Question
✓
Answer
(13)
Sol.
0.1 mole of compound ( S ) weight in gm
$=0.1 \times$ molar mass of compound $(\mathrm{S})$
$=0.1 \times 130=13 \mathrm{gm}$
Sol.
0.1 mole of compound ( S ) weight in gm
$=0.1 \times$ molar mass of compound $(\mathrm{S})$
$=0.1 \times 130=13 \mathrm{gm}$
Need a full question paper?
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.
Explore more
Similar questions
A first order reaction requires $30$ minutes for $50\%$ completion. The time required to complete the reaction by $75\%$ will be .......... $\min.$
→In the following reaction, which choice has value twice that of the equivalent mass of the oxidising agent
Uracil is base present in $RNA$ with the following structure. $\%$ of $N$ in uracil is $............$.
→Given :
Molar mass $N =14\,g\,mol ^{-1} ; O =16\,g\,mol ^{-1} ; C =12\,g\,mol ^{-1} ; H =1\,g\,mol ^{-1}$;
A current being passed for two hour through a solution of an acid liberating $11.2$ litre of oxygen at $NTP $ at anode. What will be the amount of copper deposited at the cathode by the same current when passed through a solution of copper sulphate for the same time ........... $\mathrm{g}$
→How much faster would a reaction proceed at $25\,^oC$ than at $0\,^oC$ if the activation energy is $65\,kJ$ ....... times
→The rate for a first order reaction is $0.6932 \times {10^{ - 2}}\,mol\,{l^{ - 1}}\,mi{n^{ - 1}}$ and the initial concentration of the reactants is $1\,M$, ${T_{1/2}}$ is equal to ........ $\min$
→Consider the cell at $25^{\circ} \mathrm{C}$
→$\mathrm{Zn}\left|\mathrm{Zn}^{2+}(\mathrm{aq}),(1 \mathrm{M}) \| \mathrm{Fe}^{3+}(\mathrm{aq}), \mathrm{Fe}^{2+}(\mathrm{aq})\right| \mathrm{Pt}(\mathrm{s})$
The fraction of total iron present as $\mathrm{Fe}^{3+}$ ion at the cell potential of $1.500\, \mathrm{~V}$ is $\mathrm{X} \times 10^{-2}$. The value of $x$ is $.....$ (Nearest integer).
$\left(\right.$ Given $\left.E_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{0}=0.77\, \mathrm{~V}, \mathrm{E}_{\mathrm{Zn}^{2+} / \mathrm{Zn}}^{0}=-0.76 \,\mathrm{~V}\right)$
For the reaction
→$C _{2} H _{6} \rightarrow C _{2} H _{4}+ H _{2}$
the reaction enthalpy $\Delta_{ r } H =...........{ kJ\, mol ^{-1}}$.
(Round off to the Nearest Integer).
[Given : Bond enthalpies in $kJ$ $mol$ $^{-1}:C-C : 347, C = C : 611 ; C - H : 414, H - H : 436]$
The $pH$ value of $0.1\,\,M\,\,NaOH$ solution is (when there is a given reaction $[{H^ + }]\,[O{H^ - }] = {10^{ - 15}}$)
→If $HN{O_3}$ changes into ${N_2}O$, the oxidation number is changed by
→