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3 years ago

Titanium metal is used as a structural material in many high-tech applications such as in jet engines.

Chemistry

1 answer:

Elza [17]3 years ago

3 0

Answer:

a. $Cp=0.523$

b. $Cp=25.02\frac{J}{mol^\circ C}$

Explanation:

a. First, we solve the specific heat equation as follows:

$Q=mCp\Delta T\\Cp=\frac{Q}{m\Delta T}\\Cp=\frac{89.7J}{33.0g\times5.20^\circ C}=0.523$

b. Then, we use the molar mass of titanium to determine its molar heat capacity, as follows:

$Cp=0.523\frac{J}{g^\circ C}\times 47.87\frac{g}{mol}\\Cp=25.02\frac{J}{mol^\circ C}$

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Mars2501 [29]

Explanation:

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15=5×b
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2.area of rectangle=l×b

28=l×4
l=7cm

3. perimeter of square=4×L

24=4×L
L=6cm

4. perimeter of rectangle=2(L+b)

14=2(4+b)
14=8+2b
2b=6
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3 years ago

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Identify the arrows that show removal of thermal energy when matter changes state.

8090 [49]

Let's identify first the phases of matter inside each of those beakers. The first beaker on the left has a compact shape and has its own volume. So, that must be solid. The middle beaker has a compact shape but it takes the shape of its container. So, that must be liquid. The third beaker on the right is gas because the molecules are far away from each other.

After identifying each states, let's investigate the energy for phase change. Let's start with the arrows pointing to the right. The first arrow to the right is a phase change from solid to liquid. The intermolecular forces in a solid is the strongest among the three phases of matter. So, you would need an input of energy to break them apart into liquid. The same is true for the phase change from liquid to gas. Therefore, all the arrows pointing to the right require an input of energy.

The reverse arrows pointing to the left needs to release energy. The molecules in the gas state are free such that they can travel from one point to another easily. They have the highest amount of energy. So, if you want the molecules to come closer together, you need to remove the energy to keep them in place. Therefore, the arrows pointing to the right require removal of energy.

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3 years ago

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determine the grams of NH3 produced when 6.70 grams of N2 is consumed using the following equation: N2 + 3H2 = 2NH3

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3 years ago

Light brings many chemical changes. Can you think of any chemical change brought about by light?

strojnjashka [21]

Answer:

MRCORRECT has answered the question

Explanation:

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4 years ago

If you place 1.0 L of ethanol (C2H5OH) in a small laboratory that is 3.0 m long, 2.0 m wide, and 2.0 m high, will all the alcoho

ankoles [38]

If you place 1.0 L of ethanol (C2H5OH) in a small laboratory that is 3.0 m long, 2.0 m wide, and 2.0 m high, will all the alcohol evaporate? If some liquid remains, how much will there be? The vapor pressure of ethyl alcohol at 25 °C is 59 mm Hg, and the density of the liquid at this temperature is 0.785g/cm^3 .

will all the alcohol evaporate? or none at all?

Answer:

Yes, all the ethanol present in the laboratory will evaporate since the mole of ethanol present in vapor is greater. The volume of ethanol left will therefore be zero.

Explanation:

Given that:

The volume of alcohol which is placed in a small laboratory = 1.0 L

Vapor pressure of ethyl alcohol at 25 ° C = 59 mmHg

Converting 59 mmHg to atm ; since 1 atm = 760 mmHg;

Then, we have:

= $\frac{59}{760}atm$

= 0.078 atm

Temperature = 25 ° C

= ( 25 + 273 K)

= 298 K.

Density of the ethanol = 0.785 g/cm³

The volume of laboratory = l × b × h

= 3.0 m × 2.0 m × 2.5 m

= 15 m³

Converting the volume of laboratory to liter;

since 1 m³ = 100 L; Then, we have:

15 × 1000 = 15,000 L

Using ideal gas equation to determine the moles of ethanol in vapor phase; we have:

PV = nRT

Making n the subject of the formula; we have:

$n = \frac{PV}{RT}$

$n = \frac{0.078 * 15000}{0.082*290}$

n = 47. 88 mol of ethanol

Moles of ethanol in 1.0 L bottle can be calculated as follows:

Since numbers of moles = $\frac{mass}{molar mass}$

and mass = density × vollume

Then; we can say ;

number of moles = $\frac{density*volume }{molar mass of ethanol}$

number of moles = $\frac{0.785g/cm^3*1000cm^3}{46.07g/mol}$

number of moles = $\frac{&85}{46.07}$

number of moles = 17.039 mol

Thus , all the ethanol present in the laboratory will evaporate since the mole of ethanol present in vapor is greater. The volume of ethanol left will therefore be zero.

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3 years ago