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explain why cp is always greater than cv????

why oxygen is paramagnetic in nature by molecular orbital theory

what is physical equilibrium? Give two example

Equal volumes of two solutions pH=2 and pH=4 are mixed together.Calculate the pH of the resulting solution?

In a closed system:A

_{(s)}⇌2B_{(g)+}3C_{(g)}if the partial pressure of C is doubled then partial pressure of B will be??NO3- , NO2- NO2. and NO2+

K

_{sp}of Mg(OH)_{2 }is 4.0×10^{-12}.The number of moles of Mg^{2+}ions in one litre of its saturated solution in 0.1 M NaOH is??plz answer me soon and explain

the value of Kc = 4.24 at 800K for the reaction

CO(g) + H2O(g) CO2(g) + H2(g)

Calculate the equilibrium concentration of CO2 ,H2O ,CO , H2 at 800K ,if only CO and H2O are pesent initially at concentration of 0.10M each.

100 ml of 0.1 N NaOH is mixed with 100 ml of 0.1 N H

_{2}SO_{4}.The pH of the resultant solution is??When 0.1 mole of ammonia is dissolved in sufficient water to make 1 litre of solution.The solution is found to have a hydroxide ion concentration of 1.34×10

^{-3}.The dissociaton constant of ammonia is??What is the pH of 10

^{-8}M HCl solution?the equilibrium constant kp= 2.9*10^ -5 atm^3. the total pressure of gases at equilibrium when 1.0 mole of reactant was heated will be

_{p}) are related as ${\mathrm{K}}_{\mathrm{p}}=\frac{4{\mathrm{\alpha}}^{2}\mathrm{P}}{\left(1-{\mathrm{\alpha}}^{2}\right)}$?(1) ${\mathrm{N}}_{2}{\mathrm{O}}_{4}\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_{2}\left(\mathrm{g}\right)$

(2) ${\mathrm{H}}_{2}\left(\mathrm{g}\right)+{\mathrm{I}}_{2}\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{HI}\left(\mathrm{g}\right)$

(3) ${\mathrm{N}}_{2}\left(\mathrm{g}\right)+3{\mathrm{H}}_{2}\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_{3}\left(\mathrm{g}\right)$

(4) ${\mathrm{PCl}}_{3}\left(\mathrm{g}\right)+{\mathrm{Cl}}_{2}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{PCl}}_{5}\left(\mathrm{g}\right)$

At 90'C, pure water has [H30

^{+}]=10^{-6}mole/liter. the value of k_{W}at 90'C is:^{-6}^{-8}^{-12}^{-14}_{5}is 50% dissociated at an equilibrium pressure of 4 atm. At what pressure it would dissociate to the extent of 80% at the same temperature:-a) 0.05 atm

b) 0.60 atm

c) 0.75 atm

d) 2.50 atm

Kindly answer sir/mam.

Question -The pH of 0.1 M monobasic acid is 4.50. Calculate the concentration of H+, A- and HA. Also determine the values of ka and pka of mono basic acid.NH2COONH4----->2NH3(g)+CO2(g)

total pressure of the gas is 5 atm. hence Kp is

The pH of a solution obtained by mixing 100 ml of 0.2 M CH

_{3}COOH with 100 ml of 0.2 M NaOH will be??(given pK_{a}for CH_{3}COOH =4.74 and log 2=0.301)1)-57.1

2)-2*57.1

3)-3*57.1

_{4}(g) is attained by mixing equal moles of A and B in a one litre vessel. Then at equilibrium:- (Kindly explain the answer also)a) [A] = [B]

b) [A] > [B]

c) [A] < [B]

d) [AB

_{4}] > [A]Kindly answer sir/mam.

what is the formula and basicity of hydrated oxalic acid and anhydrous oxalic acid?

If the value of Kc is 3, the percentage by mass of iso-butanein the equilibriummixture would be:-

a) 75%

b) 90%

c) 30%

d) 60%

Kindly answer sir/mam.

Q] One mole of N

_{2}O_{4}(g) at 300K is kept in a closed container under one atmosphere. It is heated to 600K when 20% by mass of N_{2}O_{4}(g) decomposes to NO_{2}(g). The resultant pressure is??^{o}C, the dissociation constant of a base, BOH, is 1.0×10−12.1.0×10−12. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be ^{−6}mol L-1^{−5}mol L-1^{−6}mol L-1^{−7}mol L-12SO2 + O2 ------> 2SO3

has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the reaction at the same temperature

SO3 -----> SO2+ ½O2

49) Which oxychloride has maximum pH?

a) NaClO b) NaClO

_{2}c) NaClO_{3}d) NaClO_{4}88) A infinite dilution the percentage ionisation for both the strong and weak electrolyes is:

a) 1% b)20% c)50% d) 100%

At temperature T, a compound AB

_{2}(g) diassociates according to the reaction :2AB

_{2}(g) [reverisble sign ] 2AB(g) + B_{2}.with degree of dissociation, x, which is small compared to unity. Deduce the expression for x in terms of equillibrium constant K

_{p}and the total pressure.a)10

^{-3 }b)10^{-5}c)10

^{-7}d)10^{-9}The equilibrium constants K

_{P1}and K_{P2}for the reactions X↔2Y and Z↔P +Q, respectively are in the ratio of 1 : 9. If the degree of dissociation of X and Z be equal then the ratio of total pressure at these equilibria isPCl5(g) PCl3(g) + Cl2(g)

Vapour density is found to be 100 when 1 mole of PCl5 is taken in a 10 litre flask at 27* C.

Calculate the equilibrium pressure. Also calculate percentage dissociation of PCl5

the value of delta G for the phosphorylation of glucose in glycolysis is 13.8 kj/mol. Find the value of Kc at 298K?

The dissociation constant of a weak acid HA and weak base BOH are 2×10

^{-5}and 5×10^{-6 }respectively.The equilibrium constant for the neutralization reaction of the two is ( ignore hydrolysis of resulting salt)The solubility product constant of Ag

_{2}CrO_{4}and AgBr are 1.1 × 10^{–12}and 5.0 × 10^{–13}respectively. Calculate the ratio of the molarities of their saturated solutions.H2(g)+I2(g)2HI(g)

at 720K is 48. What is the value of the equilibrium constant for the reaction

1/2H2(g)+1/2I2(g)HI(g)

calculate simultaneous solubility of AgCNS and AgBr in a solution of water.Ksp AgCNS=1.2*10

^{-12},Ksp AgBr=5*10^{-13}What is an evacuated vessel? [From Comprehensive Chemistry Pg.-370]

_{3}COONH_{4}: K_{b}(NH_{3}) = 1.6 × 10^{–5}, K_{a}(CH_{3}COOH) = 1.6 × 10^{–5}.100 cc of N/10 NaOH solution is mixed with 100 cc of N/5 HCl solution and the whole volume is made to 1 litre.The pH of the resulting solution will be??

_{3}(s)_{}Fe^{3}^{+}(aq) + 3OH^{-}(aq), decreasing the concentration of OH^{-}ions 1/3 times will cause the equilibrium concentration of Fe^{3}^{+}to increase by:-a) 3 times

b) 9 times

c) 18 times

d) 27 times

Kindly answer sir/mam.

reached, concentration of C was thrice the equilibrium concentration of B. Calculate KC.

The solubility product of SrF

_{2}in water is 8 x 10^{-10}. Calculate its solubility in .01 M NaF aqueous solution.an excess of agno3 is added to 100 ml of a 0.01 M solution of [cr(h2o)4cl2]cl.the number of agcl precipated would be:

is this question based on common ion effect

plz explain me ostwald dilution law

_{SP} of Ag_{2}CrO_{4},AgCl ,AgBr and AgI are respectively , 1.1*10^{-12},1.8* 10^{-12}, 5*10^{-13},8.3*10^{-17}, which one of the following salts will precipitate last AgNO

_{3}solution is added to the solution containing equal moles of NaCl , NaBr, Nal and Na_{2}CrO_{4}?(i) Ag

_{2}CrO_{4}(ii)AgI

(iii) AgCl

(iv) AgBr

calculate the pH of 1.0 X 10^ -8 M solution of HCL ?

Ksp(BaSO4)= 1.5*10-9. find solubility in a)pure water b)0.1 M BaCl2 solution

The gas A

_{2}in the left flask allowed to react with gas B_{2}present in right flask as${\mathrm{A}}_{2}\left(\mathrm{g}\right)+{\mathrm{B}}_{2}\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{AB}\left(\mathrm{g}\right);{\mathrm{K}}_{\mathrm{c}}=4\mathrm{at}27\xb0\mathrm{C}.$

What is the concentration of AB when equilibrium is established?

112) Ionisation constant of CH3COOH is 1.7 * 10^ -5 and the conc. of H+ ions is 3.4 * 10^ -4. Then find out the initial conc. of CH3COOH molecules?

113) Solution of 0.1N NH4OH and 0.1 N NH4Cl has pH9.25 . Find pKb

Reaction between N

_{2}and O_{2}takes place as follows:If a mixture of 0.482 mol of N

_{2}and 0.933 mol of O_{2}is placed in a 10 L reaction vessel and allowed to form N_{2}O at a temperature for whichK_{c}= 2.0 × 10^{–37}, determine the composition of equilibrium mixture.how to use antilog.......... plss tell me its urgent???

Calculate amount of ammonium chloride required to dissolve in 500ml water to make p

^{H}= 4.5 [ K_{b}(NH_{3}) = 1.8 x 10^{-5}]??????Please I need a answer.......

CO (g) + 1/2 O2 equlibrium equal is Co2 (g) is

17. Silver nitrate is gradually added to an equeous solution containing 0.01 M each of chloride, bromide and iodide ions. The correct sequence ( decreasing order ) in which the halides will be precipitate is

(1) Br

^{-}, Cl^{-}, l^{-}(2) l^{-}, Cl^{-}, Br^{-}(3) l

^{-}, Br^{-}, Cl^{-}(4) Cl^{-}, Br^{-}, l^{-}_{2}at STP is1)22.4 M

2)0.25 M

3)M

4)4 M

_{2}=2CO, the equilibrium pressure is 12 atm. if 50% of CO_{2}reacts k_{p}for the change is