Question Text
Question 1 :
Which of these is least likely to act as a Lewis base?
Question 2 :
The {tex}\mathrm{pH}{/tex} of aqueous solution of {tex} 1 \mathrm { M }\ \mathrm { HCOONH } _ { 4 } , \mathrm { pK } _ { \mathrm { a } } {/tex} of {tex} \mathrm { HCOOH } {/tex} is {tex}3.8{/tex} and {tex} \mathrm { pK } _ { \mathrm { b } } {/tex} of {tex} \mathrm { NH } _ { 3 } {/tex} is {tex}4.8{/tex}
Question 3 : In a reaction, <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7dbb1399925718ac6b2d1"> the concentrations of <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7dbb1ab3481716f4b7824"> and <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7db87399925718ac6b27f"> (in mol/L) are 0.5, 0.8, 0.4 and 1.0 respectively. The equilibrium constant is
Question 4 :
10 $lt$ box contain $O_3$ and $O_2$ at equilibrium at 2000 K. The $\Delta G^o = - 534.52\ kJ$ at 8 atm equilibrium pressure. The following equilibrium is present in the container,<br/>$2O_3(g)  \rightleftharpoons  3O_2 (g)$. The partial pressure of O$_3$ will be___________.   $ (ln 10 = 2.3, R = 8.3 J mole^{-1} K^{-1}$)
Question 7 : For the equilibrium,<br/>$LiCl\cdot { 3NH }_{ 3 }(s)\rightleftharpoons LiCl\cdot { NH }_{ 3 }(s)+2{ NH }_{ 3 }(g)\quad $ ${ K }_{ p }=9{ atm }^{ 2 }$ at ${ 37 }^{ o }C$. <div>A $5$ litre vessel contains $0.1$ mole of $LiCl\cdot { 3NH }_{ 3 }$. How many moles of ${ NH }_{ 3 }$ should be added to the flask at this temperature to derive the backward reaction for completion?<br/>$R=0.082 \ atm.L/molK$<br/></div>
Question 8 : ${ NH }_{ 4 }COO{ NH }_{ 2 }(s)\rightleftharpoons 2{ NH }_{ 3 }(g)+{ CO }_{ 2 }(g)$. <br/><div>If equilibrium pressure is $3$ atm for the given reaction, then ${K}_{p}$ will be:</div>
Question 9 :
$Fe_2O_3(s)$ may be converted be Fe by the reaction, $Fe_2O_3+3H_2(g)\rightleftharpoons 2Fe(s)+3H_2O(g)$; for which $K_p=8$ at temperature $720^0C.$ What % of $H_2$ remains unreacted after the reaction has come to equilibrium:
