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1 g of magnesium is burnt with 0.56g of oxygen in a closed vessel. The left-out reactant and its quantity are
(At. weight of Mg = 24, O=16)

When 22.4L of H₂(g) is mixed with 11.2L of Cl₂(g) each at STP, the moles of HCl(g) formed is equal to 
1. 1 mole of HCl(g)
2. 2 moles of HCl(g)
3. 0.5 mole of HCl(g)
4. 1.5 moles of  HCl(g)

In the Haber process, 30 L of dihydrogen and 30 L of dinitrogen were taken for the reaction, which yielded only 50% of the expected product. The composition of the gaseous mixture under the said conditions at the end is: 
1. 20 L ammonia, 10 L nitrogen, 30 L hydrogen
2. 10 L ammonia, 25 L nitrogen, 15 L hydrogen
3. 20 L ammonia, 20 L nitrogen, 20 L hydrogen
4. 20 L ammonia, 25 L nitrogen, 15 L hydrogen

The hydrated salt, Na₂SO₄.nH₂O, undergoes a 55% loss in mass on heating and becomes anhydrous. The value of n will be:

When 100 mL of PH₃ is decomposed, it produces phosphorus and hydrogen. The change in volume is:

If 0.5 moles of BaCl₂ is reacted with 0.2 moles of Na₃PO₄ then the maximum moles of Ba₃(PO₄)₂ formed is:

On reduction with CO, 200 kg of iron ore (Fe₂O₃) containing 20% impurities gives iron. The amount of iron produced will be-
1. 84 kg
2. 200 kg
3. 56 kg
4. 112 kg

KClO₃ on heating decomposes to KCl and O₂. The volume of O₂ at STP liberated by 0.1 mole KClO₃ is
1. 4.36 L
2. 3.36 L
3. 2.36 L
4. None of these

A sample of pure compound is found to have Na = 0.0887 mole, O = 0.132 mole, C = 2.65 × 10²² atoms.
The empirical formula of the compound is :
1. Na₂CO₃
2. Na₃O₂C₅
3. ${\mathrm{Na}}_{0.0887}{0}_{0.132}{\mathrm{C}}_{2.65\times {10}^{22}}$
4. NaCO

An organic substance containing C, H, and O gave the following percentage composition :
C = 40.687%, H = 5.085% and O = 54.228%. The vapour density of this organic substance is 59.
The molecular formula of the compound will be:
1. C₄H₆O₄
2. C₄H₆O₂
3. C₄H₄O₂
4. None of the above

At standard temperature and pressure (STP), the volume of oxygen required to completely combust 30 ml of acetylene under similar conditions is:
1. 100 ml
2. 75 ml
3. 50 ml
4. 25 ml

A stoichiometric reaction is initiated by filling a sealed steel vessel with 10 g of hydrogen gas and 64 g of oxygen gas, followed by an ignition to trigger an explosion. Determine the total number of moles of water (\(\text{H}_2\text{O}\)) produced by this combustion reaction once the limiting reactant is completely consumed:
1. 2 moles
2. 3 moles
3. 4 moles
4. 1 mole

A 6.85 g sample of the hydrates $\mathrm{Sr}{\left(\mathrm{OH}\right)}_2.{\mathrm{xH}}_2\mathrm{O}$ is dried in an oven to give 3.13 g of anhydrous $\mathrm{Sr}{\left(\mathrm{OH}\right)}_2$. The value of x is - 
(Atomic weights : Sr=87.60, O=16.0, H=1.0)
1.  8
2.  12
3.  10
4.  6

Sulphur burns according to the reaction
 $\frac{1}{8}{\mathrm{S}}_8\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)$ $\stackrel{}{\to }$ ${\mathrm{SO}}_2\left(\mathrm{g}\right)$
What volume of air, at 1 atm and 273 K, containing 21%  oxygen by volume is required to completely burn sulphur $\left({\mathrm{S}}_8\right)$ present in 200 g of the sample?
(This sample contains 20% inert material which does not burn)
1.  23.52 litre
2.  320 litre
3.  112 litre
4.  533.33 litre

The volume of oxygen gas (O₂) needed to completely burn 1 L of propane gas (C₃H₈)  (both O₂ & propane measured at 0°C and 1 atm) will be:
1. 7 L
2. 6 L
3. 5 L
4. 10 L

An organic compound contains carbon, hydrogen, and oxygen. If elemental analysis reveals 38.71% carbon and 9.67% hydrogen, which of the following is its empirical formula?

What is the number of moles of PbCl₂ formed when 6.5 g of PbO reacts with 3.2 g of HCl?
1. 0.044
2. 0.333
3. 0.011
4. 0.029

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. ${\mathrm{V}}_2{\mathrm{O}}_3$
2. $\mathrm{VO}$
3. ${\mathrm{V}}_2{\mathrm{O}}_5$
4. ${\mathrm{V}}_2{\mathrm{O}}_7$

1.44 gram of titanium (At. wt. =48) reacted with excess of ${\mathrm{O}}_2$ and produce x gram of non-stoichiometric compound Ti_1.44 O$$. The value of x is:
1. 2
2. 1.77
3. 1.44
4. None of the above

When 7.3 g of magnesium bicarbonate (Mg(HCO₃)₂) is decomposed by heating, how much carbon dioxide gas (in mL) is released at STP?
1. 1000 mL
2. 1120 mL
3. 2230 mL
4. 3240 mL