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Anettt [7]
3 years ago
5

1)The average lethal dose of Valium is 1.52 mg/kg of body weight. Estimate how many grams of Valium would be lethal for a 200.-l

b woman. Show all your calculations. (1lb = 453.6 g)
2) A patient in hospital is receiving the antibiotic amoxcillin IV at the rate of 50. mL/h. The IV contains 1.5 g of the antibiotic in 1000. mL. (IV stands for intravenous). Calculate the mg/min of the drip. Show all your calculations
Chemistry
1 answer:
oksano4ka [1.4K]3 years ago
7 0

Answer:

1. 0.138g of valium would be lethel in the woman

2. 125mg/min is the drip of the patient

Explanation:

1. In a body, an amount of Valium > 1.52mg / kg of body weight would be lethal.

A person that weighs 200lb requires:

200<u>lb</u> × (453.6<u>g</u> / <u>1lb</u>) × (1kg / 1000<u>g</u>) = <em>90.72kg (Weight of the woman in kg)</em>

90.72kg × (1.52mg / kg) =

137.9mg ≡

<h3>0.138g of valium would be lethel in the woman</h3>

2. The IV contains 1.5g = 1500mg/mL.

If the patient is receiving 5.0mL/h, its rate in mg/h is:

5.0<u>mL</u>/h × (1500mg/<u>mL</u>) = 7500mg/h

Now as 1h = 60min:

7500mg/<u>h</u> × (1<u>h</u> / 60min) =

<h3>125mg/min is the drip of the patient</h3>
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Write the correct ionic formula when given two elements that bond ionically.
Tanzania [10]
Answer:
            Ionic bond is formed by the opposite ions attraction between the 2 atoms in an ionically bonded compound. The two ions i.e. Cation and Anions are formed by oxidation and reduction reactions respectively. General Ionic formula is as follow,

                                             Mⁿ⁺ + Nⁿ⁻   →  MN
where;
           Mⁿ⁺   =  Cation

           Nⁿ⁻   =  Anion

           MN  =  Salt

Explanation:
                   Ionic bond is the electrostatic forces of attraction between positively charged cations and negatively charged Anions. These forces are very stronger resulting in increasing several physical properties of Ionic compounds like melting point and boiling point e.t.c.

Example:

Sodium Chloride:
                           NaCl is formed by Na⁺ cation and Cl⁻ anion as follow,

Oxidation of Na;

                                      2 Na  →  2 Na⁺  +  2 e⁻
Reduction of Cl₂;

                                    Cl₂  +  2 e⁻  →  2 Cl⁻

Crystal Lattice formation is as follow,

                                  Na⁺  +  Cl⁻   →  NaCl
4 0
3 years ago
Need help! Don’t understand
shtirl [24]
Bro honestly I don’t understand either
8 0
3 years ago
I'm hot right? here's a pic of me​
viva [34]
DANNNNNNNNNNNNGGGGGG hella hot, the hottest I seen in this world !!
4 0
2 years ago
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Calculate the vapor pressure of a solution made by dissolving 11.1 g Ca(OH)2 in 1 102 g of water at 25 °C. Vapor pressure of pur
Levart [38]

Answer:

23.15 mmHg.

Explanation:

To solve this question you need to understand that part of Raoult's law in your Chemistry textbook. So, let us delve right into the solution of the question.

We are given parameters such as the mass of Ca(OH)2 to be = 11.1 grams, mass of solvent = 102 grams, the Vapor pressure of pure water= 23.76 mm Hg, temperature = 25°C and vapour pressure of the solution= ??.

The molar mass of Ca(OH)2= 74 g/mol.

The first thing to do is to find the number of moles of Ca(OH)2 and that of water from the formula below;

Mass/ molar mass = Number of moles.

===> Number of moles, n= 11.1/ 74.

Number of moles = 0.15 moles Ca(OH)2.

===> Number of moles, n= 102/ 18.

Number of moles, n= 5.67 moles of water.

Next, we add the two moles together to find the solvent mile fraction since vapour pressure is proportional to mole fraction.

Then;

0.15 + 5.67 = 5.82.

Therefore, 5.67/ 5.82= 0.97.

Hence the vapor pressure of a solution = 0.97 × 23.76.

vapor pressure of a solution = 23.15 mmHg.

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3 years ago
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Answer:

I believe it is "Arsenenate"

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