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3 years ago

14

A doctor is testing a new medication and he doesn’t tell the people in the study about the possible side effects of the medicine

. He is _____.
showing bias
being non-compliant
being fair
using the scientific method

2 answers:

Anika [276]3 years ago

8 0

Answer is non compliant

Svetach [21]3 years ago

3 0

Answer: Being fair

Explanation:

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11 Which substance can not be broken down by a chemical change?

Rus_ich [418]

(2) Arsenic. It is an element and elements are chemically the simplest units and cannot be broken down by any chemical change.

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Given the Henry’s law constant for O2(4.34*109Pa) at 25° C, calculate the molar concentration of oxygen in air-saturated and O2s

Flauer [41]

This is an incomplete question, here is a complete question.

The Henry's law constant for oxygen dissolved in water is 4.34 × 10⁹ g/L.Pa at 25⁰C.If the partial pressure of oxygen in air is 0.2 atm, under atmospheric conditions, calculate the molar concentration of oxygen in air-saturated and oxygen saturated water.

Answer : The molar concentration of oxygen is, $2.67\times 10^2mol/L$

Explanation :

As we know that,

$C_{O_2}=k_H\times p_{O_2}$

where,

$C_{O_2}$ = molar solubility of $O_2$ = ?

$p_{O_2}$ = partial pressure of $O_2$ = 0.2 atm = 1.97×10⁻⁶ Pa

$k_H$ = Henry's law constant = 4.34 × 10⁹ g/L.Pa

Now put all the given values in the above formula, we get:

$C_{O_2}=(4.34\times 10^9g/L.Pa)\times (1.97\times 10^{-6}Pa)$

$C_{O_2}=8.55\times 10^3g/L$

Now we have to molar concentration of oxygen.

Molar concentration of oxygen = $\frac{8.55\times 10^3g/L}{32g/mol}=2.67\times 10^2mol/L$

Therefore, the molar concentration of oxygen is, $2.67\times 10^2mol/L$

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3 years ago

Which of the following is not a physical property of a liquid? indefinite volume indefinite shape definite mass

Elanso [62]

Definitely definite mass because liquids can take on any shape and can have different volumes.

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3 years ago

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What is the value for (delta)G at 1000 K if (delta)H = -220 kJ/mol and (delta)S = -0.05 kJ/(molK)?

tankabanditka [31]

The system is isothermal, so we use the formula:
(delta)G = (delta)H - T (delta) S

Plugging in the given values:
(delta)G = -220 kJ/ mol - (1000K) (-0.05 kJ/mol K)
(delta)G = -170 kJ/mol

If we take a basis of 1 mol, the answer is
D. -170 kJ

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3 years ago

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A student dissolves 6.2g of aniline c6h5nh2 in 350.ml of a solvent with a density of 1.04/gml . the student notices that the vol

Troyanec [42]

Answer : The correct answer for molarity = 0.19 $\frac{mol}{L}$ and Molality = 0.18 $\frac{mol}{Kg}$ .

Given : Mass of aniline = 6.2 g

Volume of solvent = 350 mL Density of solvent = 1.04 g/mL

1) Molarity : It is defined as number of moles of solute present in Litre of solution . It is expressed as :

$Molarity(M) = \frac{moles of solute(mole)}{volume of solution (L)}$ \

Molairty can be found in following steps :

Step 1 : To calculate mole :

Mole of solute can be calculate using mole formula :

$Mole of solute = \frac{given mass of solute (g)}{molar mass of solute\frac{g}{1 mol}}$

Molar mass of aniline (C₆H₅NH₂) = 93.13 $\frac{g}{1 mol}$

Mass of aniline = 6.2 g

Plugging values in mole formula :

$Mole = \frac{6.2 g}{93.13 \frac{g}{1 mol}}$

Mole = 0.0665 mol

Step 2 : To find volume of solution

Volume of solution = volume of solute + volume of solution

Since addition of aniline does not change final volume , so volume of solvent = volume of solution. Since volume is given in mL , so it need to be converted to L .

1 L = 1000mL

$Volume of solution = \frac{350 mL}{1000mL} * 1 L$

Volume of solution = 0.350 L

Step 3: Plug value of mole and volume in molarity formula :

$Molarity = \frac{0.0665 mol}{0.350 L }$

Molarity = 0.19 M or 0.19 $\frac{mol}{L}$

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2) Molality : It is defined as mole of solute present in Kilogram of solvent . It can be expressed as :

$Molality (m) = \frac{mole of solute (mol)}{Kilogram of solvent (Kg)}$

Following are the steps to calculate molality :

Step 1: To find mole of Solute :

Mole of solute can be found out using mole formula . It is same as done for molarity .

Mole = 0.0665 mol

Step 2 : To find kilogram of solvent :

Mass of solvent can be calculated using density formula as :

$Density \frac{g}{mL} = \frac{mass (g) }{volume (mL)}$

Plugging value in density formula :

$1.04 \frac{g}{mL} = \frac{ mass }{350 mL}$

Multiplying both side by 350 mL

$1.04 \frac{g}{mL} * 350 mL = \frac{x}{350 mL } * 350 mL$

Mass of solvent = 364 g

Since mass is in g, it need to be converted to Kg . ( 1 Kg = 1000 g )

$Mass of solvent = \frac{364 g}{1000g} * 1 Kg$

Mass of solvent = 0.364 Kg

Step 3: Plug values of mole and Kg in molality formula :

$Molality = \frac{0.0665 mol}{0.364 Kg}$

Molality = 0.18 m or 0.18 $\frac{mol}{Kg}$

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3 years ago