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arlik [135]
3 years ago
6

The temperature of a sample of gas in steel container at 30.3 Atm is

Chemistry
2 answers:
vladimir1956 [14]3 years ago
6 0

Answer:

74.09 atm

Explanation:

Using the gas laws ( Charles and Boyle's law). We have the formula ,

P1/T1 = P2/T2

Where P1 = 30.3atm

T1 = -100 degree Celsius

to kelvin = -100+ 273 = 173K

T2 = 150 degree Celsius

To Kelvin = 150 = 150+273 = 423K

Imputing values

P1/T1 = P2/T2

30.3/173 = P2/ 423

Cross multiply

173×P2 = 30.3 ×423

173P2 = 12816.9

Divide both sides by 173

P2 = 12816.9/173

P2 = 74.09 atm

I hope this was helpful, please mark as brainliest

ddd [48]3 years ago
6 0

Answer:

P2=74.086atm

Explanation:

Using the formula p1/t1=P2/t2

P1=30.3atm

P2=?

T1=-100°c to Kelvin=273-100=173k

T2=150°c to Kelvin=273+150=423k

30.3\173=x/423

Cross multiply

173x=423×30.3

173x=12816.9

Divide both sides by 173

X=74.086atm

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How much energy must be removed from a 94.4 g sample of benzene (molar mass= 78.11 g/mol) at 322.0 K to solidify the sample and
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Answer : The energy removed must be, 29.4 kJ

Explanation :

The process involved in this problem are :

(1):C_6H_6(l)(322K)\rightarrow C_6H_6(l)(279K)\\\\(2):C_6H_6(l)(279K)\rightarrow C_6H_6(s)(279K)\\\\(3):C_6H_6(s)(279K)\rightarrow C_6H_6(s)(205K)

The expression used will be:  

Q=[m\times c_{p,l}\times (T_{final}-T_{initial})]+[m\times \Delta H_{fusion}]+[m\times c_{p,s}\times (T_{final}-T_{initial})]

where,

Q = heat released for the reaction = ?

m = mass of benzene = 94.4 g

c_{p,s} = specific heat of solid benzene = 1.51J/g^oC=1.51J/g.K

c_{p,l} = specific heat of liquid benzene = 1.73J/g^oC=1.73J/g.K

\Delta H_{fusion} = enthalpy change for fusion = -9.8kJ/mol=-\frac{9.8\times 1000J/mol}{78g/mol}=-125.6J/g

Now put all the given values in the above expression, we get:

Q=[94.4g\times 1.73J/g.K\times (279-322)K]+[94.4g\times -125.6J/g]+[94.4g\times 1.51J/g.K\times (205-279)K]

Q=-29427.312J=-29.4kJ

Negative sign indicates that the heat is removed from the system.

Therefore, the energy removed must be, 29.4 kJ

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3 years ago
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In a study of the formation of NOx air pollution, a chamber heated to 2200°C was filled with air (0.790 atm N₂, 0.210 atm O₂). W
Irina-Kira [14]

Answer:

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O₂ = 0.1715atm

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For the reaction:

N₂(g) + O₂(g) ⇄ 2NO(g)

Where Kp is defined as:

Kp = \frac{P_{NO}^2}{P_{N_2}P_{O_2}}}

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Replacing in Kp:

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0.0460 = 4X² / 0.1659 - X + X²

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Solving for X:

X = - 0.050 → False answer. There is no negative concentrations.

X = <em>0.0385 atm</em> → Right answer.

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O₂ = 0.210atm - X = <em>0.1715atm</em>

NO = 2X = <em>0.0770atm</em>

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