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3 years ago

Tracie measured 87.47 mg of cholesterol in 0.03 mL of blood. What is the density of this mixture in g/mL?

Chemistry

1 answer:

Lelu [443]3 years ago

5 0

We can use a simple equation to solve this problem.

d = m/v

Where d is the density, m is the mass and v is the volume.

d = ?

m = 87.47 mg = 87.47 x 10⁻³ g

v = 0.03 mL

By applying the equation,

d = 87.47 x 10⁻³ g / 0.03 mL

d = 2.92 g/mL

Hence, the density of the mixture is 2.92 g/mL.

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Concentrations-

Arisa [49]

Moles of HCl is 3.47mol

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6 0

3 years ago

How many grams of Ca(NO3)2 are needed to make 25.0 g of a 15.0% Ca(NO3)2(aq)?

yarga [219]

Answer:

3.75 g.

Explanation:

mass percent is the ratio of the mass of the solute to the mass of the solution multiplied by 100.

mass % = (mass of solute/mass of solution) x 100.

mass of calcium nitrite = ??? g,

mass of the solution = 25.0 g.

∴ mass % = (mass of solute/mass of solution) x 100

∴ mass of solute (calcium nitrite) = (mass %)(mass of solution)/100 = (15.0 %)(25.0 g)/100 = 3.75 g.

5 0

3 years ago

Suppose the reaction between nitrogen and hydrogen was run according to the amounts presented in Part A, and the temperature and

andrew11 [14]

Explanation:

Assuming that moles of nitrogen present are 0.227 and moles of hydrogen are 0.681. And, initially there are 0.908 moles of gas particles.

This means that, for $N_{2}(g) + 3H_{2}(g) \rightarrow 2NH_{3}$

moles of $N_{2}$ + moles of $H_{2}$ = 0.908 mol

Since, 2 moles of $N_{2}$ = $2 \times 0.227$ = 0.454 mol

As it is known that the ideal gas equation is PV = nRT

And, as the temperature and volume were kept constant, so we can write

$\frac{P(_in)}{n_(in)}$ = $\frac{P_(final)}{n_(final)}$

$\frac{10.4}{0.908}$ = $\frac{P_(final)}{0.454
}$

$P_(final)$ = $10.4 \times \frac{0.454}{0.908}$

= 5.2 atm

Therefore, we can conclude that the expected pressure after the reaction was completed is 5.2 atm.

7 0

3 years ago

A student preforms a chemical reaction in which 35 grams of hydrogen and 65 grams of oxygen reacted to form water. What is the m

tatuchka [14]

Answer:

Mass of water = 73.08 g

Explanation:

Given data:

Mass of hydrogen = 35 g

Mass of oxygen = 65 g

Mass of water = ?

Solution:

First of all we will write the balanced chemical equation:

2H₂ + O₂ → 2H₂O

Number of moles of hydrogen = mass/ molar mass

Number of moles of hydrogen = 35 g/ 2 g/mol

Number of moles of hydrogen = 17.5 mol

Number of moles of oxygen = 65 g / 32 g/mol

Number of moles of oxygen = 2.03 moles

Now we compare the moles of water with moles hydrogen and oxygen.

H₂ : H₂O

2 : 2

17.5 : 17.5

O₂ : H₂O

1 : 2

2.03 : 2× 2.03 =4.06 mol

Number of moles of water produced by oxygen are less so oxygen is limitting reactant.

Mass of water:

Mass of water = number of moles × molar mass

Mass of water = 4.06 mol × 18 g/mol

Mass of water = 73.08 g

8 0

3 years ago

Describe the properties of alkaline earth metals. Based on their electronic arrangement, explain whether they can exist alone in

zheka24 [161]

Answer: all i know about alkaline metals is he alkaline earth metals are shiny, silvery-white, and somewhat reactive metals at standard temperature and pressure.

All the alkaline earth metals readily lose their two outermost electrons to form cations with a 2+ charge.

All of the alkaline earth metals except magnesium and strontium have at least one naturally occurring radioisotope.

Magnesium and calcium are ubiquitous and essential to all known living organisms.

Explanation:

7 0

2 years ago

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