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3 years ago

3. Nicotine, the addictive drug in cigarettes, contains 74.0% carbon, 8.6% hydrogen,

Chemistry

1 answer:

Vinvika [58]3 years ago

8 0

Answer:

the mass of each element can be recovered from is 162.23 grams

Explanation:

the mass really depends on the volume. If there is 74.0% carbon, 8.6% hydrogen and 17.3% nitrogen then you first cross out the 0 and 3 which leaves you with 17% and 74%. Then all you have to do is multiply 17% and 74% and then divided it by 8.6%.

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Which mass of urea, CO(NH2)2, contains the same mass of nitrogen as 101.1g of potassium nitrate?

Effectus [21]

In order to calculate the mass of nitrogen, we must first calculate the mass percentage of nitrogen in potassium nitrate. This is:
% nitrogen = mass of nitrogen / mass of potassium nitrate
% nitrogen = 14 / 101.1 x 100

The mass of nitrogen = % nitrogen x sample mass
= (14 / 101.1) x 101.1
= 14 grams

The molar weight of nitrogen is 14. Each mole of urea contains two moles of nitrogen. Therefore, for there to be 14 grams of nitrogen, there must be 0.5 moles of urea.
Mass of urea = moles urea x molecular weight urea
Mass of urea = 0.5 x 66.06
Mass of urea = 33.03 grams

4 0

3 years ago

Explain why chloro acetic acid<br>strong and than acetic acid<br>

Basile [38]

Chloroacetic acid is stronger than acetic acid because of the electron-withdrawing effect of chlorine. This effect is caused by the electronegativity.

7 0

3 years ago

What is the concentration of the murexide soution with a transmittance of 28.65%. (molar absorptivity = 3847)

Ainat [17]

Answer:

The concentration of the murexide solution is 0.0000745 M

Explanation:

From Beer-Lambert's law,

A = εlc

A = Absorbance = 28.65% = 0.2865

ε = molar absorptivity = 3847 M/cm

l = path length = 1cm

c = concentration in mol/L = ?

c = A/εl = 0.2865/(3847×1) = 0.0000745 mol/L

Hope this Helps!

6 0

2 years ago

The lowest energy state of an atom is its

erica [24]

Answer:

Principle quantum number.

Explanation:

8 0

3 years ago

Read 2 more answers

Calculate the pH of: (a) 0.1M HCl; (b) 0.1M NaOH; (c) 3 X 10% M HNO3; (d) 5 X 10-10 M HCIO.; and (e) 2 x 10-8 M KOH.

Shtirlitz [24]

Answer:

(a) $pH = -Log (0.1M) = 1$

(b) $pH = -Log (10^{-13}M) = 13$

(d) $pH = -Log (4.93x10^{-10}M) = 9.3$

(e) $pH = -Log (5^{-7}M) = 6.3$

Explanation:

To calculate de pH of an acid solution the formula is:

$pH = -Log ([H^{+}]) = 1$

were [H^{+}] is the concentration of protons of the solution. Therefore it is necessary to know the concentration of the protons for every solution in order to solve the problem.

(a) and (c) are strong acids so they dissociate completely in aqueous solution. Thus, the concentration of the acid is the same as the protons.

(b) and (e) are strong bases so they dissociate completely in aqueous solution too. Thus, the concentration of the base is the same as the oxydriles. But in this case it is necessary to consider the water autoionization to calculate the protons concentration:

$K_{w} =[H^{+} ][OH^{-}]=10^{-14}$