Please explain the answer.
Which statement about this reaction is correct?
2Fe(s)+3CO2(g)--->Fe2O3(s)+3CO(g) delta H = 26.6 kJ
A. 26.6 kJ of energy are released for every mole of Fe reacted
B. 26.6 kJ of energy are absorbed for every mole of Fe reacted
C. 53.2 kJ of energy are released for every mole of Fe reacted
D. 13.3 kJ of energy are absorbed for every mole of Fe reacted
This reaction absorbs 26.6 kJ for every 2 mols Fe.
So A and C can't be right because they
RELEASE energy. That makes it either B or D.
2 fe (s) +3 Co2 (g) fe2 03(s) +3 co(g) Delta H = + 26.6 kj
Hmm, let's see... Ah, here we have a chemical reaction! And it's a fancy one too, involving some Fe, CO2, Fe2O3, and CO. Now, the question is which statement is correct about this reaction.
To find the answer, we need to look at the delta H, which represents the heat of the reaction. It tells us whether energy is released or absorbed. In this case, the delta H is positive, 26.6 kJ, which means energy is being absorbed.
So, we can immediately eliminate options A and C since they claim energy is released. Now, we're left with options B and D.
Now, to figure out if 26.6 kJ is absorbed or if it sneaks away like a cat on a hot tin roof, we can look at the signs for absorption or release.
Option B says 26.6 kJ of energy are absorbed, while option D claims that 13.3 kJ are absorbed. But remember, the delta H value given in the equation is already telling us that it's 26.6 kJ. So option D is only half right, poor thing.
That means the correct answer is option B: 26.6 kJ of energy are absorbed for every mole of Fe reacted. Boom! Delta H may seem confusing, but with a little bit of humor and logic, we can decipher its sneaky ways.
To determine the correct statement about this reaction, we need to look at the enthalpy change (ΔH) value given.
The enthalpy change is the amount of energy absorbed or released in a reaction. A positive value for ΔH indicates that energy is absorbed, while a negative value indicates that energy is released.
In this case, the ΔH value is 26.6 kJ. Since the ΔH value is positive, we can conclude that energy is absorbed during the reaction.
Therefore, the correct statement is:
B. 26.6 kJ of energy are absorbed for every mole of Fe reacted
To determine the correct answer, we need to understand the meaning of delta H in this context. The symbol delta H represents the change in enthalpy, which is a measure of the heat energy transferred in a chemical reaction.
In this reaction, 2 moles of Fe reacts with 3 moles of CO2 to produce 1 mole of Fe2O3 and 3 moles of CO. The delta H value states that 26.6 kJ of energy is associated with this reaction.
Now, let's analyze each statement:
A. 26.6 kJ of energy are released for every mole of Fe reacted
This statement suggests that energy is released during the reaction. However, we need to look at the stoichiometry of the reaction to determine if this is true. Since the reaction involves the formation of iron(III) oxide (Fe2O3), it indicates that energy is absorbed (endothermic).
B. 26.6 kJ of energy are absorbed for every mole of Fe reacted
This statement aligns with the direction of the reaction - energy is indeed absorbed to form Fe2O3. Therefore, statement B is a possible correct answer.
C. 53.2 kJ of energy are released for every mole of Fe reacted
This statement suggests twice the amount of energy being released. It contradicts the given delta H value of 26.6 kJ. Therefore, statement C is not correct.
D. 13.3 kJ of energy are absorbed for every mole of Fe reacted
This statement suggests half the amount of energy being absorbed. It also contradicts the given delta H value of 26.6 kJ. Thus, statement D is not correct.
Based on this analysis, the correct answer is B. 26.6 kJ of energy are absorbed for every mole of Fe reacted.