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Syllabus

Noble gases have high positive values of electron gain enthalpy

calculate the enthalpy of formation of methane

C +O2 --CO2 deltaH = -393.7 KJ/MOL

H2+1/2 O2 ---H2O H= -285.8 KJ/MOL

CH4 +2O2 ---CO2+2H2O H = -890.4 KJ/MOL

Standard enthalpy of vapourisation D

_{vap}H^{Q}for water at 100° C is 40.66 kJmol^{–1}. The internal energy of vapourisation of water at 100°C (in kJmol^{–1}) is ?calculate the standard enthalpy of formation of ethene (C2H4)from the following equation-

C2H4(g) + 3O2(g)-----》 2CO2 +2H2O enthalpy of formatiom of reaction is -1323 kJ/m

Enthalpy of formation of CO2,H2O and O2 are -393.5 ,-249,0 respectively

what is the difference between Qc and kc.

_{12}H_{22}O_{11}) from the following data :-(1) C

_{12}H_{22}O_{11}+ 12 O_{2}---------->12 CO_{2}+_{}11 H_{2}O..................dH = -5200.7 KJ/mol(2)C + O

_{2}-----------> CO_{2}.................dH= -394.5(3) H

_{2}+ 1/2O_{2}---------> H_{2}O...................dH = -285.8 KJ/molThe work done in an open vessel at 300 K, when 112 g iron reacts with dil HCl to give FeCl2 is?

Ans 1.2 kcal

For the reaction NH4Cl (s) NH3 (g) + HCL (g) at 25 , enthalpy change DH = +177 kJ per mole and entropy change triangle DS = +285 JK^{-1}mol^{-1}.Calculate free energy changeDG at 25°C and predict whether the reaction is spontaneous or not._{2}is mixed with 11.2 L of H_{2}at STP?a) 0.576 J/K

b) 5.76 J/K

c) 7.56 J/K

d) 2.76 J/K

6C + 2H2 gives C6H6

The standard enthalpy of combustion of Benzene is -3266.0 kJ and standard enthalpy of formation of CO2 and H2O are -393.1 kJ and -286.0 kJ respectively.

please explain

brieflycp-cv=RC(graphite) + O2---------> CO2, H= -393.5 kJ/mol

H2 + 1/2 O2 ------>H2O ,H= -269.4kJ/mol

6C + 6H2 + 3O2 -------> C6H12O6 , H= -1169.8kJ/mol

2NH

_{3 }+ CO_{2}NH_{2}CONH_{2}+ H_{2}OGibbs' energy at 298K=-13.6 kJ mol

^{-1}. Find the equilibrium constant at 298 K.Q109. At 300 K the standard enthalpies of formation of C

_{6}H_{5}COOH_{(s)}, CO_{2}_{(g)}and H_{2}O_{(i)}are – 408, – 393 and – 286 kJ mol^{–1}respectively. Calculate the heat of combustion of benzoic acid at contant volume :(1) + 3201 kJ

(2) + 3199.75 kJ

(3) – 3201 kJ

(4) – 3199.75 kJ

Starting with the thermodynamic relationships, G=H-TS,derive the following relationship:

deltaG=-TdeltaS(total).

^{o}C. If the work done in this process is 3KJ,then find the final temperature of the gas (C_{v}=20J/mol)The enthalpy of combustion of ethyl alcohol is 1380.7 KJ/mol. If the enthalpies of formation of CO2 and H20 are 394.5 and 286.6 KJ/mol. Calculate the enthaply of formation of ethyl alcohol.

derive the relationship between delta H and delta U for an ideal gas .explain each term involved in the equation.

With the help of first law of thermodynamics and H = U + pv, prove dH = qp...

what is the value of (delta) ng for the following reaction :-

H

_{2}(g) + I_{2}(g) --_{}2HI(g)THE HEAT OF COMBUSTION OF METHANE AT CONSTANT VOLUME IS MEASURED IN A BOMB CALORIMETER AT 298K AND IS FOUND TO BE -885KJ/MOL. CALCULATE THE HEAT OF COMBUSTION AT COSTANT PRESSURE.

A spherical balloon of 21 cm diameter is to be filled up with hydrogen at NTP from a cylinder containing the gas at 20 atm. at 27 degree celcius. If the cylinder can hold 2.82 litres of water, calculate the numbers of balloons that can be filled up ?

what is atomicity of gas?explain briefly

If enthalpy of a reaction CH2Cl2 (g) --- C (g) + 2H (g) + 2Cl (g) is 1482 kJ/mol and bond dissociation enthalpy of (C-H) bond is 415 kJ/mol than bond dissociation enthalpy of (C-Cl) bond is

Find the difference between heats of reaction at constant pressure and constant volume for the following reaction at 25 C in kJ.

2C6H6 + 15O2 ---------> 12CO2 + 6H2O.

^{o}C ?What do you mean by Cp and Cv. Derive the relation between Cp and Cv.

Calculate the bond enthalpy of Cl-Cl bond from the following data

CH

_{4}+Cl_{2}--------> Ch_{3}Cl+HClΔH= -100.3kJ. Also the bond enthalpies of C-H, C-Cl, H-Cl bonds are 413, 326 & 431 kJ mol

^{-1 }respectively.Q. Calculate the enthalpy of combustion of ${B}_{2}{H}_{6}$ from the following data:

$B\left(s\right)+3{O}_{2}\left(g\right)\to 2{B}_{2}{O}_{3}\left(s\right)\phantom{\rule{0ex}{0ex}}{\u2206}_{f}H=-2546.0kJmo{l}^{-1}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}{H}_{2}\left(g\right)+1/2{O}_{2}\left(g\right)\to {H}_{2}O\left(l\right)\phantom{\rule{0ex}{0ex}}{\u2206}_{f}H=-286.0kJmo{l}^{-1}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}{H}_{2}O\left(l\right)\to {H}_{2}O\left(l\right)\phantom{\rule{0ex}{0ex}}{\u2206}_{f}H=+44.0kJmo{l}^{-1}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\u2206B\left(s\right)+3/2{H}_{2}\left(g\right)\to 1/2{B}_{2}{H}_{6}\left(g\right)\phantom{\rule{0ex}{0ex}}{\u2206}_{f}H=+18.0kJmo{l}^{-1}\phantom{\rule{0ex}{0ex}}$

Derive C

_{p}- C_{v}= R.Q. The enthalpy of solution of anhydrous CuS${O}_{4}$ is - 15.9 kCAl/mol and that of CuS${O}_{4}$.5${H}_{2}O$ is 2.8

kCal/mol. Calculate the enthalpy of hydration (in kCal/mol) of anhydrous CuS${O}_{4}$ into CuS${O}_{4}$.5${H}_{2}O$

Report your answer in terms of magnitude, rounding it off to the nearest whole number.

_{2}O(l) is -280.70 kj/mol and enthalpy of neutralisation of strong acid and strong base is -56.70 kj/mol. What is the enthalpy of formation of OH^{-}ionsQ.Calorific valueof ethane, in kJ/g if for the rxn

2C2H6 + 7O2--- 4CO2 + 6H2O + 745.6 kcal

Ans -52

How?

calculate the enthalpy of the reaction of C2H4(g)+H2(g) give rise to C2H6(g)from the the following data??

pls fast urgent I want it within 2hrs????pls plsssssssss help

A) ETHYLENE

B) PROPYLENE

C) 1:1 MIXTURE OF TWO GASES

how to convert Ethyne to acetaldehyde ?

difference between state function and state variable?

If water vapour is assumed to be a perfect gas, molar enthalpy change for vapourisation of 1 mol of water at 1bar and 100°C is 41kJ mol

^{-1}. Calculate the internal energy change, when(i) 1 mol of water is vaporised at 1 bar pressure and 100°C.

(ii) 1 mol of water is converted into ice.

predict the sign of entropy change for the following:-

a)C(graphite)-C(diamond)

b)electrolysis of NaCl solution

c)sublimation of camphor

d)CaCO3(s)-CaO(s)+ CO2(g)

For an isolated system, delta U = 0; what will be delta S?

The combustion of one mole of benzene takes place at 298 K and 1 atm. After combustion, CO2(g) and H2O (1) are produced and 3267.0 kJ of heat is liberated. Calculate the standard enthalpy of formation, ΔfHΘof benzene. Standard enthalpies of formation of CO2(g) and H2O(l) are -393.5 kJ mol1and 285.83kJ mol1respectively.

1)0.6 2)0.3 3) 2 4)6

Calculate the amount of heat evolved when[1] 500cm3 of 0.1 M HCl acid is mixed with 200cm3 of 0.2 M NaOH solution [2] 200cm3 of 0.2 M H2SO4 is mixed with 400cm3 of 0.5 M KOH solution. Assuming that the specific heat of water is 4.18 K-1 g-1 ignoring the heat absorbed by the container, therometer, stirrer etc., what would be the rise is temperature in each of the above cases?

A 5 L cylinder contains 10 moles of oxygen at 27 degrees celsius. Due to sudden leakage through the hole, all the gas escaped into the atmosphere and the cylinder got empty. If the atmospheric pressure is 1 atm, calculate the work done by the gas.

Bond dissociation enthalpies of hydrogen(g) and nitrogen(g) are 436.0 kJ/mol and 941.8 kJ/mol and enthalpy of formation of NH3(g) is -46kJ/mol .What is the enthalpy of atomisation of NH3? What is the average bond enthalpy of N - H bond?

the heat of combustion of benzene in a bomb calorimeter was found to be 3263.9 kj/mol at 25 C.calculate the heat of combustion of benzene at constant pressure?

Calculate the enthalpy change on freezing of 1.0 mol of waterat 10.0°C to ice at –10.0°C. Δ

_{fus}H= 6.03 kJ mol^{–1}at 0°C.C_{p}[H_{2}O(l)] = 75.3 J mol^{–1}K^{–1}C_{p}[H_{2}O(s)] = 36.8 J mol^{–1}K^{–1}A 10CM COLUMN OF AIR IS TRAPPED BY AN 8CM LONG COLUMN OF Hg in a capillary tube horizontally fixed at 1 atm pressure . calculate the length of air column .when the tube is fixed

a) Vertically with open end up

b) Vertically with open end down

c) At 45

^{o}from the horizontal with the open end up .1) H

^{+}(aq) + OH^{-}(aq) ----------> H_{2}O(l);ΔH= -X_{1}kJ/mol2) H

_{2}(g) + 1/2 O_{2}(g) ----------> H_{2}O(l);ΔH = -X_{2}kJ/mol3) CO

_{2}(g) + H_{2}(g) ------------> CO(g) + H_{2}O(l);ΔH = -X_{3}kJ/mol4) C

_{2}H_{2}(g) + 5/2 O_{2}(g) ------------> 2CO(g) + H_{2}O(l);ΔH = +X_{4}kJ/mol

Enthalpy of formation of H

_{2}O(l) is:-a) +X

_{1}kJ/molb) +X

_{2}kJ/molc) +X

_{3}kJ/mold) +X

_{4}kJ/mol Kindly answer sir/mam.

For a reaction,both delta H and delta S are positive.under what condition,the reaction occurs spontaneously

write the conjugate acid and base of H2O2 ???

Predict the feasibility of a reaction when

(i) both delta H and delta S increases.

(ii)both delta H and delta S decreases.

(iii)delta H increases but delta S decreases.

(iv)delta H decreases but delta S increases.

What isfirst law of thermodynamics.how will we draw a born haber cycle for MgCl2 ?

CH2 = CH2 (g) + H2 (g) → CH3 -CH3 (g).

The bond energies of C-C, C-H, H-H and C = C bonds are 83 k cal, 99 k cal,

104k cal and 145 k cal respectively.

an athlete is given 180g of glucose (c6 h12 o6). he utilises 50% of the energy due to internal combustionin the body. In order to avoid storage of energy oin the body, calculate the mass of water he'll need to perspire.

Given enthalpy of combustion of glucose is -2800 kj/mol and enthalipy os evaporation of water is 44kj/mol.

Enthalpy of solution (ΔH) for BaCl_{2 }. 2H_{2}O & BaCl_{2}are 8.8 & -20.6kJ mol^{-1}reapectively. Calculate the heat of hydration of BaCl_{2}to BaCl_{2 . }2H_{2}O................The molar heat of formation of nh4no3 (s) is -367.54 kj and those of no2(g) is 81.46and h2o(l) is -285.78 kj at 298k and 1.0 atmospheric pressure .Calculate delta H and delta U for the reaction.