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nlexa [21]
3 years ago
13

7. If 100.0 grams of Hydrogen burns, how many moles of Water will form?

Chemistry
1 answer:
yan [13]3 years ago
5 0

50moles of H₂O

Explanation:

Given parameters:

Mass of hydrogen burning = 100g

Unknown:

Number of moles of water formed = ?

Solution:

To solve this problem, we have to apply the mole's concept. We should first obtain the balanced equation for the reaction. Then express the mass as moles and compared to that of water.

Solve from the known to the unknown;

      Equation:

         2H₂     +     O₂    →     2H₂O

Number of moles of Hydrogen gas  = \frac{mass}{molar mass}

 Molar mass of H₂ = 2(1) = 2g/mol

  Number of moles = \frac{100}{2}  = 50moles

From the equation of the reaction;

         2 mole of H₂  produced 2 mole of H₂O;

Then 50 mole of  H₂ will produce 50moles of H₂O

50 mole of water will be formed

learn more:

Number of moles brainly.com/question/1841136

#learnwithBrainly

   

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igor_vitrenko [27]

Answer:

[NO₂] = 0.434 M

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Explanation:

The equilibrum is:  N₂O₄(g)  ⇆  2NO₂ (g)

1 moles of nitrogen (IV) oxide is in equilibrium with 2 moles of nitrogen dioxide.

Initally we only have 2.20 moles of NO₂. So let's write the equilibrium again:

              2NO₂ (g)   ⇆   N₂O₄(g)      

Initially   2.20 mol              -

React          x                      x/2

X amount has reacted, and the half has been formed, according to stoichiometry.

Eq       (2.20-x) / 3.50L     (x/2)/ 3.50L

We divide by the volume because we need molar concentrations. Let's make the Kc's expression:

Kc = [N₂O₄] / [NO₂]²

0.513 = ((x/2)/ 3.50L) /  [(2.20-x) / 3.50L]

0.513 = ((x/2)/ 3.50L) / [(2.20-x)² / 3.50L²]

0.513 = ((x/2)/ 3.50L) / [2.20-x)² / 3.50L²]

0.513 = ((x/2)/ 3.50L) / (4.84 - 4.40x + x²) / 12.25)

0.513 / 12.25 (4.84 - 4.40x + x²) = x/2 / 3.50

0.203 - 0.184x + 0.0419x² = x/2 / 3.50

3.50(0.203 - 0.184x + 0.0419x²) = x/2

7 (0.203 - 0.184x + 0.0419x²) - x = 0

1.421 - 2.288x + 0.2933x² = 0  → Quadratic formula

a = 0.2933 ;  b = -2.288 ; c = 1.421

(-b +- √(b²-4ac)) / (2a)

x₁ = 7.12

x₂ = 0.68 → We consider this value, so we can have a (+) concentration.

Concentrations in the equilibrium are:

[NO₂] = (2.20-0.68) / 3.50 = 0.434 M

[N₂O₄] = (0.68/2) / 3.50  = 0.0971 M

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Answer:

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