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viva [34]
2 years ago
13

A Textbook of

Chemistry
1 answer:
Vlad [161]2 years ago
3 0

Explanation:

Information Technology CBSE Code 402 for class IX and X is based on National Skills Qualifications Framework. The book is designed and structured to help learner acquire the knowledge and skills regarding conputers, office productivity tools and internet necessary in real life competitive worlf

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Wine goes bad soon after opening because the ethanol (CH3CH2OH) dissolved in it reacts with oxygen (O2) gas to form water and aq
andrezito [222]

The number of mole of oxygen needed is of 0.080 mole.

To solve this question, we'll begin by writing the balanced equation for the reaction. This is illustrated below:

<h3>CH₃COOH + 2O₂ —> CO₂ + 2H₂O</h3>

From the balanced equation above,

2 moles of O₂ reacted to produce 2 moles of H₂O.

Finally, we shall determine the number of mole of O₂ needed to produce 0.080 mole of H₂O. This can be obtained as follow:

From the balanced equation above,

2 moles of O₂ reacted to produce 2 moles of H₂O.

Therefore,

0.080 mole of O₂ will also react to produce 0.080 mole of H₂O.

Thus, 0.080 mole of oxygen, O₂, is needed for the reaction.

Learn more: brainly.com/question/1563415

7 0
3 years ago
What is the total anion concentration (in mEq/L ) of a solution that contains 6.0 mEq/L Na + , 11.0 mEq/L Ca 2+ , and 1.0 mEq/L
lubasha [3.4K]

24



Ddddd

Hope I helped

5 0
3 years ago
A 99.8 mL sample of a solution that is 12.0% KI by mass (d: 1.093 g/mL) is added to 96.7 mL of another solution that is 14.0% Pb
andre [41]

Answer:

m_{PbI_2}=18.2gPbI_2

Explanation:

Hello,

In this case, we write the reaction again:

Pb(NO_3)_2(aq) + 2 KI(aq)\rightarrow PbI_2(s) + 2 KNO_3(aq)

In such a way, the first thing we do is to compute the reacting moles of lead (II) nitrate and potassium iodide, by using the concentration, volumes, densities and molar masses, 331.2 g/mol and 166.0 g/mol respectively:

n_{Pb(NO_3)_2}=\frac{0.14gPb(NO_3)_2}{1g\ sln}*\frac{1molPb(NO_3)_2}{331.2gPb(NO_3)_2}  *\frac{1.134g\ sln}{1mL\ sln} *96.7mL\ sln\\\\n_{Pb(NO_3)_2}=0.04635molPb(NO_3)_2\\\\n_{KI}=\frac{0.12gKI}{1g\ sln}*\frac{1molKI}{166.0gKI}  *\frac{1.093g\ sln}{1mL\ sln} *99.8mL\ sln\\\\n_{KI}=0.07885molKI

Next, as lead (II) nitrate and potassium iodide are in a 1:2 molar ratio, 0.04635 mol of lead (II) nitrate will completely react with the following moles of potassium nitrate:

0.04635molPb(NO_3)_2*\frac{2molKI}{1molPb(NO_3)_2} =0.0927molKI

But we only have 0.07885 moles, for that reason KI is the limiting reactant, so we compute the yielded grams of lead (II) iodide, whose molar mass is 461.01 g/mol, by using their 2:1 molar ratio:

m_{PbI_2}=0.07885molKI*\frac{1molPbI_2}{2molKI} *\frac{461.01gPbI_2}{1molPbI_2} \\\\m_{PbI_2}=18.2gPbI_2

Best regards.

5 0
3 years ago
Read 2 more answers
What happens when an acid reacts with a base?
shepuryov [24]

Answer:

They neutralize each other

3 0
3 years ago
Read 2 more answers
A certain amount of hydrogen peroxide was dissolved in 100. mL of water and then titrated with 1.68 M KMnO4. What mass of H2O2 w
Stels [109]

Answer:

see explanation below

Explanation:

First to all, this is a redox reaction, and the reaction taking place is the following:

2KMnO4 + 3H2SO4 + 5H2O2 -----> 2MnSO4 + K2SO4 + 8H2O + 5O2

According to this reaction, we can see that the mole ratio between the peroxide and the permangante is 5:2. Therefore, if the titration required 21.3 mL to reach the equivalence point, then, the moles would be:

MhVh = MpVp

h would be the hydrogen peroxide, and p the permanganate.

But like it was stated before, the mole ratio is 5:2 so:

5MhVh = 2MpVp

Replacing moles:

5nh = 2MpVp

Now, we just have to replace the given data:

nh = 2MpVp/5

nh = 2 * 1.68 * 0.0213 / 5

nh = 0.0143 moles

Now to get the mass, we just need the molecular mass of the peroxide:

MM = 2*1 + 2*16 = 34 g/mol

Finally the mass:

m = 0.0143 * 34

m = 0.4862 g

8 0
3 years ago
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