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Anni [7]
3 years ago
11

Hydrogenation of double and triple bonds is an important industrial process. Calculate (in kJ/mole) the standard enthalpy change

ΔH° for the hydrogenation of ethyne (acetylene) to ethane. Just enter a number (no units).
Chemistry
1 answer:
Lady bird [3.3K]3 years ago
3 0

Answer:

\Delta _RH=-310.53kJ/mol

Explanation:

Hello,

In this case, the undergoing chemical reaction is:

C_2H_2(g)+2H_2(g)\rightarrow C_2H_6(g)

Thus, the standard enthalpies of formation are:

\Delta _fH_{C_2H_2}=226.73kJ/mol\\\Delta _fH_{H_2}=0kJ/mol\\\Delta _fH_{C_2H_6}=-83.8 kJ/mol

Hence, the standard enthalpy of reaction becomes:

\Delta _RH=-83.8kJ/mol-0kJ/mol-226.73kJ/mol\\\Delta _RH=-310.53kJ/mol

Best regards.

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how many grams of molecular oxygen (O2) is produced from 13.8 grams of calcium chlorate (Ca(ClO3)2)in the following chemical rea
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Answer:

6.72 g

Explanation:

Given data:

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Ca(ClO₃)₂        →      CaCl₂ + 3O₂

Number of moles of calcium chlorate:

Number of moles = mass / molar mass

Number of moles = 13.8 g/ 206.98 g/mol

Number of moles = 0.07 mol

Now we will compare the moles of oxygen and  calcium chlorate.

                 Ca(ClO₃)₂         :            O₂

                      1                   :              3

                    0.07               :            3×0.07=0.21 mol

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Mass = number of moles × molar mass

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