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4 years ago

Can someone please explain how to do number 11?

Chemistry

1 answer:

BaLLatris [955]4 years ago

8 0

Answer:

HBr + Mg(OH)2 —> MgBr2 + H2O.

To balance the above, we must do a head count of the individual atoms present to ensure they balance on both sides of the equation. To get the balance equation, add 2 in front of HBr and 2 in front of H2O as shown below:

2HBr + Mg(OH)2 —> MgBr2 + 2H2O

We can see clearly that the numbers of the individual atoms on the left side is the same on the right side

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What typefs) of bonding would be expected for each of the following materials: solid xenon, calcium fluoride (CaF, bronze, cadmi

klio [65]

Answer:

a) Solid Xenon - only van der waals forces of attractions.

b) Calcium Fluoride - Ionic Bonding

c) Bronze - Metallic Bonding

d) Cadmium telluride - Covalent bonding with slight ionic character.

e) Rubber - Covalent bonding with some van der Waals forces of attraction.

f) Tungsten - Metallic bonding

Explanation:

a) Xenon is a noble gas having fully filled stable electronic configuration.

So, there is no bonding between xenon atoms in solid xenon.

Only van der waals forces of attraction are found.

b) Calcium fluoride is an ionic compound formed from calcium (2+) and Fluoride ion.

c) Bronze is an alloy formed mainly from copper and tin which are both metals.

So, metallic bonding is in found in bronze.

d) Cadmium telluride is formed form cadimium (2+) ion and Telluride ion with -2 charge.

So, it has slight ionic character with predominant covalent bonding

e) Rubber is a polymer which is formed from isoprene units.

So, covalent bonding exists along with van der waals forces.

f) Tungsten is a metal. So, metallic bonding is found between the atoms of tungsten.

8 0

3 years ago

What mass of copper is produced when zinc is added to a solution containing 31.9g copper ii tetraoxosulphate vi

solmaris [256]

Answer:

12.7g of Cu

Explanation:

First let us generate a balanced equation for the reaction. This is illustrated below:

Zn + CuSO4 —> ZnSO4 + Cu

Molar Mass of Cu = 63.5g/mol

Molar Mass of CuSO4 = 63.5 + 32 + (16x4) = 63.5 + 32 + 64 = 159.5g/mol

From the equation,

159.5g of CuSO4 produced 63.5g of Cu.

Therefore, 31.9g of CuSO4 will produce = (31.9 x 63.5) / 159.5 = 12.7g of Cu

4 0

3 years ago

Complete the passage to describe how electrons are represented in electron dot diagrams. The maximum number of dots an electron

romanna [79]

D. 8, A. 2

Hope this helps

6 0

4 years ago

Read 2 more answers

The accepted value is 29.35. Which correctly describes this student's experimental data?

kkurt [141]

Answer:

- Both accurate and precise.

Explanation:

The experimental data is characterized as the data that is generated through a specific test or measurement with the purpose of analysis or evaluation. As per the question, the minuteness of the given data(29.27, 29.32, and 29. 27)most aptly describes that the experimental data collected by the student possesses 'accuracy and precision' apt and specific. It would yield the most worthy and reliable conclusion.

3 0

3 years ago

How many moles of aluminum oxide (Al2O3) can be produced from 12.8 moles of oxygen gas (02)

zhannawk [14.2K]

Answer:

Theoretical Yield

Percent yield

Example stoichiometry problem

How much oxygen can be prepared from 12.25 g KClO3 . (Use molar mass KClO3 = 122.5 g.)

Most stoichiometry problems can be solved using the following steps.

Step 1.

Write and balance the equation for the decomposition of KClO3 with heat (∆). 2KClO3 + ∆ → 2KCl + 3O2

Step 2.

Convert what you have (in this case g KClO3) to moles.

# moles = grams/molar mass = 12.25 g /122.5 = 0.100 mole KClO3.

Step 3.

Using the coefficients in the balanced equation, convert moles of what you have (moles KClO3) to moles of what you want (in this case moles oxygen).

0.100 mol KClO3 x (3 moles O2/2 moles KClO3) = 0.100 x (3/2) = 0.150 mole O2.

Step 4.

Convert moles from step 3 to grams.

moles x molar mass = grams

0.150 mole O2 x (32.0 g O2/mole O2) = 4.80 g O2 produced from 12.25 g KClO3. This is the theoretical yield. If the ACTUAL yield is 4.20 grams, calculate percent yield. Percent yield = (actual yield/theoretical yield) x 100 = (4.20/4.80) x 100 = 87.5% yield

NOTE: In step 1, moles can be obtained other ways; in step 4 moles can be converted to other units.

a. For solutions, M x L = moles (or mL x M = millimoles).

b. For gases, L/22.4 = moles

4 0

3 years ago