Answer:
The answer that is true is A
Explanation:
The first thing to do is to perform stoichiometry relationships and calculations.
First relationship: 0.3 moles of CO₂ are produced
6 mol CO₂ _____ 1 mol C₆H₁₂O₆
0.3 mol CO₂ _____ X = 0.05 mol of C₆H₁₂O₆
Calculation: 0.3 mol x 1 mol / 6 mol = 0.05 mol of C₆H₁₂O₆
Second relationship: 0.60 moles of CO₂ are produced
6 mol CO₂ _____ 1 mol C₆H₁₂O₆
0.6 mol CO₂_____ X = 0.1 mol of C₆H₁₂O₆
Calculation: 0.6 mol x 1 mol / 6 mol = 0.1 mol of C₆H₁₂O₆
6 mol CO₂ _____ 6 mol O₂
0.6 mol CO₂ _____ X = 0.6 mol of O₂
Calculation: 0.6 mol x 6 mol / 6 mol = 0.6 mol of O₂
Then, the answer that is true is A, because in order for 0.6 moles of CO₂ to be produced, there must initially be 0.1 mol of C6H12O6 as calculated.
The B is not correct because for more CO₂ to be produced, more C₆H₁₂O₆ must react, this is defined according to Proust's law or law of defined proportions, stated as: “When the combination of two or more elements occurs to form a new compound, they always do it in a mass relationship that is completely constant”. It is by this law that no more CO₂ can be produced with the same amount of C₆H₁₂O₆ reagent.
The C is not correct either, although the temperature and volume of the container are the same, the O₂ is in excess to react, so 0.6 mol of it is needed to produce 0.6 mol of CO₂, according to the calculations made .
The D is not correct because it would also not respect the law of defined proportions or Proust's law. Although O₂ is in excess, it cannot react more than the stoichiometric ratio. Simply, if it is in excess, the rest of the O₂ will remain unreacted.
Answer:
For the reaction to proceed, the initial amount of [tex]\rm C_6H_1_2O_6[/tex] in the container must have been 0.010 moles.
Explanation:
The reaction represents the decomposition of glucose. From the stoichiometry of the balanced equation,
[tex]\rm C_6H_1_2O_6\;+\;6\;CO_2\;\rightarrow\;6\;CO_2\;+\;6\;H_2O[/tex]
1 mole of [tex]\rm C_6_H_1_2O_6[/tex] produces 6 moles of [tex]\rm CO_2[/tex].
In first statement there is 0.30 moles of [tex]\rm CO_2[/tex] was produced.
For the production of 0.30 moles of [tex]\rm CO_2[/tex], [tex]\rm C_6_H_1_2O_6[/tex] required is:
0.05 moles of [tex]\rm C_6_H_1_2O_6[/tex] is required.
For the production of 0.60 moles of [tex]\rm CO_2[/tex], [tex]\rm C_6_H_1_2O_6[/tex] required is:
0.1 moles of [tex]\rm C_6H_1_2O_6[/tex] is required.
Since the total required amount of [tex]\rm C_6H_1_2O_6[/tex] is 0.1 + 0.05 moles
= 0.105 moles.
The minimum required amount of [tex]\rm C_6H_1_2O_6[/tex] will be 0.10 moles.
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