JEE Mole Concept PYQs with Solutions PDF, Download Now

By usual analysis, 1.00 g of compow1d (X) gave 1.79 g of magnesium pyrophosphate. The percentage of phosphorus in compound (X) is: (nearest integer)
(Given, molar mass in $$gmol^{-1}$$ : 0 = 16, Mg = 24, P = 31 )

Given below are four compounds :
(a) n-propyl choride
(b) iso-propyl chloride
(c) sec-butyl chloride
(d) neo-pentyl chloride
Percentage of carbon in the one which exhibits optical isomerism is:

$$A + 2B \rightarrow AB_{2}$$
36.0 g of ' A' (Molar mass : 60 g $$mol^{-1}$$) and 56.0 g of 'B' (Molar mass: 80 g $$mol^{-1}$$) are allowed to react. Which of the following statements are correct?
A. 'A' is the limiting reagent.
B. 77.0 g of $$AB_{2}$$ is formed.
C. Molar mass of $$AB_{2} is 140 g $$mol^{-1}$$
D. 15.0 g of A is left unreacted after the completion of reaction.
Choose the correct answer from the options given below :

Aqueous HCI reacts with $$MnO_{2} \left(s\right)$$ to form $$MnCl_{2}\left(aq\right)$$, $$Cl_{2}\left(g\right)$$ and $$H_{2}O\left(l\right)$$. What is the weight (in g) of Cl_{2} liberated when 8.7 g of $$MnO_{2} \left(s\right)$$ is reacted with excess aqueous HCI solution ?
(Given Molar mass in g $$mol^{-1}$$ Mn = 55, Cl = 35.5, 0 = 16, H = l )

x mg of pure HCl was used to make an aqueous solution. 25.0 mL of 0.1 M $$Ba(OH)_{2}$$ solution is used when the HCl solution was titrated against it. The numerical value of x is ______$$\times 10^{-1}$$. (nearest integer)
Given : Molar mass of HCl and $$Ba(OH)_{2}$$ are 36.5 and 171.0 g $$mol^{-1}$$ respectively.

0.01 mole of an organic compound (X) containing 10% hydrogen, on complete combustion produced $$0.9_{g}H_{2}O$$. Molar mass of (X) is_____$$mol^{-1}$$.

When 81.0 g of aluminium is allowed to react with 128.0 g of oxygen gas, the mass of aluminium oxide produced in grams is_______ - (Nearest integer) Given : Molar mass of Al is 27.0 g $$mol^{-1}$$ Molar mass of O is 16.0 g $$mol^{-1}$$.

The observed and normal molar masses of compound  $$MX_2$$ are  $$65.6$$  and  $$164$$  respectively. The percent degree of ionisation of  $$MX_2$$  is  $$\underline{\hspace{2cm}}\%.$$  (Nearest integer)

The number of moles of methane required to produce $$11$$ g $$CO_2(g)$$ after complete combustion is : (Given molar mass of methane in $$g mol^{-1} : 16$$)

5 g of NaOH was dissolved in deionized water to prepare a 450 mL stock solution. What volume (in mL) of this solution would be required to prepare 500 mL of 0.1 M solution? Given : Molar Mass of Na, O and H is 23, 16 and 1 g mol$$^{-1}$$ respectively

Combustion of glucose $$(C_6H_{12}O_6)$$ produces $$CO_2$$ and water. The amount of oxygen (in g) required for the complete combustion of $$900 \text{ g}$$ of glucose is : [Molar mass of glucose in $$\text{gmol}^{-1} = 180$$]

A sample of CaCO$$_3$$ and MgCO$$_3$$ weighed 2.21 g is ignited to constant weight of 1.152 g. The composition of the mixture is: (Given molar mass in g mol$$^{-1}$$, CaCO$$_3$$: 100, MgCO$$_3$$: 84)

Consider the following reaction: $$3PbCl_2 + 2(NH_4)_3PO_4 \rightarrow Pb_3(PO_4)_2 + 6NH_4Cl$$. If $$72$$ mmol $$PbCl_2$$ is mixed with $$50$$ mmol of $$(NH_4)_3PO_4$$, then amount of $$Pb_3(PO_4)_2$$ formed in mmol is (nearest integer):

$$2.8 \times 10^{-3}$$ mol of $$CO_{2}$$ is left after removing $$10^{21}$$ molecules from its 'x' mg sample. The mass of $$CO_{2}$$ taken initially is Given: $$N_{A} = 6.02 \times 10^{23} mol^{-1}$$

The elemental composition of a compound is  $$54.2\%C,\ 9.2\%H$$  and  $$36.6\%O.$$ If the molar mass of the compound is  $$132\ \text{g mol}^{-1},$$ the molecular formula of the compound is: [Given: Relative atomic masses  C:H:O = 12:1:16]