Question
Write the applications of electronegativity
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Answer
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Draw the cis and trans structures of hex-2-ene. Which isomer will have higher b.p. and why?
1. Why is nitric acid added to sodium extract before adding silver nitrate for testing halogens?
2. How does
i. an electron withdrawing group (EWG) and
ii. an electron donating group (EDG) influence the acid strength of carboxylic end?
2. How does
i. an electron withdrawing group (EWG) and
ii. an electron donating group (EDG) influence the acid strength of carboxylic end?
What will be the pressure of the gaseous mixture when 0.5 L of $\mathrm{H}_2$ at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1 L vessel at $27^{\circ} \mathrm{C}$ ?
→In terms of period and group where would you locate the element with $Z=114$?
→Calculate the enthalpy change on freezing of 1.0 mol of water at $10.0^{\circ} C$ to ice at $-10.0^{\circ} C$.
$\Delta_{\text {fus }} H=6.03 kJ mol^{-1} \text { at } 0^{\circ} C .$
$C_{p}\left[H_2 O(l)\right]=75.3 J mol^{-1} K^{-1}$
$C_{p}\left[H_2 O(s)\right]=36.8 J mol^{-1} K^{-1}$
→$\Delta_{\text {fus }} H=6.03 kJ mol^{-1} \text { at } 0^{\circ} C .$
$C_{p}\left[H_2 O(l)\right]=75.3 J mol^{-1} K^{-1}$
$C_{p}\left[H_2 O(s)\right]=36.8 J mol^{-1} K^{-1}$
One mole of $H_2O$ and one mole of CO are taken in 10L vessel and heated to 725K. At equilibrium 40% of water (by mass) reacts with CO according to the equation,
$\text{H}_2\text{O (g) + CO (g)}\rightleftharpoons\text{H}_2\text{ (g) + CO}_2\text{ (g)}$
Calculate the equilibrium constant for the reaction.
→$\text{H}_2\text{O (g) + CO (g)}\rightleftharpoons\text{H}_2\text{ (g) + CO}_2\text{ (g)}$
Calculate the equilibrium constant for the reaction.
Structures of molecules of two compounds are given below:
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Which of the two compounds will have intermolccular hydrogen bonding and which compound is expected to show intramolecular hydrogen bonding?
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The melting point of a compound depends on. among other things, the extent of hydrogen bonding. On this basis explain which of the above two compounds will show higher melting point.
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Solubility of compounds in water depends on power to form hydrogen bonds with water. Which of the above compounds will form hydrogen bond with water easily and be more soluble in it?
Suggest a list of the substances where carbon can exhibit oxidation states from $-4$ to $+4$ and nitrogen from $-3$ to $+5$.
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$\text{A}(\text{s})\rightleftharpoons2\text{B}(\text{g})+3\text{C}(\text{g})$
It conc. of 'C' is increased by factor of 2, what will be the equilibrium concentration of 'B' with respect to its original value.
→$\text{A}(\text{s})\rightleftharpoons2\text{B}(\text{g})+3\text{C}(\text{g})$
It conc. of 'C' is increased by factor of 2, what will be the equilibrium concentration of 'B' with respect to its original value.