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Irina-Kira [14]
3 years ago
8

Calculate the mass of Na2O that can be produced by the chemical reaction of 4.0 grams of sodium with excess oxygen in the reacti

on.
4NA + O2 ⟶ 2Na2O
Chemistry
1 answer:
e-lub [12.9K]3 years ago
8 0

Answer:

The mass of Na₂O that can be produced by the chemical reaction of 4.0 grams of sodium with excess oxygen in the reaction is 5.39 grams.

Explanation:

You know  the balanced reaction:

4 NA + O₂ ⟶ 2 Na₂O

By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction) react and are produced:

  • Na: 4 moles
  • O₂: 1 mole
  • Na₂O: 2 moles

Being:

  • Na: 23 g/ole
  • O: 16 g/mole

the molar mass of the compounds participating in the reaction is:

  • Na: 23 g/mole
  • O₂: 2*16 g/mole= 32 g/mole
  • Na₂O: 2*23 g/mole +16 g/mole=  62 g/mole

Then by stoichiometry of the reaction they react and are produced:

  • Na: 4 moles* 23 g/mole= 92 g
  • O₂: 1 mole*32  g/mole= 32 g
  • Na₂O: 2 moles* 62 g/mole= 124 g

Then you can apply the following rule of three: if 92 grams of Na produce 124 grams of Na₂O, 4 grams of Na, how much mass of Na₂O does it produce?

massofNa_{2}O =\frac{4 grams of Na*124 gramsofNa_{2}O }{92 grams of Na}

mass of Na₂O=5.39 g

<em><u>The mass of Na₂O that can be produced by the chemical reaction of 4.0 grams of sodium with excess oxygen in the reaction is 5.39 grams.</u></em>

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Answer:

133.33 g/mole

Explanation:

To get the molar mass, you will need to first determine the atoms in the compound.

AlCl₃

We have aluminum (Al) and Chlorine (Cl)

Next step is to determine how many atoms of each element you have in the compound. The subscript will tell you how many. If you see no subscript, that means 1 atom.

Al = 1 atom

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Then you multiply the number of atoms by the atomic weight to get the molar mass of each element and add them up to get the total molar mass of the compound:

Element          # of atoms        atomic weight           molar mass

Al                         1               x     26.98 g/mole =    26.98 g/mole

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                                                             TOTAL =   133.33 g/mole

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3 years ago
A piece of metal weighing 57.3 g is heated to a temperature of 88.0°C and is then immersed in 155 g of water at a temperature of
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The method used by Joseph Priestley to obtain oxygen made use of the thermal decomposition of mercuric oxide given below. What v
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Answer:

The volume of the oxygen gas is 0.246 L

Explanation:

Step 1: Data given

Temperature = 39 °C = 312 K

Temperature = 725 torr = 725 / 760 atm =  0.953947 atm

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Molar mass of mercuric oxide = 216.59 g/mol

Step 2: The balanced equation

2HgO → 2Hg + O2

Step 3: Calculate moles mercuric oxide

Moles = mass / molar mass

Moles HgO = 3.97 grams / 216.59 g/mol

Moles HgO = 0.0183 moles

Step 3: Calculate moles oxyen

For 2 moles HgO we'll have 2 moles Hg and 1 mol O2

For 0.0183 moles HgO we'll have 0.0183/2 = 0.00915 moles O2

Step 4: Calculate volume O2

p*V = n*R*T

⇒with p = the pressure of the gas = 0.953947 atm

⇒with V = the volume of O2 gas = TO BE DETERMINED

⇒with n = the moles of O2 = 0.00915 moles

⇒with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 312 K

V = (n*R*T)/p

V = (0.00915 moles * 0.08206 L*atm/mol*K * 312 K ) / 0.953947 atm

V = 0.246 L

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3 0
3 years ago
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Answer:

B 2

Explanation:

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