Mole ConceptHard
Question
When a certain amount of octane, C8H18, is burnt completely, 7.04 g CO2 is formed. What is the mass of H2O formed simultaneously?
Options
A.1.62 g
B.6.48 g
C.3.24 g
D.2.28 g
Solution
$C_{8}H_{18} + \frac{25}{2}O_{2} \rightarrow 8CO_{2} + 9H_{2}O$
8 × 44 g 9 × 18 g
$\therefore 7.04g \frac{9 \times 18}{8 \times 44} \times 7.04 = 3.24\text{ g}$
Create a free account to view solution
View Solution FreeMore Mole Concept Questions
Volume of a gas at NTP is 1.12 × 10-7cc. The number of molecule in it is :...The molecular formula of a non stoichiometric oxide of vanadium is VO1.8. The oxide contain both V3+ and V4+ ions. The m...Law of multiple proportions is not applicable for the oxide(s) of...A protein isolated from a bovine preparation, was subjected to amino acid analysis. The amino acid present in the smalle...One mole of the aquous solution of complex CoCl3.4NH3 passess through anion exchange resine and resulting solution treat...