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Klio2033 [76]
1 year ago
5

Indicate the oxidation state for each of the following:

Chemistry
1 answer:
Nimfa-mama [501]1 year ago
6 0
  • P2H2 Oxidation State - Diphosphene

       P2H2 has an oxidation number of +1. In P2H2, the oxidation    

        number of H is -1

  • H2C2O4 Oxidation State - Oxalic Acid

       C has an oxidation number of +3 in H2C2O4. O has an oxidation

        number of -2 in H2C2O4. H2C2O4 has an oxidation number of +1.

  • CrO2 Oxidation State - Chromium(IV) Oxide

         CrO2 has an oxidation number of +4.

<h3>Explain oxidation?</h3>

The oxidation state, also known as the oxidation number, is an atom's hypothetical charge if all of its bonds to other atoms were fully ionic.

The sum of the oxidation states of all the atoms in an ion equals the ion's charge.

A substance's more electronegative element is given a negative oxidation state. The one that is less electronegative is given a positive oxidation state.

To learn more about oxidation refer to :

brainly.com/question/27239694

#SPJ13

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Question 6 Jackson visited the Grand Canyon with his family. He noticed that when he stood at the edge of the canyon and yelled
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3 years ago
What is the percent yield for a process in which 10.4g of CH3OH reacts and 10.1 g of CO2 is formed
monitta

Answer:

A. 70.7%

Explanation:

In the first step lets compute the molar mass of CH₃OH and CO

Molar Mass of CH₃OH =  1(12.01 g/mol) + 4(1.008 g/mol) +1(16.00 g/mol)

                                     = 32.042 g/mol

Molar Mass of CO₂      = 1(12.01 g/mol) + 2(16.00 g/mol)  

                                     = 44.01 g/mol

                                   

Mass of only one reactant i.e. CH₃OH is given so  it must be the limiting reactant. Next, the theoretical yield is calculated directly as follows:

Given mass of CH₃OH is 10.4 g. So we have:

                                     10.4g CH₃OH

Convert grams of CH₃OH to moles of CH₃OH utilizing molar mass of CH₃OH as:

                          1 mol CH₃OH / 32.042 g CH₃OH

Convert CH₃OH to moles of CO₂ using mole ratio as:

                             2 mol CO₂ / 2 mol CH₃OH

Convert moles of  CO₂ to grams of  CO₂ utilizing molar mass of  CO₂ as:

                           44.01 g/mol CO₂ / 1 mol CO₂

Now calculating theoretical yield using above steps:

[ 10.4 g CH₃OH ]  [1 mol CH₃OH / 32.042 g CH₃OH ]  [2 mol CO₂ / 2 mol CH₃OH]  [44.01 g/mol CO₂ / 1 mol CO₂]

Multiplication is performed here. We are left with 10.4 and 44.01 g CO₂ from numerator terms in the above equation and 32.042 from denominator terms after cancellation process of above terms. So this equation becomes:

= ( 10.4 ) ( 44.01 ) g CO₂ / 32.042

= 457.704/32/042

=  14.28 g CO₂

Theoretical yield =  14.28 g CO₂  

Finally compute the percent yield for a process in which 10.4g of CH₃OH reacts and 10.1 g of CO₂ is formed:

percent yield = (actual yield / theoretical yield) x 100

As we have calculated theoretical yield which is 14.28 g CO₂ and actual yield is 10.1 g CO₂ So,

percent yield = (10.1 g CO₂ / 14.28 g CO₂) x 100%

                       = 0.707 x 100%

                       = 70.7 %

Hence option A 70.7% yield is the correct answer.

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