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3 years ago

What is bulimia? can someone explain it to me.

2 answers:

4 0

It is an emotional disorder involving distortion of body image and an obsessive desire to lose weight, in which bouts of extreme overeating are followed by depression and self-induced vomiting, purging, or fasting.The exact cause of bulimia is currently unknown; though it is thought that multiple factors contribute to the development of this eating disorder, including genetic, environmental, psychological, and cultural influences. Some of the main causes for bulimia include:
Stressful transitions or life changes
History of abuse or trauma
Negative body image
Poor self-esteem
Professions or activities that focus on appearance/performance

Serjik [45]3 years ago

3 0

Answer:

It is a obsessive eating disorder. Where one eats over the average amount and then makes themselves vomit. This is called purging. It is one of 3 main eating disorders. It is a very complex and misunderstood disease. One typically confuses it with binge eating or anorexia.

You might be interested in

Look at the bottom of the periodic table. There are two rows of elements separated from the others. Where do these

mina [271]

Answer:

The first row of elements fits in period 6, after the element lanthanum (La). The second row of elements fits in period 7, after the element actinium (Ac). 

I hope this helps!

4 0

3 years ago

The dissociation of sulfurous acid (H2SO3) in aqueous solution occurs as follows:

aksik [14]

Answer:

The [SO₃²⁻]

Explanation:

From the first dissociation of sulfurous acid we have:

H₂SO₃(aq) ⇄ H⁺(aq) + HSO₃⁻(aq)

At equilibrium: 0.50M - x x x

The equilibrium constant (Ka₁) is:

$K_{a1} = \frac{[H^{+}] [HSO_{3}^{-}]}{[H_{2}SO_{3}]} = \frac{x\cdot x}{0.5 - x} = \frac {x^{2}}{0.5 -x}$

With Ka₁= 1.5x10⁻² and solving the quadratic equation, we get the following HSO₃⁻ and H⁺ concentrations:

$[HSO_{3}^{-}] = [H^{+}] = 7.94 \cdot 10^{-2}M$

Similarly, from the second dissociation of sulfurous acid we have:

HSO₃⁻(aq) ⇄ H⁺(aq) + SO₃²⁻(aq)

At equilibrium: 7.94x10⁻²M - x x x

The equilibrium constant (Ka₂) is:

$K_{a2} = \frac{[H^{+}] [SO_{3}^{2-}]}{[HSO_{3}^{-}]} = \frac{x^{2}}{7.94 \cdot 10^{-2} - x}$

Using Ka₂= 6.3x10⁻⁸ and solving the quadratic equation, we get the following SO₃⁻ and H⁺ concentrations:

$[SO_{3}^{2-}] = [H^{+}] = 7.07 \cdot 10^{-5}M$

Therefore, the final concentrations are:

[H₂SO₃] = 0.5M - 7.94x10⁻²M = 0.42M

[HSO₃⁻] = 7.94x10⁻²M - 7.07x10⁻⁵M = 7.93x10⁻²M

[SO₃²⁻] = 7.07x10⁻⁵M

[H⁺] = 7.94x10⁻²M + 7.07x10⁻⁵M = 7.95x10⁻²M

So, the lowest concentration at equilibrium is [SO₃²⁻] = 7.07x10⁻⁵M.

I hope it helps you!

8 0

3 years ago

In the graphic, 195 represents the _______.

Marrrta [24]

Answer:

ITS ANSWER IS

OPTION B. ATOMIC NUMBER

HI HAVE A NICE DAY

5 0

2 years ago

The rate of reaction for a chemical species is typically -rA fn (K, Ca, etc), given the reaction equation or reaction stoichiome

JulsSmile [24]

Answer:

The rate of reaction rA is an intensive parameter.

Explanation:

The rate of reaction for a chemical species is typically -rA. Negative sign only shows that reactants are consumed when time is passing in the reaction.

Reaction rate will depend of several factors such as: Constant of equilibrium - K, Concentration of species - CA, Temperature - T and so on.

When we analyze the reaction rate the units are mol/Ls. It means that reaction rate will only depend of concentration and other variables. In this way, rate of reaction only is afected when we have changes in concentrations.

Concentration is an intensive parameter, it is not important if we have 100 kg or 100 L, or even 1 Kg or 1 L of total solution. Concentrations are the proportion of them and they will remain constant independent of the total mass or volume studied.

Due to the above, concentration and rate of reaction are intensive parameters and they do not depend of the total mass or volume studied.

3 0

3 years ago

What is the answer please help

snow_lady [41]

Answer:

type the question brainly, someone already answered

Explanation:

4 0

3 years ago