If 2.74 g of the metal oxide contains 1.53 g of metal, then the empirical formula of vanadium oxide is:
(Atomic Mass of V = 52)
1.
2.
3.
4.
A gaseous mixture of propane and butane of volume 3 litre on complete combustion produces 11.0 litre under standard conditions of temperature and pressure. The ratio of volume of butane to propane is:
1. 1 : 2
2. 2 : 1
3. 3 : 2
4. 3 : 1
The percentage by volume of in a gaseous mixture of , and CO is 20. When 100 mL of the mixture is burnt in excess of , the volume of produced is
1. 90 mL
2. 160 mL
3. 140 mL
4. None of these
The percentage of oxygen present in the compound is-
1. 23.3%
2. 45.36%
3. 41.94%
4. 17.08%
0.607 g of a silver salt of tribasic organic acid was quantitatively reduced to 0.37 g of pure Ag. What is the mol. wt. of the acid?
1. 207 g
2. 210 g
3. 531 g
4. 324g
A gaseous compound is composed of 85.7% by mass carbon and 14.3% by mass hydrogen. It's density is 2.28 g/litre at 300 K and 1.0 atm pressure. Determine the molecular formula of the compound:
1.
2.
3.
4.
Calculate the % of free in oleum (a solution of in ) that is labelled 109% .
1. 40
2. 30
3. 50
4. None
100 mL of 10% NaOH (w/V) is added to 100 mL of 10% HCl (w/V). The resultant solution becomes:
1. Alkaline
2. Strongly alkaline
3. Acidic
4. Neutral
1.44 gram of titanium (At. wt. =48) reacted with excess of and produce x gram of non-stoichiometric compound The value of x is:
1. 2
2. 1.77
3. 1.44
4. None of the above
2.0 g sample contain mixture of and , on very strong heating leave a residue weighing 1.96 g. The reaction responsible for loss of weight is (unbalance equation)
What is the percentage by mass of in original sample?
1. 10%
2. 20%
3. 40%
4. 60%