When 18.5 g of K2O(s) is completely dissolved by HI(aq), how many grams of KI(aq) form in solution?
Step 1 of 3
Here we have to calculate the mass of KI in gram.
The given mass of K2O = 18.5 g
K2O (s) + 2HI (aq) 2KI (aq) + H2O (l)
Moles = mass solute/ molecular mass = 18.5 /94.196 = 0.196 0.12 moles
Here 1 mole of K2O has formed 2 moles of KI.
Molecular mass of KI = 166.0028 g/mole
Moles = gram/ molecular weight
Or, gram = moles molecular weight
= 39.84 g
Thus the mass of KI is 39.84 g
Textbook: Introductory Chemistry
Author: Nivaldo J Tro
This full solution covers the following key subjects: completely, Dissolved, form, grams, solution. This expansive textbook survival guide covers 19 chapters, and 2046 solutions. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The full step-by-step solution to problem: 93P from chapter: 14 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. Since the solution to 93P from 14 chapter was answered, more than 895 students have viewed the full step-by-step answer. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. The answer to “When 18.5 g of K2O(s) is completely dissolved by HI(aq), how many grams of KI(aq) form in solution?” is broken down into a number of easy to follow steps, and 18 words.