1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
kvasek [131]
3 years ago
7

How many grams are in 7 moles of water H2O molecules

Chemistry
1 answer:
fgiga [73]3 years ago
6 0

Answer:

7 moles of water (H20) molecules is 126.10696 grams.

Explanation:

You might be interested in
Generally, observed behavior that can be formulated into a statement, sometimes mathematical in nature, is called a(n):
earnstyle [38]

Answer:

Generally, observed behavior that can be formulated into a statement, sometimes mathematical in nature, is called a natural law- D.

7 0
2 years ago
Read 2 more answers
What is the molariity of a 50.0 mL aqueous solution containing 10.0 grams of hydrogen peroxide, H2O2?
daser333 [38]

Answer:

6 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 = <em>0.05 L</em>

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 H and O.

H= 1.01 g/mol         O= 16.00 g/mol

2.) Multiply them and then add them together to have their combined molecular weights. (You have to multiply by 2 because of their equation; H2O2).

2(1.01) + 2(16.00)= 34.02 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/ 34.02 g = <em>0.2939 mol</em>

<em />

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

M= 0.2939 mol / 0.05 L = <em>5.878 mol/L</em>

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 5.878 to 6 mol/L

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

4 0
3 years ago
Please help
Mashutka [201]

Answer:

Potential

Explanation:

The answer is potential!

6 0
1 year ago
Read 2 more answers
What is the relationship between wavelength and frequency
Vladimir [108]

they are both types of measurements

3 0
3 years ago
Read 2 more answers
What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH4Cl produced by the reaction
Mashcka [7]

Answer:

a) HCl is the limiting reagent.

b) Mass of NH₄Cl formed = 6.68 g

c) Pressure of the gas remaining in the flask = 1.742 atm

Explanation:

The complete Question is presented in the attached image to this solution.

To solve this question, we first need to obtain the limiting regaent for this reaction.

The limiting reagent is the reagent that is in short supply in the reaction and is used up in the reaction. It determines the amount of products that will be formed and the amount of other reactants that will be required for the reaction.

NH₃ (g) + HCl (g) ⟶ NH₄Cl (s)

1 mole of NH₃ reacts with 1 mole of HCl

we first convert the masses of the gases available to number of moles.

Number of moles = (Mass/Molar Mass)

Molar mass of NH₃ = 17.031 g/mol, Molar mass of HCl = 36.46 g/mol

Number of moles of NH₃ = (4.55/17.031) = 0.2672 mole

Number of moles of HCl = (4.55/36.46) = 0.1248 mole

Since 1 mole of NH₃ reacts with 1 mole of HCl

It is evident that HCl is in short supply and is the limiting reagent.

NH₃ is in excess.

So, to calculate the amount of NH₄Cl formed,

1 mole of HCl gives 1 mole of NH₄Cl

0.1248 mole of HCl will also gove 0.1248 mole of NH₄Cl

Mass (Number of moles) × (Molar Mass)

Molar mass of NH₄Cl = 53.491 g/mol

Mass of NH₄Cl formed = 0.1248 × 53.491 = 6.68 g

c) The gas remaining in the flask is NH₃

0.1248 mole of NH₃ is used up for the reaction, but 0.2672 mole was initially available for reaction,

The amount of NH₃ left in the reacting flask is then

0.2672 - 0.1248 = 0.1424 mole.

Using the ideal gas Equation, PV = nRT

We can obtain the rrequired pressure of the remaining gas in the flask

P = Pressure = ?

V = Volume = 2.00 L

n = number of moles = 0.1424 mole

R = molar gas constant = 0.08205 L.atm/mol.K

T = absolute temperature in Kelvin = 25 + 273.15 = 298.15 K

P = (nRT/V)

P = (0.1424×0.08205×298.15/2) = 1.742 atm

Hope this Helps!!!

7 0
3 years ago
Other questions:
  • A box contains identical balls of which 12 are red, 18 white and 8 blue. Three balls are drawn from the box one after the other
    11·1 answer
  • Which of the following are examples of physical change? Copper oxidizing Iron rusting Carbon dioxide sublimating Water evaporati
    8·1 answer
  • How would you find how many unpaired electrons are in a compound? Ex. unpaired electrons in aluminum in aluminum II oxide.
    12·1 answer
  • Despite the superior intellect of our lab workers, none of the problems above actually caused the discrepancies. This occurs som
    8·1 answer
  • How are sound waves can be used for various applications
    5·1 answer
  • water from a town is suspected to contain chloride ions but not sulphate ions . describe how the presence of the chloride ions i
    9·1 answer
  • A gold block with a mass of 325 g was heated from 22°C to 87°C. How much heat
    15·1 answer
  • When 0.25 moles of NH3 are produced according to the reaction below, how many moles of H2 must have reacted?
    6·2 answers
  • I need helpppppppp, please
    11·1 answer
  • Nonmetals are defined as elements that generally cannot conduct:.
    14·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!