Advertisements
Advertisements
Question
Give example of compound whose:
Empirical formula is different from the molecular formula.
Advertisements
Solution
C6H12O6.
APPEARS IN
RELATED QUESTIONS
Ethane burns in oxygen to form CO2 and H2O according to the equation:
\[\ce{2C2H6 + 7O2 -> 4CO2 + 6H2O}\]
If 1250 cc of oxygen is burnt with 300 cc of ethane, calculate:
- the volume of CO2 formed.
- the volume of unused O2.
Give the empirical formula of C2H2
A compound contains 87.5% by mass of nitrogen and 12.5% by mass of hydrogen. Determine the empirical formula of this compound.
The percentage composition of sodium phosphate, as determined by analysis is : 42.1% Na, 18.9% P, 39% of O. Find the empirical formula of the compound.
[H =1, N =14, Na = 23, P = 31, Cl = 35.5, Pt = 195]
A compound 'X' consists of 4.8% of C and 95.2% of Br by mass.
Determine the empirical formula of this compound.
[C = 12, Br = 80]
0.2 g atom of silicon combine with 21.3 g of chlorine. Find the empirical formula of the compound formed.
Give the empirical formula of C6H18O3.
- A compound has the following percentage composition by mass: carbon 14.4%, hydrogen 1.2% and chlorine 84.5%. Determine the empirical formula of this compound. Work correctly to 1 decimal place. (H = 1; C = 12; Cl = 35.5)
- The relative molecular mass of this compound is 168, so what is its molecular formula?
- By what type of reaction could this compound be obtained from ethyne?
The Empirical formula of an organic compound is CHCl2.
If its relative molecular mass is 168, what is its molecular formula?
[At. Wt. C = 12, H = 1, Cl = 35.5]
A compound has the following percentage composition by mass: carbon 14.4%, hydrogen 1.2% and chlorine 84.5%. By what type of reaction could this compound be obtained from ethylene?
