Organic hydrogenation reactions, in which H2 and an "unsaturated" organic compound combine, are used in the food, fuel, and polymer industries. In the simplest case, ethene (C2H4) and H2 form ethane (C2H6). If 144 kJ is given off per mole of C2H4 reacting, how much heat is released when 14.6 kg of C2H6 forms?
Write the balanced chemical reaction:
C2H4 + H2 -> C2H6 , ΔH = -144 kJ/mol C2H4
Then we get the number of moles of C2H4 using the given mass, 14.6 kg of C2H6.
Molar mass, C2H6 = 2*12 + 6*1 = 30 g/mol
n,C2H6 = 14.6 * 1000 g / 30 g/mol = 486.67 mol
Since the mole ratio for C2H4 and C2H6 is 1:1,
n,C2H4 = 486.67 mol
Finally, we multiply the energy by this number of moles:
-144 kJ/mol C2H4 * 486.67 mol C2H4
= -70,080 kJ
Note that the negative sign just indicates that the heat is released.
Hope this helps~ :)
To find out how much heat is released when 14.6 kg of C2H6 forms, we need to first determine the number of moles of C2H6. We can use the molar mass of C2H6 to calculate this.
The molar mass of C2H6 is the sum of the atomic masses of carbon and hydrogen, which can be found on the periodic table.
Molar mass of C = 12.01 g/mol
Molar mass of H = 1.01 g/mol
Molar mass of C2H6 = (2 * Molar mass of C) + (6 * Molar mass of H)
= (2 * 12.01 g/mol) + (6 * 1.01 g/mol)
= 24.02 g/mol + 6.06 g/mol
= 30.08 g/mol
Now, let's convert the given quantity of 14.6 kg to grams:
14.6 kg * 1000 g/kg = 14,600 g
Next, we can use the molar mass of C2H6 to calculate the number of moles:
Number of moles = Mass / Molar mass
= 14,600 g / 30.08 g/mol
Now we have the number of moles of C2H6. Since we know that 144 kJ is released per mole of C2H4 reacting, we can use this information to determine the total amount of heat released.
Heat released = Number of moles * Heat of reaction
= (14,600 g / 30.08 g/mol) * 144 kJ/mol
Now, let's calculate the value:
Heat released = (14,600/30.08) * 144 kJ
≈ 703.32 kJ
Therefore, approximately 703.32 kJ of heat is released when 14.6 kg of C2H6 forms.
To determine the amount of heat released when 14.6 kg of C2H6 forms, we first need to convert the mass of C2H6 to moles.
The molar mass of C2H6 is calculated by adding the atomic masses of carbon (C) and hydrogen (H):
C2H6 = (2 × atomic mass of C) + (6 × atomic mass of H)
C2H6 = (2 × 12.01 g/mol) + (6 × 1.008 g/mol)
C2H6 = 24.02 g/mol + 6.048 g/mol
C2H6 = 30.068 g/mol
Now we can calculate the number of moles of C2H6 by dividing the mass of C2H6 by its molar mass:
Number of moles of C2H6 = mass of C2H6 / molar mass of C2H6
Number of moles of C2H6 = 14.6 kg × (1000 g/kg) / 30.068 g/mol
Number of moles of C2H6 = 486.98 mol
Now that we know the number of moles of C2H6 formed, we can calculate the heat released per mole of C2H6 using the given value of 144 kJ/mol:
Heat released = number of moles of C2H6 × heat released per mole of C2H6
Heat released = 486.98 mol × 144 kJ/mol
Heat released = 70,179.12 kJ
Therefore, 14.6 kg of C2H6 forms, releasing approximately 70,179.12 kJ of heat.