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AlladinOne [14]
3 years ago
11

(a) Sketch, in a cubic unit cell, a [111] and a [112] lattice direction. (b) Use a trigonometric calculation to determine the an

gle between these two directions. (c) Use Equation 3.3 to determine the angle between these two directions.

Chemistry
1 answer:
fgiga [73]3 years ago
7 0

Answer and Explanation:

a) The direction is shown in the cube diagram attached to this solution.

b) the angle between two planes (h₁, k₁, l₁) and (h₂, k₂, l₂) is given by the formula,

Cos Φ = (h₁h₂ + k₁k₂ + l₁)/√((h₁² + k₁² + l₁²)(h₂² + k₂² + l₂²))

For (111) and (112)

Cos Φ = (1.1 + 1.1 + 1.2)/√((1² + 1² + 1²)(1² + 1² + 2²))

Cos Φ = (1 + 1 + 2)/√((1+1+1)(1+1+4))

Cos Φ = 4/√(3×6)

Cos Φ = 4/√18

Φ = cos⁻¹ (4/√18) = 19.56°

c) equation 3.3 is missing from the question, I would be back to provide the answers to that as soon as the equation is provided!

Hope this Helps!!

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It's the rows. They are periods. (1,2,3,4,5,6,7 - the ones without the letters).
6 0
3 years ago
When a mixture of sulfur and metallic silver is heated, silver sulfide is produced. What mass of silver sulfide is produced from
IgorLugansk [536]

The question is incomplete, here is the complete question.

When a mixture of sulfur and metallic silver is heated, silver sulfide is produced. What mass of silver sulfide is produced from a mixture of 3.0g Ag and 3.0g S_8.

Answer : The mass of silver sulfide is produced from a mixture is 3.44 grams.

Explanation : Given,

Mass of Ag = 3.0 g

Mass of S_8 = 3.0 g

Molar mass of Ag = 107.8 g/mole

Molar mass of S_8 = 256 g/mole

Molar mass of Ag_2S = 247.8 g/mole

First we have to calculate the moles of Ag and S_8.

\text{ Moles of }Ag=\frac{\text{ Mass of }Ag}{\text{ Molar mass of }Ag}=\frac{3.0}{107.8g/mole}=0.0278moles

\text{ Moles of }S_8=\frac{\text{ Mass of }S_8}{\text{ Molar mass of }S_8}=\frac{3.0g}{256g/mole}=0.0117moles

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

16Ag(s)+S_8(s)\rightarrow 8Ag_2S(s)

From the balanced reaction we conclude that

As, 16 mole of Ag react with 1 mole of S_8

So, 0.0278 moles of Ag react with \frac{0.0278}{16}=0.00174 moles of S_8

From this we conclude that, S_8 is an excess reagent because the given moles are greater than the required moles and Ag is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of Ag_2S

From the reaction, we conclude that

As, 16 mole of Ag react to give 8 mole of Ag_2S

So, 0.0278 moles of Ag react to give \frac{0.0278}{16}\times 8=0.0139 moles of Ag_2S

Now we have to calculate the mass of Ag_2S

\text{ Mass of }Ag_2S=\text{ Moles of }Ag_2S\times \text{ Molar mass of }Ag_2S

\text{ Mass of }Ag_2S=(0.0139moles)\times (247.8g/mole)=3.44g

Therefore, the mass of silver sulfide is produced from a mixture is 3.44 grams.

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3 years ago
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Answer:

no it can not

Explanation:

6 0
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Which of the following describes an atom?
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Answer:

Correct answer is option (3) .

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7 0
3 years ago
B. If the sand you ran across has a specific-heat capacity of 835 J/(kgºc),
Murrr4er [49]

Answer: 16700 Joules

Explanation:

The quantity of heat required to raise the temperature of a substance by one degree Celsius is called the specific heat capacity.

Q=m\times c\times \Delta T

Q = Heat absorbed = ?

m = mass of sand = 2 kg

c = heat capacity = 835J/kg^0C

Initial temperature  = T_i = 40^0C

Final temperature= T_f  = 50^0C

Change in temperature ,\Delta T=T_f-T_i=(50-40)^0C=10^0C

Putting in the values, we get:

Q=2kg\times 835J/kg^0C\times 10^0C

Q=16700J

16700 J of energy must be added to a 2-kilogram pile of it to increase its temperature from 40°C to 50°C

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