d= 8/10 so yah that was a guess
∆H° of the following reaction H₂(g) + I₂(g) → 2HI(g) is -3kJ/mol.
<h3>What is Bond Enthalpy? </h3>
The minimum amount of energy which is required to braak down or form the bonds in chemical reaction is known as bond enthalpy.
It can be calculated as:
∆Hrxn = sum of ∆H bond broken - sum. of ∆H of bond formed.
In order to Calculate ∆Hrxn for the given equation we have:
Bond energies in kJ/mol
- H—H = 436
- H—I = 295
- I—I = 151
Now, the given reaction is
H₂(g) + I₂(g) → 2HI(g)
Here, 1 mol of H₂ and 1 mole of I₂ breaks to form 2 moles of HI.
Therefore,
We know that,
∆Hrxn = B. E(H—H) + B. E(I—I) - 2B. E(H—I)
= 436 + 151 - 2× 295
= 436+ 151 - 590
∆Hrxn = -3kJ/mol.
Thus, from the above conclusion we can say that ∆Hrxn of the reaction H₂(g) + I₂(g) → 2HI(g) is -3kJ/mol.
learn more about Bond energy:
brainly.com/question/26964179
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Answer:
Percent yield = 88%
Explanation:
Given data:
Mass of C₇H₆O₃ = 200.0 g
Actual yield of aspirin = 231 g
Percent yield = ?
Solution:
Chemical equation:
C₇H₆O₃ + C₄H₆O₃ → C₉H₈O₄ + C₂H₄O₂
Number of moles of aspirin:
Number of moles = mass/molar mass
Number of moles = 200.0 g/ 138.12 g/mol
Number of moles = 1.45 mol
Now we will compare the moles of aspirin with C₇H₆O₃.
C₇H₆O₃ : C₉H₈O₄
1 : 1
1.45 : 1.45
Theoretical yield of aspirin:
Mass = number of moles × molar mass
Mass = 1.45 g × 180.158 g/mol
Mass = 261.23 g
Percent yield:
Percent yield =( actual yield / theoretical yield )× 100
Percent yield = (231 g/ 261.23 g)× 100
Percent yield = 0.88 × 100
Percent yield = 88%
Answer:
it would be the second option. It responds to stimuli to help protect an organism and maintain structure