Chemistry Question Bank

Assertion : If 30 mL of H2 and 20 mL of O2 react to form  water,  5  mL  of  H2  is  left  at  the  end  of  the reaction Reason :H2 is the limiting reagent.

Assertion :Number of molecules present in SO2 is twice the number of molecules present in O2. Reason : Molecular mass of SO2 is double to that of O2.

Assertion :Both  12g  of  carbon  and  27g  of aluminium contain 6.023 × 1023 atoms. Reason :Molar  mass  of  an  element  contains Avogadro number of atoms.

Assertion :  Both  138  g  of  K2CO3  and  12  g  of carbon have same number of carbon atoms. Reason :  Both  contains  1  g atom of  carbon  which contains 6.022 × 1023 carbon atoms.

Assertion :Pure water obtained from different states of India always contains hydrogen and oxygen in the ratio of 1 : 8 by mass. Reason: Total mass of reactants and products during chemical change is always the same.

5 mL of N-HCl, 20 mL of N/2 H2SO4 milli equivalent and 30 mL of N/3 HNO3 are mixed together and the volume is made to 1L. The normality of the resulting solution is

N2 + 3H2-> 2NH3 Molecular  weight  of  NH3  and  N2  are  x1  and  x2, respectively. Their equivalent weights are y1 and y2, respectively. Then (y1 – y2) is (a) 2x x

Given the reaction : Na O(s) H O( ) 2NaOH(aq) -> l What is the molarity of the solution formed if 1.35g of  Na2O  is  mixed  with  H2O  such  that  the  final volume is 100 mL?

A  solution  containing  12.0%  NaOH  by  mass  has  a density of 1.131 g/mL. What volume of this solution contains 5.00 mol of NaOH ?

A solution of NaOH is prepared by dissolving 4.0 g of  NaOH in 1  L of water. Calculate the volume of the HCl gas at STP that will neutralize 50 mL of this solution.

1 mole of oxalic acid is treated with conc. H2SO4. The  resultant  gaseous  mixture  is  passed  through  a solution of KOH. The mass of KOH consumed will be (where KOH absorbs CO2.) (COOH)2 CO + CO2 + H2O 2 KOH + CO2…

In a compound C, H and N atoms are present as 9%, 1%, 3.5% respectively. Molecular weight of compound is 108. Molecular formula of compound is (a) C H N (b) C H N (c) C H N (d) C H N

O Thus, 1.0 g Mg reactis with 0.67 . g O But only 0.56g O is available which less than 0.67 g is. Thus, O . is the limiting reagent. MOLE & EQUIVALENT CONCEPT Further, 16g O reacts with 24g of Mg. 0.56g O will re…

1.0 g of magnesium is burnt with 0.56 g O2 in a closed vessel. Which reactant is left in excess and how much? (At. wt. Mg = 24, O = 16) (NEET 2014)

When 22.4 litres of H2(g) is mixed with 11.2 litres of Cl2(g), each at STP, the moles of HCl(g) formed is equal to (NEET 2014)

Equal masses of H2, O2 and methane have been taken in a container of volume V at temperature 27°C in identical conditions. The ratio of the volumes of gases H2 : O2 : methane would be (NEET 2014)

6.02 × 1020 molecules of urea are present in 100 mL of its solution. The concentration of solution is (NEET 2013)

The vapour density of a gas is 11.2. The volume occupied by one gram of the gas at STP is (Manipal – 2013)

20.0 kg of N2(g) and 3.0 kg of H2(g) are mixed to produce NH3 (g). The amount of NH3(g) formed is (Kerala CEE 2011)

60g of a compound on analysis produced 24g of carbon, 4g hydrogen and 32g oxygen. The empirical formula of the compound is. (BVP 2010)

The number of atoms in 0.1 mol of a triatomic gas is ( A N =6.022×10 ) (CBSE AIPMT 2010)

To dissolve 0.9 g metal, 100 mL of 1N HCl is used. What is the equivalent weight of metal? (MP PMT 2010)

In an experiment, 4 g of M2Ox oxide was reduced to 2.8 g of the metal. If the atomic mass of the metal is 56 g mol–1, the number of O atoms in the oxide is (AFMC 2010)

10 g of hydrogen and 64 g of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be (AIPMT 2009)

The volume of 2 N H2SO4 solution is 0.1 dm3. The volume of its decinormal solution (in dm3) will be (MHT CET 2009)