ago
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