Question
S. No
Column I
Column II
1.
$Cl_2O$
+7
2.
$Cl_2O_7$
+4
3.
$ClO_2$
+1
4.
$Cl_2O_6$
+6

Answer

S. No
Column I
Column II
1.
$Cl_2O$
+1
2.
$Cl_2O_7$
+7
3.
$ClO_2$
+4
4.
$Cl_2O_6$
+6

Need a full question paper?

Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.

Start Generating Free

Similar questions

Define following.
(i) Molarity
(ii) Molality
(iii) Normality
(iv) Formality
For any gaseous reaction how will you write the equilibrium constant $\left( K _{ p }\right)$ ? What is the relationship between $K_p$ and $K_{ c }$ ? Derive it.
  1. Arrange the following according to given property
$\text{CH}_3\stackrel{\oplus \ \ \ }{\text{CH}}_2,\text{C}_6\text{H}_5-\stackrel{\oplus\ \ \ \ }{\text{CH}}_2,(\text{CH}_3)_3\stackrel{\oplus \ \ \ \ }{\text{CH}},$
$\text{CH}_2=\text{CH}-\stackrel{\oplus\ \ \ \ }{\text{CH}}_2$ (decreasing order of stability)
  1. $\text{HC}\equiv\text{C}^{\ominus},\text{Ch}_2=\stackrel{\ominus\ \ \ \ \ \ }{\text{CH}_2},\text{CH}_3-\stackrel{\ominus\ \ \ \ \ }{\text{CH}_2},\stackrel{\ominus \ \ \ \ \ }{\text{CH}_3}$ (increasing order of stabillity)
  2. $\text{C}_6\text{H}_5\stackrel{\bf. \ \ \ \ }{\text{CHCH}_3},\text{C}_6\text{H}_5\text{CH}_2\stackrel{\bf.\ \ \ \ \ }{\text{CH}_2},\text{C}_6\text{H}_5\stackrel{\bf.}{\text{C}}_3(\text{CH}_3)_2$ (increasing order of stabillity)
  3. $\text{CH}_3-\stackrel{\oplus \ \ \ \ }{\text{CH}}-\text{O}-\text{CH}_3,\text{CH}_3-\stackrel{\oplus \ \ \ \ }{\text{CH}},-\text{OCH}_3,$
${\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{O}}\\{\ \ \ \ \ \ \ \\ \ \ \ \ \ \ \ \ \ \ \ \ \ \\ \|}\\\ \text{CH}_3-\stackrel{\oplus \ \ \ \ }{\text{CH}}\text{C}-\text{OCH}_3$ (decreasing order of stability)
  1.  
Balance the following equations in basic medium by ion-electron method and oxidation number methods and identify the oxidising agent and the reducing agent.$\text{P}_4(\text{s})+\text{OH}^{-}(\text{aq})\rightarrow\text{PH}_3(\text{g})+\text{HPO}_2^-(\text{aq})$
Discuss the principle and method of softening of hard water by synthetic ionexchange resins.
  1. For the reaction:
$\text{N}_2(\text{g})+3\text{H}_2(\text{g})\rightleftharpoons2\text{NH}_3(\text{g}),$
The value of $K_p$ is $3.6 \times 10^{-2}$ at $500K$.
Colculate the value of $K_c$ for the reaction at the same temperature R = 0.083L bar $K^{-1}mol^{-1}$​​​​​​​.
  1. What is the effect of increasing pressure in the reactions? Give reason.
$\text{PCl}_5(\text{g})\rightleftharpoons\text{PCl}_3(\text{g})+\text{Cl}_2\text{(g)}$
$\text{N}_2(\text{g})+\text{O}_2(\text{g})\rightleftharpoons2\text{NO(g)}$
  1. Predict the acidic, basic or neutral nature of the following salts:
$NaCN, KBr, NaNO_2, NH_4NO_3$
  1. What is the minimum volume of water required to dissolve 1 g of calcium sulphate at 298K? (For calcium sulphate $K_{sp} is 9.1 \times 10^{-6}$).
  2. At $450K ; K_p = 2.0 \times 10^{10}bar^{-1}$ for the reaction at equilibrium:
​​​​​​​​​​​​​​$2\text{SO}_2(\text{g})+\text{O}_2(\text{g})\rightleftharpoons2\text{SO}_3(\text{g})$
What is $K_c$ at this temperature?
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 $27^{\circ} \mathrm{C}$ ?
Write a note on entropy and spontaneity.
At $450K, K_p= 2.0 \times 10^{10}/bar$ for the given reaction at equilibrium.
$2\text{SO}_2\text{(g) + O}_2\text{(g)}\rightleftharpoons\text{2SO}_3\text{(g)}$
What is $K_c$ at this temperature?