List of top Questions asked in MHT CET

The solubility of \(\text{N}_{2}\) gas in water at \(25^{\circ }C\) and \(1\) bar is \(6.85\times 10^{-4}\) \(\text{mol L}^{-1}\). Calculate the molarity of \(\text{N}_{2}\) gas dissolved in water under atmospheric conditions when the partial pressure of \(\text{N}_{2}\) in atmosphere is \(0.50\) bar.
Calculate the boiling point elevation of an aqueous solution containing \(0.5\) g glucose in \(20\) g water if \(K_{b}\) for water is \(0.52\) \(\text{K kg mol}^{-1}\). [Molar mass of glucose \(=180\) \(\text{g mol}^{-1}\)]
Calculate van't Hoff factor for \(\text{CaCl}_{2}\), if osmotic pressure of \(\text{CaCl}_{2}\) and urea solutions of same concentrations at same temperature are \(0.65\) and \(0.27\) atm respectively.
The main function of a salt bridge in an electrochemical cell is to:
If a galvanized iron sheet is scratched and the iron surface is exposed to the atmosphere, the iron does not undergo corrosion. This is because:
A conductivity cell containing \(0.01\) M KCl produces resistance \(600\) ohms at \(25^{\circ }C\). Find the cell constant if conductivity of \(0.01\) M KCl at the same temperature is \(0.0014\) \(\text{ohm}^{-1}\text{cm}^{-1}\).
What is the total number of atoms present per fcc unit cell on all its faces only ?
Bottom ash of thermal power stations can be used as raw material for cement and brick industry. This example illustrates which of the following principle of green chemistry?
Calculate the molar mass of a metal having density \(10\) \(\text{g cm}^{-3}\) and fcc structure with edge length \(400\) pm.
Calculate the void volume of a unit cell of polonium metal if the radius of polonium is \(190\) pm.
What is IUPAC name of allylbromide ?
Assign the oxidation number of \(N\) in the following species respectively.
(i) \(\text{NH}_{4}^{+}\)     (ii) \(\text{NO}_{2}\)
Which one of the following nitrates will decompose to give \(\text{NO}_{2}\) on heating ?
What type of information is collected using FTIR spectroscopy ?
Identify the conjugate base of \(\text{NH}_{3}\) from following.
Calculate the solubility in g/L of sparingly soluble salt \(BA\) if solubility product is \(5.2\times 10^{-13}\) (molar mass \(BA=188\) g/mol).
Calculate the work done when \(2\) moles of an ideal gas expand isothermaly and reversibly from \(10\) \(\text{dm}^{3}\) to \(20\) \(\text{dm}^{3}\) at \(300\) K
\((R=8.314\text{JK}^{-1}\text{mol}^{-1})\)
The \(K_{SP}\) of \(\text{Mg(OH)}_{2}\) is \(1.2\times 10^{-11}\). Then what will be the highest pH of the \(0.1\) M \(\text{Mg}^{2+}\) ions from which \(\text{Mg(OH)}_{2}\) is not precipitated?
In a process, \(\Delta U=0\) and \(q\neq 0\). Then the process must involve
Which is the incorrect statement among the following?
Calculate the standard enthalpy of combustion of \(\text{C}_{2}\text{H}_{2}(g)\),
\(\text{C}_{2}\text{H}_{2}(g)+5/2\text{O}_{2}(g)\rightarrow 2\text{CO}_{2}(g)+\text{H}_{2}\text{O}(l)\)
\([\Delta _{f}H^{0}(\text{CO}_{2})=-390\) kJ \(\text{mol}^{-1}\), \(\Delta _{f}H^{0}(\text{H}_{2}\text{O})=-285\) kJ \(\text{mol}^{-1}\) and \(\Delta _{f}H^{0}(\text{C}_{2}\text{H}_{2})=225\) kJ \(\text{mol}^{-1}]\)
What is a correct set of four quantum number values for an electron present in \(3p\) orbital?
Which of the following terms is used for presence of H bonding in a molecule itself?
What is bond order in \(\text{N}_{2}\) molecule?
An AND gate is followed by a NOT gate in series. With two input \(A\) and \(B\), the Boolean expression for the output \(Y\) will be