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%
For the reaction;
\(2Fe{(NO_3)}_3 + 3Na_2CO_3 \rightarrow Fe_2{(CO3)}_3 + 6NaNO_3\)
Initially if 2.5 mole of \(Fe{(NO_3)}_3 \) and 3.6 mole of \(Na_2CO_3\) is taken. If 6.3 mole of \(NaNO_3\) is obtained then % yield of given reaction is:
1. 50
2. 84
3. 87.5
4. 100
0.8 mole of a mixture of CO and CO2 requires exactly 40 gram of NaOH in a solution for complete conversion of all the CO2 into Na2CO3. How many moles more of NaOH would it require for conversion into Na2CO3, if mixture (0.8 mole) is completely oxidised to CO2?
1. 0.2
2. 0.6
3. 1
4. 1.5
The impure 6 g of is dissolved in water and then treated with excess of silver nitrate solution. The weight of precipitate of silver chloride is found to be 14 g. The % purity of solution would be:
1. 95%
2. 85%
3. 75%
4. 65%
25.4 g of and 14.2 g of are made to react completely to yield a mixture of ICI and ICI3. The mole of ICI and ICI3 formed, is respectively -
1. 0.5, 0.2
2. 0.1, 0.1
3. 0.1, 0.3
4. 0.3, 0.4
The vapour density of a mixture containing and is 38.3. The mole of in a 100 g mixture is:
[Vapour density = (Molar mass / 2)]
1. 0.437
2. 0.347
3. 0.557
4. 0.663
Copper forms two oxides. For the same amount of copper, twice as much oxygen was used to form first oxide than to form second one. What is the ratio of the valencies of copper in first and second oxides?
1. 2:5
2. 1:6
3. 2:1
4. 1:2
5 mL of a gaseous hydrocarbon was exposed to 30 mL of . The resultant gas, on cooling is found to measure 25 mL of which 10 mL is absorbed by NaOH and the remainder by pyrogallol. Determine molecular formula of hydrocarbon. All measurements are made at constant room temperature.
1. CH4
2. C2H2
3. C3H4
4.C2H4
60 mL of a mixture of nitrous oxide and nitric oxide was exploded with excess of hydrogen. If 38 mL of was formed, calculate the volume of each gas in the mixture. All measurements are made at constant P and T.
1.20 ml +30 ml
2. 44 ml + 16 ml
3. 10 ml+40 ml
4 .25 ml +25 ml
2.0 g sample containing and loses 0.248 g when heated to 300C, the temperature at which decomposes to , and . What is the % of in mixture?
1.66.5
2.50.6
3.60.5
4.6.65