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Syllabus

Noble gases have high positive values of electron gain enthalpy

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 heat evolved at constant volume .

( R = 8.314 J / K mol. )

what is the difference between Qc and kc.

1) freezing of water?

2) cooling of gas from 80 degree Celsius to 20 degree Celsius?

3) evaporating ethanol at room temperature

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

a) open system

b) closed system

c) isolated system

d) none of the above

The 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

_{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

what is the significance of delta U and delta H? I want a brief answer

please explain

brieflycp-cv=Rwhy change in volume is area * displacement??

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

how does entropy change with decrease in pressure?

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.

^{o}C. If the work done in this process is 3KJ,then find the final temperature of the gas (C_{v}=20J/mol)35 ML OF OXYGEN WERE COLLECTED AT 6 DEGREE CELCIUS AND 758 MM PRESSURE. CALCULATE ITS VOLUME AT NTP? WHAT IS THE VALUE OF T

_{2}HERE.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.

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

entropy are spontaneous at lower temperature. Justify on the basis

of Gibbs equation.

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

H

_{2}(g) + I_{2}(g) --_{}2HI(g)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)

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)

^{(dH/dt)p-(dU/dt)v=R (B) (dH/dt)p > (dU/dt)v (C)(dU/dV) for ideal gas is zero (D)all are correct}_{2}Cl_{6}_{ }from the following data :(i) 2Al(s) + 6HCl (aq) $\to $ Al

_{2}Cl_{6}(aq) + 3H_{2}(g);${\u25b3}_{r}H\xb0=-1004.0kJ$

(ii) H

_{2}(g) + Cl_{2}(aq) $\to $ 2HCl(g);$\u25b3$

_{r}H$\xb0$ = $-183.9kJ$(iii) HCl(g) + aq $\to $ HCl(aq);

${\u25b3}_{r}H\xb0=-73.2kJ$

(iv) Al

_{2}Cl_{6}(s) + aq $\to $ Al_{2}Cl_{6}(aq);${\u25b3}_{r}H\xb0=-643.0kJ$

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

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.

What do you mean by Cp and Cv. Derive the relation between Cp and Cv.

explain the effect of temperature on spontinity of exothermic and endothermic reaction?plz reply soon

Solve this :$3.\mathrm{The}\mathrm{process}{\mathrm{CH}}_{3}\mathrm{COOH}\underset{}{\overset{}{\to}}{\mathrm{CH}}_{3}{\mathrm{COO}}^{-}+{\mathrm{H}}^{+},\mathrm{should}\mathrm{be}:\phantom{\rule{0ex}{0ex}}\left(1\right)\mathrm{exothermic}\left(2\right)\mathrm{endothermic}\phantom{\rule{0ex}{0ex}}\left(3\right)\mathrm{nethier}\mathrm{exothermic}\mathrm{nor}\mathrm{endothermic}\left(4\right)\mathrm{exothermic}\mathrm{or}\mathrm{endothermic}\mathrm{depending}\mathrm{upon}\mathrm{tempreature}$

_{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^{-}ions(NO LINKS)Derive C

_{p}- C_{v}= R.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

Calorific valueof ethane, in kJ/g if for the rxn

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

Ans -52

How?

3 mol of an ideal gas at 1.5 atm and 25 degree celsius expands isothermally in a reversible manner to twice the original volume against an external pressure of 1 atm. calculate the work done....

A) ETHYLENE

B) PROPYLENE

C) 1:1 MIXTURE OF TWO GASES

how to convert Ethyne to acetaldehyde ?

i) Freezing of water ii) Condensation of steam iii) Cooling of a liquid iv) Dissolution of a solute

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.

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. W = -∆U a) Enthalpy change

2. ∆U = 0 b) Universal gas constant

3. Cp - Cv c) Adiabatic process

4. qP d) Isothermal process

e) Cyclic process

difference between state function and state variable?

show that the heat absorbed at constant volume is equal to increase in internal energy of the system wheras that at constant pressure is equal to the increase in enthalpy of the system

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?

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

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.

2A ₂ (g) + 5B ₂ (g) -------> 2A ₂ B5 (g)

at temperature = 27°C that is... 300Kelvin

The difference between deltaH and deltaE is X.

We have to find the ratio X/R.

I'm a bit confused to place which value of R here.

Please try to answer it before 1:00pm today.

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?

_{2}O at its boiling point is1) 3 cal mol

^{}^{-1}K^{-1}2)5 cal mol

^{-1}^{}K^{-1}3) 7 cal mol

^{-1}^{}K^{-1}4) Infinite

ANS : 4) how?

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 .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.

what is the use of stirrer in these calorimeters..

write the conjugate acid and base of H2O2 ???

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

how will we draw a born haber cycle for MgCl2 ?

What isfirst law of thermodynamics.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.

how does Hess's law follow 1st law of thermodynamics?

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.