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Jobisdone [24]
3 years ago
10

During a reaction, the enthalpy of formation of an intermediate is 90.3 kJ/mol. During the reaction, 2 moles of the intermediate

are formed as a reactant. What is the enthalpy value for this step of the reaction?
A. -180.6 kJ

B. 90.3 kJ

C. -90.3 kJ

D. 180.6 kJ​
Chemistry
1 answer:
Soloha48 [4]3 years ago
7 0

Answer:

180.6 kJ​

Explanation:

The enthalpy of reaction refers to the energy absorbed or released during a reaction. If heat is absorbed in a reaction, the enthalpy of reaction is positive. If heat is released in a reaction, the enthalpy of reaction his negative.

Since the energy absorbed when one mole of the intermediate is formed is 90.3 kJ/mol, then, when two moles of intermediate is formed, 2 × 90.3 kJ/mol = 180.6 kJ​ of energy is absorbed.

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A sample of PCl5(g) was placed in an otherwise empty flask at an initial pressure of 0.500 atm and a temperature above 500 K. Ov
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Answer:

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                     PCl₅ (g)      ⇔          PCl₃ (g) +       Cl₂ (g)

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t = eq                -x                             x                      x

--------------------------------------------- --------------------------

Moles at eq: 0.500-x                       x                      x

       

Given the pressure of PCl₅ at equilibrium = 0.150 atm

Thus, 0.500 - x = 0.150

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K_p=\frac{x^2}{0.500-x}  

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Titanium has an HCP crystal structure, a c/a ratio of 1.669, an atomic weight of 47.87 g/mol, and a density of 4.51 g/cm3. Compu
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Answer : The atomic radius for Ti is, 1.45\times 10^{-8}cm

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where,

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Now put all the values in above formula (1), we get

4.51g/cm^3=\frac{6\times (47.87g/mol)}{(6.022\times 10^{23}mol^{-1}) \times V}

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Formula used :

V=6R^2c\sqrt{3}

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Now put (c = 1.669 a) and (a = 2R) in this formula, we get:

V=6R^2\times (1.669a)\sqrt{3}

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