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Noble gases have high positive values of electron gain enthalpy
Standard enthalpy of vapourisation DvapHQ for water at 100° C is 40.66 kJmol–1. The internal energy of vapourisation of water at 100°C (in kJmol–1) is ?
what is the difference between Qc and kc.
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
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
please explain cp-cv=R briefly
how does entropy change with decrease in pressure?
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
why change in volume is area * displacement??
Derive Gibbs Energy change and non mechanical work.
derive the relationship between delta H and delta U for an ideal gas .explain each term involved in the equation.
what is the value of (delta) ng for the following reaction :-
H2(g) + I2(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.
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?
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.
what is the significance of delta U and delta H? I want a brief answer
what is the use of stirrer in these calorimeters..
Derive Cp- Cv = 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
how to convert Ethyne to acetaldehyde ?
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.
what is exactly meant by enthalapy H.
difference between state function and state variable?
Calculate the amount of heat evolved when 500cm3 of 0.1 M HCl acid is mixed with 200cm3 of 0.2 M NaOH solution  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.
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. ΔfusH= 6.03 kJ mol–1at 0°C.
Cp[H2O(l)] = 75.3 J mol–1K–1
Cp[H2O(s)] = 36.8 J mol–1K–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 45o from the horizontal with the open end up .
Why does a liquid boils at a lower temperature at the top of a mountain than at sea level?
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
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.
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
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.
how will we draw a born haber cycle for MgCl2 ?
What is first law of thermodynamics.
Enthalpy of solution (ΔH) for BaCl2 . 2H2O & BaCl2 are 8.8 & -20.6kJ mol-1 reapectively. Calculate the heat of hydration of BaCl2 to BaCl2 . 2H2O................
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.
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.
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