N2 + O2 --> 2 NO change in heat (delta H)= 43.2 kcal
based on the reaction, which statement is true?
a) 43.2 kcal are consumed when 1.00g of O2 reacts
b) 43.2 kcal are consumed when 1.00g of N2 reacts
c) 43.2 kcal are consumed when 1.00g of NO is produced
d) 43.2 kcal are consumed when 1.00 mole of O2 reacts
I think it is D because the heat is used when the reaction occurs and the product is made. Is this correct?
I have a problem with your reasoning. All of the answers "are consumed" so any could be true based on that alone. As for the product being made why wouldn't c be just as true? NO is a product and it is made? And for that matter, why choose d based on formation of NO? Why not a or b for reactant used?
You are correct that D is the right answer but you don't get credit for that because you are guessing.
i need help to make a data for my project but i don't know how close can a magnet be from the staples after it will pick up the objects but i don't know how to put in a data
1. If you have a new post, you are unlikely to get an answer posting piggy back onto another question. Go to the top of the page, click on Post a New Question, and make your post.
2. When you use these boards, don't use text style typing. Begin sentences with a capital letter and end them with periods. Write I when you mean I and not i.
3. For this particular question, you need to clarify exactly what you want. I can tell it has something to do with magnets and staples but that's all I can decipher.
Yes, you are correct! In order to determine which statement is true, let's analyze the given reaction: N2 + O2 -> 2 NO
The delta H, which represents the change in heat, is given as 43.2 kcal. This value indicates the amount of heat that is absorbed or released during the reaction.
Now, let's evaluate each statement to see which one is true:
a) 43.2 kcal are consumed when 1.00g of O2 reacts. To determine if this statement is true, we need to calculate the amount of O2 that reacts. We can use the molar mass of O2 (32 g/mol) to find the number of moles of O2 in 1.00g. Once we know the number of moles involved, we can then calculate the amount of heat consumed.
b) 43.2 kcal are consumed when 1.00g of N2 reacts. Again, we need to calculate the number of moles of N2 in 1.00g and then determine the amount of heat consumed.
c) 43.2 kcal are consumed when 1.00g of NO is produced. Similar to the previous statements, we need to calculate the number of moles of NO produced from 1.00g of NO, and then determine the associated heat consumed.
d) 43.2 kcal are consumed when 1.00 mole of O2 reacts. This statement allows us to directly compare the given delta H value (in kcal) to the number of moles of O2 involved in the reaction.
Considering the given reaction and the definition of delta H, statement d) is true. The delta H value of 43.2 kcal represents the heat consumed when 1.00 mole of O2 reacts.
Therefore, the correct answer is d) 43.2 kcal are consumed when 1.00 mole of O2 reacts.