The mass of CO₂ gas produced during the combustion of one gallon of octane is 8.21 kg.
The given parameters:
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The mass of the octane burnt is calculated as follows;
The combustion reaction of octane is given as;
From the reaction above:
228.46 g of octane -------------------> 704 g of CO₂ gas
2,664.37 of octane --------------------> ? of CO₂ gas
Thus, the mass of CO₂ gas produced during the combustion of one gallon of octane is 8.21 kg.
Learn more about combustion of organic compounds here: brainly.com/question/13272422
Answer:
Explanation:
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In this case, since the acid is monoprotic and the KOH has one hydroxyl ion only, we can see that at the equivalence point the moles of both of them are the same:
Thus, since we are given 1.70 g of the acid, we compute the moles of acid that were titrated:
Which equal the moles of KOH. In such a way, since the molarity is defined as moles over liters (M=n/V), the liters are moles over molarity (V=n/M), thus, the resulting volume is:
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Answer:
a. 63.2%
b. 11.7%
c. 73.3%
d. 0.995%
e. 55.5%
Explanation:
An ionic compound is a compound that is formed by ions, so one of the elements must donate electrons (which is the cation, the positive ion), and the other will receive these electrons (which is the anion, the negative ion).
The power of an element has to attract the electrons is called electronegativity, and so, as higher is the difference of electronegative of the elements, it is more probable that one of them will "still" the electrons and will form an ionic compound. The percent of this ionic character can be found by the Pauling's equation:
*100%
Where is the electronegativity difference of the elements. Thus, consulting an electronegativity table:
a. = 1.5
= 3.5
*100%
%IC = 63.2%
b. = 1.6
= 2.1
*100%
%IC = 11.7%
c. = 0.7
= 3.0
*100%
%IC = 73.3%
d. = 1.7
= 1.9
*100%
%IC = 0.995 %
e. = 1.2
= 3.0
*100%
%IC = 55.5%