Empirical & Molecular Formula

Q. 11.2 litre of a gas at STP weighs 14 g. The gas could not be

1. 
2. 
3. 
4. 

Q. 0.242 g sample of K is heated in the presence of oxygen gas. This resulted in the formation of 0.440 g of a crystalline compound. What is the formula of this compound?

1. 
2. 
3. 
4. 

Q.

1.615 g of anhydrous $ZnS{O}_4$ was places in moist air. After a few days, its mass was found to be 2.875g. The molecular formula for hydrated zinc sulphate is

1. 
2. 
3. 
4. 

Q. The number of moles of carbon dioxide which contain 8 g of oxygen is

1. 0.5 mol
2. 0.40 mol
3. 0.25 mol
4. 0.20 mol

Q.

The simplest formula of a compound containing $50\%$ of element X (atomic mass 10) and $50\%$ of element Y (atomic mass 20) is

1. $X_{2}Y$
2. $X{Y}_3$
3. $X_2{Y}_3$
4. $XY$

Q.

A hydrocarbon contains $86\%$ carbon, 488ml of the hydrocarbon weight 1.68 g at STP. Then the hydrocarbon is an

1. Alkane
2. Alkene
3. Arene
4. Alkyne

Q.

One litre of a gas at STP weight 1.16 g it can possible be

1. $CO$
2. $O_2$
3. $C{H}_4$
4. $C_2{H}_2$

Q.

Two oxides of a metal contain $27.6\%and30.0\%$ of Oxygen, respectively. If the formula of the first be $M_3$$O_4$. Find that of the second.

1. 

2. 

3. O

4. 

Q.

The ratio of the mass of C-12 atom to that of an atom of element $X$ (whose atomicity is four) is 1 : 9. Themolecular mass of element $X$ is

1. 

2. 

3. 

4. 

Q. Butyric acid is an organic compound containing only C, H and O and is a component of rancid butter. If 0.44 g of butyric acid is burnt in excess oxygen, it yields 0.88 g of $C{O}_2$ and 0.36 g of water as the only products. The empirical formula of butyric acid is:

1. $CH{O}_4$
2. $CHO$
3. $C_2{H}_{4}O$
4. $C{H}_{4}O$