In the reaction below, what is the limiting reactant when 1.24 moles NH3 of reacts with 1.79 moles of NO? 4NH_3 + 6NO (right arrow) 5N_2 + 6H_2O

1. NO
2. H_2O
3. NH_3
4. N_2

1. NO .

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to identify the limiting reactant by simply calculating the moles of any product, say N2, via the moles of each reactant and including the corresponding mole ratio (4:5 and 6:5):

Thus, since NO yields the fewest moles of N2 product, we infer it is the limiting reactant.

Regards!

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.