1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
Leviafan [203]
2 years ago
15

Mr. Auric Goldfinger, criminal mastermind, intends to smuggle several tons of gold across international borders by disguising it

as lumps of iron ore. He commands his engineer minions to form the gold into little spheres with a diameter of exactly
8 cm and paint them black.

However, his chief engineer points out that customs officials will surely notice the unusual weight of the "iron ore" if the balls are made of solid gold (density
). She suggests forming the gold into hollow balls instead , so that the fake "iron ore" has the same density as real iron ore
One of the balls of fake "iron ore," sliced in half.

Calculate the required thickness of the walls of each hollow lump of "iron ore." Be sure your answer has a unit symbol, if necessary, and round it to 2
significant digits.
Chemistry
1 answer:
Aleks [24]2 years ago
4 0

The thickness of the walls of each hollow lump of iron ore is: 0.295cm. This is determined using the knowledge of the Volume of a Hollow Sphere.

<h3>What is the Volume of a Hollow Sphere?</h3>

The formula for the Volume of a Hollow Sphere is give as:

Volume of a Hollow = 4/3 R³ – 4/3 r³

Step 1 - Find the apparent volume of 8cm diameter sphere including the wall the the hollow inside

V = 4/3 r³

V = (4/3) (8)³

V = (4/3) * (22/7) * 512

V = 2145.52cm³

Step 2 - Determine the mass of Gold required for the sphere to achieve the density of iron ore if the apparent volume is as given in Step 1 above.

Recall that Mass = Density * Volume

Mass = 5.15 *  2145.52

Mass = 11049.45

Step 3 - Find volume of gold based on mass calculated in Step 2 above

Recall that :

Volume = Mass/Density

Thus,

V = 11049.4/19.3

Thus, Volume = 572.51cm³

Step 4 - Find the width of the wall of a hollow sphere for the volume realized in step 3

Recall the initial formula:

Volume of a Hollow = 4/3 R³ – 4/3 r³

Thus, 572.51 = (4/3) (8³ - (8 - t)³)

572.51 = (4/3) *(22.7) *(8³ - (8 - t)³)

572.51 = (88/21) *(8³ - (8 - t)³)

Multiply both sides by 21 and we have

88 (512 - (8 - t)³) = 12,022.71

Simplify further
(8 - t)³ = 357.38

t = 0.9035cm

Learn more about Volume of a Hollow Sphere at:
brainly.com/question/15244746
#SPJ1

You might be interested in
Buffer consists of undissociated acid (ha) and the ion made by dissociating the acid (a-). How does this system buffer a solutio
docker41 [41]

In buffer solution there is an equilibrium between the acid  HA and its conjugate base A⁻: HA(aq) ⇌ H⁺(aq) + A⁻(aq).

When acid (H⁺ ions) is added to the buffer solution, the equilibrium is shifted to the left, because conjugate base (A⁻) reacts with hydrogen cations from added acid, according to Le Chatelier's principle: H⁺(aq) + A⁻(aq) ⇄ HA(aq). So, the conjugate base (A⁻) consumes some hydrogen cations and pH is not decreasing (less H⁺ ions, higher pH of solution).

A buffer can be defined as a substance that prevents the pH of a solution from changing by either releasing or absorbing H⁺ in a solution.

Buffer is a solution that can resist pH change upon the addition of an acidic or basic components and it is able to neutralize small amounts of added acid or base, pH of the solution is relatively stable


3 0
3 years ago
Most elements on the periodic table are
ivanzaharov [21]

Answer:

Metals

Explanation:

hope this helps

5 0
2 years ago
Read 2 more answers
What does combustion mean
frutty [35]

Answer:

combustion is a high-temperature exothermic redox chemical reaction between a fuel and an oxidant, usually atmospheric oxygen, that produces oxidized, often gaseous products, in a mixture termed as smoke.

6 0
2 years ago
Consider the following reaction:
adell [148]

Answer:

1. d[H₂O₂]/dt = -6.6 × 10⁻³ mol·L⁻¹s⁻¹; d[H₂O]/dt = 6.6 × 10⁻³ mol·L⁻¹s⁻¹

2. 0.58 mol

Explanation:

1.Given ΔO₂/Δt…

    2H₂O₂     ⟶      2H₂O     +     O₂

-½d[H₂O₂]/dt = +½d[H₂O]/dt = d[O₂]/dt  

d[H₂O₂]/dt = -2d[O₂]/dt = -2 × 3.3 × 10⁻³ mol·L⁻¹s⁻¹ = -6.6 × 10⁻³mol·L⁻¹s⁻¹

 d[H₂O]/dt =  2d[O₂]/dt =  2 × 3.3 × 10⁻³ mol·L⁻¹s⁻¹ =  6.6 × 10⁻³mol·L⁻¹s⁻¹

2. Moles of O₂  

(a) Initial moles of H₂O₂

\text{Moles} = \text{1.5 L} \times \dfrac{\text{1.0 mol}}{\text{1 L}} = \text{1.5 mol }

(b) Final moles of H₂O₂

The concentration of H₂O₂ has dropped to 0.22 mol·L⁻¹.

\text{Moles} = \text{1.5 L} \times \dfrac{\text{0.22 mol}}{\text{1 L}} = \text{0.33 mol }

(c) Moles of H₂O₂ reacted

Moles reacted = 1.5 mol - 0.33 mol = 1.17 mol

(d) Moles of O₂ formed

\text{Moles of O}_{2} = \text{1.33 mol H$_{2}$O}_{2} \times \dfrac{\text{1 mol O}_{2}}{\text{2 mol H$_{2}$O}_{2}} = \textbf{0.58 mol O}_{2}\\\\\text{The amount of oxygen formed is $\large \boxed{\textbf{0.58 mol}}$}

8 0
3 years ago
You are in a laboratory creating a new chocolate bar. You want to create the sweetest chocolate bar by maximizing the sugar conc
svetoff [14.1K]
Water helps dissolve sugar
3 0
3 years ago
Read 2 more answers
Other questions:
  • Mercury(II) oxide (HgO) decomposes to form mercury (Hg) and oxygen (O2). The balanced chemical equation is shown below. 2HgO mc0
    15·2 answers
  • What are the conditions of an EF4?
    14·1 answer
  • Identify each type of titration curve. note that the analyte is stated first, followed by the titrant.
    14·1 answer
  • The answer is what I need to know thank you
    11·1 answer
  • You have 1 1/2 moles of 1 kg bottles of O2. What is the mass of O2 that you have? A. 9.033x10^23 kg B. 9.033x10^23 atoms C. 1.80
    10·2 answers
  • The atomic number of an element configuration 2,8, 8,2,13​
    12·1 answer
  • if you react 28 grams of butene with excess hydrogen how many grams of butane would you expect to get
    12·1 answer
  • sound travels 1,500 m/s through water at 25 degrees celciesunder these conditions how long would it take to travel 300m
    7·1 answer
  • What would be the mass, in grams, of 1.505 x 1023 molecules of carbon disulfide?
    5·1 answer
  • How many moles of xenon trioxide are present in 1. 69 grams of this compound.
    10·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!