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Syllabus

Iron Pyrite --(A)--> Colourless Acidic Gas --(B)--> SO3 --(C)--> oleum --(D)--> Sulphuric acid

Question:9

MnO

_{2}+ 4HCl $\to $ MnCl_{2}+ 2H_{2}O + Cl_{2}1.746g of pure MnO

_{2}is heated strongly with conc. HCl. Calculate:a) Moles of MnO

_{2}used.b) Mass of salt formed.

c) Moles of chlorine gas formed.

d) Volume of chlorine gas formed at STP.

e) Mass of acid required.

Solve this :15. Indium (atomic weight = 114.82) has two naturally occurring isotopes, the predominant one form has isotopic weight 114.9041 and abundance of 95.72%. Which of the following isotopic weights is the most likely for the other isotope?

(A) 112.94

(B) 115.90

(C) 113.90

(D) 114.90

dioxide gas and steam. If all measurements are made at constant pressure and 100 0C,find

the composition of the resulting mixture. The equation for the reaction is:

C2H4(g) + 3O2(g) ? 2CO2(g) + 2H2O(g)

Q. The number of

i) molecules [S = 32]

ii) atoms in 192 g. of sulphur. [${S}_{8}$]

24. Solid ammonium dichromate decomposes as under:

${\left(N{H}_{4}\right)}_{2}C{r}_{2}{O}_{7}\to {N}_{2}+C{r}_{2}{O}_{3}+4{H}_{2}O$

If 63 g of ammonium dichromate decomposes. Calculate:

$\left(a\right)thequantityinmolesof{\left(N{H}_{4}\right)}_{2}C{r}_{2}{O}_{7}\phantom{\rule{0ex}{0ex}}\left(b\right)thequantityinmolesofnitrogenformed\phantom{\rule{0ex}{0ex}}\left(c\right)thevolumeof{N}_{2}evolvedatSTP.\phantom{\rule{0ex}{0ex}}\left(d\right)whatwillbethelossofmass?\phantom{\rule{0ex}{0ex}}\left(e\right)calculatethemassofchromium\left(III\right)oxideformedatthesametime.$

1) Avagadro's Law.

2) Gay Lussac's Law.

3) Boyle's Law.

4) Charle's Law.

_{3}is dissolved in water and treated with excess of silver nitrate solution. 1.43g of precipitate is produced. Calculate the percentage of NaCl in the mixture. Given Ag = 108, Na = 23, N = 14, O =16, Cl = 35.5.Qb) i) Calculate the mass of residue obtained by heating 2.7 g. Ag

_{2}CO_{1}? [ Ag = l08 C= 12 O = 16]ii) How many moles of water are in 720 g of it ?

iii) Calculate the number of atoms in 8 g of helium gas at STP.

iv) KCIO

_{3}on heating decomposes to give KCl and oxygen. What is the volume of O_{2}at stp liberated by 0.1 mole of KClO_{3}.Q. (i) If 150 cc of gas A contains X molecules, how many molecules of gas B

will be in 75 cc of B? The gases A and B are under the same conditions of temperature and

pressure.

(ii) Name the law on which the problem is based.

Q. Aluminium carbide reacts with Water according to the following equation:

$A{l}_{4}{C}_{3}+12{H}_{2}O\to 4Al{\left(OH\right)}_{3}+3C{H}_{4}$

(i) What mass Of aluminium hydroxide is formed from 12g Of aluminium

carbide?

(ii) What volume of methane at s.t.p. is obtained from 12g of aluminium carbide?

[Relative molecular weight of $A{l}_{4}{C}_{3}=144;Al{\left(OH\right)}_{3}=78$]

Please can you help me.

Q. Calculate the percentage of carbon in a 55% pure sample of carbon carbonate.

24. Solid ammonium dichromate decomposes as under:

${\left({\mathrm{NH}}_{4}\right)}_{2}{\mathrm{Cr}}_{2}{\mathrm{O}}_{7}\to {\mathrm{N}}_{2}+{\mathrm{Cr}}_{2}{\mathrm{O}}_{3}+4{\mathrm{H}}_{2}\mathrm{O}$

If 63 g of ammonium dichromate decomposes, calculate:

(a) The quantity in moles of (NH

_{4})_{2}Cr_{2}O_{7}(b) The quantity in moles of nitrogen formed

(c) The volume of N

_{2}evolved at STP.(d) The loss of mass

a] the number of moles of SO2 liberated by 776g of ZnS and,

b] the weight of ZnS required to produce 22.4 lits of SO2 at s.t.p. (S=32, Zn=65,O=16)

_{4}) was mixed with 106 cc oxygen and then exploded. On cooling, the volume of the mixture became 82 cc, of which 58 cc was unchanged oxygen. Which law does this experiment support? Explain with calculations.Q.(i) A gas of mass 32 gms has a volume of 20 litres at S.T.P. Calculate the gram molecular weight of the gas.

(ii) How much Calcium oxide is formed when 82 g of calcium nitrate is heated? Also find the volume of nitrogendioxide evolved:

$2Ca(N{O}_{3}{)}_{2}\to 2CaO+4N{O}_{2}+{O}_{2}$

(Ca = 40, N = 14, O = 16)

(Zn=65 ,C=12 ,O=16)

Calculate the empirical formu;a of the salt. [Na = 23, S = 32, O = 16].

c) 4.92g of hydrated magnesium sulphate $(MgS{O}_{4}.x{H}_{2}O)$ on strong heating leaves 2.40g of anhydrous magnesium sulphate. Calculate the value of x in $MgS{O}_{4}.x{H}_{2}O.[Mg=24,S=32,O=16,H=1]$

Solve this :$\mathrm{c})\mathrm{A}\mathrm{compound}\mathrm{has}\mathrm{the}\mathrm{following}\mathrm{percentage}\mathrm{composition}:\phantom{\rule{0ex}{0ex}}\mathrm{Na}=18.60\%,\mathrm{S}=25.80\%,\mathrm{H}=4.03\%,\mathrm{O}=51.58\%.\phantom{\rule{0ex}{0ex}}\mathrm{The}\mathrm{molecular}\mathrm{weight}\mathrm{of}\mathrm{the}\mathrm{compound}\mathrm{is}248.\mathrm{Calculate}\mathrm{the}\mathrm{molecular}\mathrm{formula}\mathrm{of}\mathrm{the}\mathrm{crystalline}\mathrm{salt},\mathrm{assuming}\mathrm{all}\mathrm{hydrogen}\mathrm{to}\mathrm{be}\mathrm{present}\mathrm{as}\mathrm{water}\mathrm{of}\mathrm{crysallisatio}\phantom{\rule{0ex}{0ex}}[\mathrm{Na}=23,\mathrm{S}=32,\mathrm{O}=16,\mathrm{H}=1]$