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3 years ago

Which of the following is true of the mass of an object?

Chemistry

1 answer:

shtirl [24]3 years ago

6 0

Answer:

Its mass is measured on a scale.

It is measured on a balance.

Explanation:

The mass of an object can easily be determined using a balance or weighing scale.

Mass is the amount of matter contained in a substance. it is has the same value every where and will not vary by geography or location.

Weight is the force on body due to gravity. It is a function of mass and acceleration due to gravity.

Both mass and weight are different.

They can both be measured using a weight device.

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A block of iron has a mass of 150 g and a volume of 20 ml. What is the density of iron? *

shtirl [24]

Answer:

<h3>The answer is 7.50 g/mL</h3>

Explanation:

The density of a substance can be found by using the formula

$density = \frac{mass}{volume} \\$

From the question

mass of iron = 150 g

volume = 20 mL

We have

$density = \frac{150}{20} = \frac{15}{2} \\$

We have the final answer as

Hope this helps you

4 0

3 years ago

Read 2 more answers

Element X has two isotopes. If 72.0% of the element has an isotope mass of 84.9 atomic mass units, and 28.0% of the element has

bija089 [108]

<h2>Answer:</h2>

Average atomic mass of an element is the sum of the masses of its isotopes each multiplied by its natural abundance

$\footnotesize \longrightarrow \: \rm Average \: atomic \: mass = \dfrac{ \sum\limits \: \% age \: of \: each \: isotope \times Atomic \: mass }{100} \\$

$\footnotesize \longrightarrow \: \rm Average \: atomic \: mass = \dfrac{ 72 \times84.9 + 28 \times 87 }{100} \\$

$\footnotesize \longrightarrow \: \rm Average \: atomic \: mass = \dfrac{ 6112.8 + 2436 }{100} \\$

$\footnotesize \longrightarrow \: \rm Average \: atomic \: mass = \dfrac{ 8548.8 }{100} \\$

$\footnotesize \longrightarrow \: \bf Average \: atomic \: mass = 85.488 \: amu \\$

8 0

2 years ago

How far will you run in 3 minutes if you run at a pace of 4 meters per second?

atroni [7]

Answer:

you will run 720 meters

Explanation:

because 4 times 60 is 240 and 240 times 3 is 720

7 0

3 years ago

In reality, a hydrate of iron(III) nitrate had to be used, not the anhydrous salt. As you may guess, some of the hydrate’s mass

liq [111]

<u>Answer:</u> The mass of nonahydrate iron (III) nitrate is 16.2 g

<u>Explanation:</u>

To calculate the number of moles for given molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}$

Molarity of $Fe(NO_3)_3$ = 0.0020 M

Volume of solution = 2 L

Putting values in above equation, we get:

$0.0200M=\frac{\text{Moles of }Fe(NO_3)_3}{2L}\\\\\text{Moles of }Fe(NO_3)_3=(0.0200mol/L\times 2L)=0.04mol$

The chemical equation for the decomposition of hydrated iron (III) nitrate follows:

$Fe(NO_3)_3.9H_2O\rightarrow Fe(NO_3)_3+9H_2O$

By Stoichiometry of the reaction:

1 mole of iron (III) nitrate is produced from 1 mole of hydrated iron (III) nitrate

So, 0.04 moles of iron (III) nitrate will be produced from = $\frac{1}{1}\times 0.04=0.04mol$ of hydrated iron (III) nitrate

To calculate the mass from given number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Molar mass of nonahydrate iron (III) nitrate = 404.0 g/mol

Moles of nonahydrate iron (III) nitrate = 0.04 moles

Putting values in above equation, we get:

$0.04mol=\frac{\text{Mass of nonahydrate iron (III) nitrate}}{404.0g/mol}\\\\\text{Mass of nonahydrate iron (III) nitrate}=(0.04mol\times 404.0g/mol)=16.2g$

Hence, the mass of nonahydrate iron (III) nitrate is 16.2 g

7 0

3 years ago

Is Actinium Metal, Non-Metal ,or Semi-Metal?

SCORPION-xisa [38]

Metal
On the periodic table its atomic number is 89
The Semi-metals aka the metalloids are atomic umbers 5,14,32,33,51,52,and 85

The Metals are everything that is located to the left of the metalloids excluding Hydrogen(H) and Helium (He)
Everything to the right of the metalloids are non-metals including Hydrogen (H) and Helium (He)

4 0

3 years ago