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julsineya [31]
3 years ago
10

6. Macromolecules represent which level of organization in the body?

Chemistry
1 answer:
hodyreva [135]3 years ago
6 0

Answer:

Chemical

Explanation:

Macromolecules are part of the chemical components of cells. For example, DNA, proteins, and lipids.

Cells of similar types/function form tissues. Different types of tissues interact together to form organs. Organs form a common function.

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A sample of gold (Au) has a mass of 45.39 g.
professor190 [17]
<span>1. What is the molar mass of gold?
Molar mass is a unit that expresses the mass of a molecule per one mol. The molar mass can be obtained by adding the neutron with the proton of the atoms. Gold has atomic number 79 so the proton is 79. The number of the neutron is 118. Then the molar mass would be: 79 + 118 = </span>197 g/mol<span>


</span><span>2. Calculate the number of moles of gold (Au) in the sample. Show your work. 
</span>In this question, you are given the mass of the gold and asked for how many moles the sample has. To find the number of moles you just need to divide the weight by the molar mass.
For 45.39 grams of gold, the number of moles would be:
45.39 / (197g/mol)= 0.23 moles


3. Calculate the number of atoms of gold (Au) in the sample. Show your work.Moles is unit of a number of molecules but 1 mol doesn't represent 1 molecule. The number of atoms can be obtained by multiplying the number of moles with Avogadro number. The calculation would be:
0.23 moles * (6.023 * 10^23 molecules/mol)= 1.387 * 10^23 molecules
8 0
3 years ago
A(g) + 2B(g) → C(g) + D(g)
WITCHER [35]

Answer:

0.169

Explanation:

Let's consider the following reaction.

A(g) + 2B(g) ⇄ C(g) + D(g)

We can find the pressures at equilibrium using an ICE chart.

       A(g) + 2 B(g) ⇄ C(g) + D(g)

I       1.00     1.00        0        0

C       -x        -2x        +x       +x

E    1.00-x  1.00-2x     x         x

The pressure at equilibrium of C is 0.211 atm, so x = 0.211.

The pressures at equilibrium are:

pA = 1.00-x = 1.00-0.211 = 0.789 atm

pB = 1.00-2x = 1.00-2(0.211) = 0.578 atm

pC = x = 0.211 atm

pD = x = 0.211 atm

The pressure equilibrium constant (Kp) is:

Kp = pC × pD / pA × pB²

Kp = 0.211 × 0.211 / 0.789 × 0.578²

Kp = 0.169

6 0
3 years ago
When the metal was placed in the calorimeter its
guajiro [1.7K]

Answer:

Exam 3 Material

Homework Page Without Visible Answers

This page has all of the required homework for the material covered in the third exam of the first semester of General Chemistry. The textbook associated with this homework is CHEMISTRY The Central Science by Brown, LeMay, et.al. The last edition I required students to buy was the 12th edition (CHEMISTRY The Central Science, 12th ed. by Brown, LeMay, Bursten, Murphy and Woodward), but any edition of this text will do for this course.

Note: You are expected to go to the end of chapter problems in your textbook, find similar questions, and work out those problems as well. This is just the required list of problems for quiz purposes. You should also study the Exercises within the chapters. The exercises are worked out examples of the questions at the back of the chapter. The study guide also has worked out examples.

These are bare-bones questions. The textbook questions will have additional information that may be useful and that connects the problems to real life applications, many of them in biology.

Explanation:

5 0
2 years ago
Read 2 more answers
Calculate the volume in mL of a 0.708 M KOH solution containing 0.098 mol of solute
Olenka [21]
Molarity = mol/liter

0.708M = 0.098mol/L
Rearrange to find L:
0.098mol/0.708M = .138L

For every liter there is 1000 mL:
.138L • 1000mL =138mL KOH
7 0
3 years ago
How many grams in 11.9 moles of sulfur? Avogadro’s number: 6.02x1023 atoms = 1 mole Molar mass of sulfur: 32.06 g sulfur = 1 mol
sergiy2304 [10]

Answer:

Mass = 0.37 g

Explanation:

Given data:

Number of moles of sulfur = 11.9 mol

Mass of sulfur in 11.9 mol = ?

Molar mass of sulfur = 32.06 g

Solution:

Number of moles = mass/molar mass

by putting values,

11.9 mol = mass/ 32.06 g/mol

Mass = 11.9 mol × 32.06 g/mol

Mass = 0.37 g

4 0
2 years ago
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