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Dmitrij [34]
2 years ago
9

The chemical equation below shows the burning of magnesium (Mg) with oxygen (O2) to form magnesium oxide (MgO). 2Mg + O2 Right a

rrow. 2MgO The molar mass of O2 is 32.0 g/mol. What mass, in grams, of O2 is required to react completely with 4.00 mol of Mg? 2.00 64.0 128 256
Chemistry
1 answer:
Nadusha1986 [10]2 years ago
4 0

Answer:

64.0

Explanation:

2Mg+O2 ---> 2MgO

use dimentional analysis to find the amount of moles of O2 needed first

4.00molMg x 1.00mol O2/ 2.00 mol Mg=. 2.00 mol O2

using the coefficients you can see the mole ratio for O2:Mg the mole ratio is 1:2 which is why there is 1 mole on the top for 2 moles on the bottom. The Mg would cancel and multiply 4 by 1 then divide by 2, or multipy 4 by 1/2

Now that you have the moles of O2 you use the molar mass to find the grams in 2 moles of O2

2.00 mol O2 x 32.0g/1.00 mol = 64.0 g

multiply 2 by 32

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Tissues form organs, and organs form systems. Hope this helped!

Explanation:

7 0
2 years ago
A 1.00 L sample of a gas has a mass of 1.92 g at STP. What is the molar mass (molecular weight) of the gas
miss Akunina [59]

Answer:

The answer is below

Explanation:

Avogadro stated that "Equal volumes of all gases at the same temperature and pressure contain the same number of molecules". Hence at standard temperature and pressure 1 mole of a gas occupies 22.4 liters of volume.

1 mol = 22.4 liters

Given a gas with 1 L and mass of 1.92 g at STP.

number of moles = 1 L / (22.4 L / mol) = 0.0446 mol

The molar mass = mass of gas / number of moles

molar mass = 1.92 g / 0.0446 mol

molar mass = 43.008 g / mol

5 0
2 years ago
A chef makes a marinade by mixing red pepper flakes, dried onion flakes, and a ground ginger with soy sauce. He sets the marinad
Alisiya [41]

Answer:

Suspension

Explanation:

This mixture is a simple suspension.

A suspension is a mixture of small insoluble particles of a solid in a liquid or gas. Here, it is insoluble particles in liquid.

  • Suspensions are settle on standing this is why they have to be mixed again.
  • The particles do not pass through ordinary filter paper.
  • They are usually cloudy and have an opaque color.
  • The marinade is simply a suspension.
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3 0
2 years ago
Read 2 more answers
How many milliliters of C5H8 can be made from 366 mL C5H12 ?
zlopas [31]

The number of Ml  of C₅H₈  that can  be  made  from 366  ml  C₅H₁₂  is 314.7 ml  of C₅H₈


  <u><em>calculation</em></u>

 step  1: write  the  equation for  formation of C₅H₈

C₅H₁₂  →  C₅H₈  + 2 H₂

Step 2: find the mass of C₅H₁₂

mass = density × volume

= 0.620 g/ml × 366 ml =226.92 g

Step 3: find moles  Of  C₅H₁₂

moles  = mass÷  molar mass

from periodic table the  molar mass of  C₅H₁₂ = (12 x5) +(  1 x12) = 72 g/mol

moles = 226.92 g÷ 72 g/mol =3.152 moles

Step 4: use the  mole ratio  to determine the  moles of C₅H₈

C₅H₁₂:C₅H₈  is 1:1  from equation above

Therefore the  moles of C₅H₈  is also = 3.152  moles

Step 5: find the mass  of C₅H₈

mass = moles x molar mass

from periodic table the  molar mass of C₅H₈ = (12 x5) +( 1 x8) = 68 g/mol

= 3.152  moles x 68 g/mol = 214.34 g

Step 6: find Ml of  C₅H₈

=mass / density

= 214.34 g/0.681 g/ml = 314.7 ml



8 0
2 years ago
How much energy is required to melt a 20.0lb bag of ice a 0°c? A pound (lb.) is equivalent to 0.4536. The Hfusion of ice is +6.0
erma4kov [3.2K]
To compute the energy, Q, needed to melt a certain amount of ice, n, in moles, we have

Q = n \Delta H_{f}

where the latent heat of fusion for ice is equal to 6.009 kJ/mol.

Now, since we have a 20.0 lb ice, we must first convert its mass to grams. Thus mass = (20.0)(1000)(0.4536) = 9072 g.

To find the number of moles present, we must recall that the molar mass of water (ice) is equal to <span>1.00794(2) + </span><span>15.9994 </span>≈ 18.01 g/mol. Hence, we have

ice_{moles} = (\frac{9072 g}{1})(\frac{1 mol}{18.01 g}) =503.72 moles

Now, to compute for the molar heat of fusion, Q,

Q = (503.72)(6.009) = 3026.9 kJ

Therefore, the amount of heat needed to melt the 20-lb bag of ice is equal to 3026.9 kJ.
 
Answer: 3026.9 kJ
6 0
2 years ago
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