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11111nata11111 [884]
3 years ago
12

In the reaction 2H2+____O2----2H2O, what coefficient should be placed in front of O2 to balance the reaction? Please help

Chemistry
1 answer:
Natali5045456 [20]3 years ago
7 0

Answer:

D

Explanation:

2H2+______O2- - - - - 2H2O

I'd say no coefficient is needed cos it's already balanced

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Explain a plastic gayer
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2 years ago
Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3? Assume that there is exce
adoni [48]

Answer:

The answer is "10.84 g".

Explanation:

The formula for calculating the number for moles:

\text{Number of moles }= \frac{\ Mass}{ \ molar \ mass }

In the given acid nitric:

Owing to the nitric acid mass = 75.9 g

Nitric acid molar weight= 63\  \frac{g}{mol}

If they put values above the formula, they receive:

\text{moles in nitric acid} = \frac{75.9}{63}

                               =1.204 \ mol

In the given chemical equation:

3 NO_2 \ (g) + H_2O \ (l) \longroghtarrow 2 HNO_3 \ (aq) + NO\ (g)

In this reaction, 2 mols of nitric acid are produced by 1 mole of water.

So, 1.204 moles of nitric acid will be produced:

= \frac{1}{2} \times 1.204

=0.602\ \ \text{mol of water}.

We are now using Equation 1 in determining the quantity of water:

Water moles = 0.602\  mol

Water weight molar = 18.02 \ \frac{g}{mol}

\to 0.602 = \frac{\text{mass of mols}}{ 18.02}\\\\\to \text{mass of mols} = 0.602 \times 18.02\\\\

                         =10.84 \ g

8 0
3 years ago
At 25°C, K = 0.090 for the following reaction. H2O(g) + Cl2O(g) equilibrium reaction arrow 2 HOCl(g) Calculate the concentration
wlad13 [49]

Answer:

  • [HOCl] = 0.00909 mol/liter
  • [H₂O] = 0.03901 mol/liter
  • [Cl₂O] = 0.02351 mol/liter

Explanation:

<u />

<u>1. Chemical reaction:</u>

H_2O(g)+Cl_2O(g)\rightleftharpoons 2 HOCl(g)

<u>2. Initial concentrations:</u>

i) 1.3 g H₂O

  • Number of moles = 1.3g / (18.015g/mol) = 0.07216 mol
  • Molarity, M = 0.07216 mol / 1.5 liter = 0.0481 mol/liter

ii) 2.2 g Cl₂O

  • Number of moles = 2.2 g/ (67.45 g/mol) = 0.0326 mol
  • Molarity = 0.0326mol / 1.5 liter = 0.0217 mol/liter

<u>3. ICE (Initial, Change, Equilibrium) table</u>

            H_2O(g)+Cl_2O(g)\rightleftharpoons 2 HOCl(g)

I            0.0481      0.0326            0

C              -x                 -x              +x

E          0.0481-x    0.0326-x         x

<u />

<u>4. Equilibrium expression</u>

       K_c=\dfrac{[HOCl]^2}{[H_2O].[Cl_2O]}

     0.09=\dfrac{x^2}{(0.0481-x)(0.0326-x)}

<u />

<u>5. Solve:</u>

            x^2=0.09(x-0.0481)(x-0.0326)\\\\0.91x^2+0.007263x-0.000141125=0

Use the quadatic formula:

x=\dfrac{-0.007263\pm \sqrt{(0.007263)^2-4(0.91)(-0.000141125)}}{2(0.91)}

The positive result is x = 0.00909

Thus the concentrations are:

  • [HOCl] = 0.00909 mol/liter
  • [H₂O] = 0.0481 - 0.00909 = 0.03901 mol/liter
  • [Cl₂O] = 0.0326 - 0.00909 = 0.02351 mol/liter

3 0
3 years ago
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