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2 years ago

Write the balanced equation for the ionization of the weak base pyridine, c5h5n , in water, h2o. Phases are optional.

Chemistry

1 answer:

Lelu [443]2 years ago

6 0

The balanced equation for the ionization of the weak base pyridine,C5H5N in water, H2O

C_5H_5N ( aq.) + H2O ( l) ---------> C5H5NH+ (aq.) + OH- (aq.)

<h3>What is the balanced equation for the ionization?</h3>

Generally, Pyridine is characterized by a ring structure, in this characteristic ring structure N is sp2 hybridized, hence creating a lone pair present on N so s - character is more, as well as lone pair, is present.

Therefore, Considering The following functions of the equation:weak base pyridine,C5H5N in water, H2O

We write the balanced equation for the ionization as

C_5H_5N ( aq.) + H2O ( l) ---------> C5H5NH+ (aq.) + OH- (aq.)

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What volume of benzene (C6H6, d= 0.88 g/mL, molar mass = 78.11 g/mol) is required to produce 1.5 x 103 kJ of heat according to t

Anton [14]

Answer:

We need 42.4 mL of benzene to produce 1.5 *10³ kJ of heat

Explanation:

Step 1: Data given

Density of benzene = 0.88 g/mL

Molar mass of benzene = 78.11 g/mol

Heat produced = 1.5 * 10³ kJ

Step 2: The balanced equation

2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) ΔH°rxn = -6278 kJ

Step 3: Calculate moles of benzen

1.5 * 10³ kJ * (2 mol C6H6 / 6278 kJ) = 0.478 mol C6H6

Step 4: Calculate mass of benzene

Mass benzene : moles benzene * molar mass benzene

Mass benzene= 0.478 * 78.11 g

Mass of benzene = 37.34 grams

Step 5: Calculate volume of benzene

Volume benzene = mass / density

Volume benzene = 37.34 grams / 0.88g/mL

Volume benzene = 42.4 mL

We need 42.4 mL of benzene to produce 1.5 *10³ kJ of heat

4 0

2 years ago

The empirical formula of a hydrocarbon (compound that contains only C and H is found to be CH. laboratory procedures have found

gulaghasi [49]

Answer:

C₆H₆

Explanation:

Molar mass of the compound is 78g/mol

Unknown:

Molecular formula of the compound = ?

Solution:

The empirical formula of the compound is CH.

Empirical formula is the simplest formula of a compound.

To solve this problem:

Find the molar mass of CH;

Molar mass = 12 + 1 = 13g/mol

Multiplication index = $\frac{78}{13}$ = 6

So;

(CH)₆ ;

Therefore:

C₆H₆

6 0

2 years ago

The half life of carbon is 5,730 years. What fraction of the original 14/6 C would be in a wooden axe handle that was 17,190 yea

Mariana [72]

Answer:

$\frac{1}{8}$

Explanation:

The half-life of carbon (5730 y) is the time it takes for half the carbon to decay.

After one half-life, half (50 %) of the original amount will remain.

After a second half-life, half of that amount (25 %) will remain, and so on.

$\text{17 190 y} \times \frac {\text {1 half-life}}{\text{5730 y}} = \text{3 half-lives}$

We can construct a table.

No of half-lives Fraction remaining

1 $\frac{1}{2}$

2 $\frac{1}{4}$

3 $\frac{1}{8}$

The general formula is

$\text{Fraction remaining} = \frac{1}{2^{n}}$

where n = the number of half-lives.

Thus, $\frac{1}{8}$ of the original carbon remains after 17 190 y.

8 0

3 years ago

Can u make slime with takyglue,shavingcreame,Landry deterget mixed with baby oil,water

ss7ja [257]

The answer is yes, it works very well but it will b a very foamy sline bc of shaving cream

6 0

3 years ago

Read 2 more answers

WILL RATE BRAINLIST

svlad2 [7]

Answer:

The limiting reactant is the covers.

We are left with 3750 sheets of lined paper, 1125 sheets of graph paper and 25 staples.

Explanation:

the reaction is:

B - book

C - cover

Sl = sheet of lined paper

Sg - sheet of graph paper

St - staple

1B = 2C + 50Sl + 25Sg + 3St

We have covers for 150/2 = 75 books

We have lined paper for 7500/50 = 150 books

We have graph paper for 3000/25 = 120books

We have Staples for 250/3 = 83.(3) books, so for 83 books as we cannot make 1/3 of a book.

Because we only have covers for 75 books, covers are the limiting reactant.

After making 75 books we are left with:

0 covers

7500 - 75*50 = 3750 sheets of lined paper

3000 - 75*25 = 1125 sheets of graph paper

250 - 75*3 = 25 staples

6 0

3 years ago