posted by Lauren K. on .
Consider the following reaction:
H2O(l) + 3NO2(g) --> 2HNO3(l) + NO(g)
What volume of NO (in L) is produced starting from 1.80 g of water and 11.5 g of NO2 at 300 K and 1 atm? (use R = 0.0821 L atm/mol K).
I am completely confused :(
This is a limiting reagent problem. How do I know that? Because BOTH reactants are given. The way you solve these is to wrote a stoichiometry problem using each reagent, see how much of the product will be formed, then take the smaller value as the correct number. Here is a worked example of a stoichiometry problem. Work it once (to the mole stage of the product) with the first reagent, then a second time (to the mole stage) using the second reagent. When the numbers don't agree, always use the smaller value.
Here is the example, just follow the steps.