हिंदी

Define the Enthalpy of ionisation. - Chemistry

Advertisements
Advertisements

प्रश्न

Define the Enthalpy of ionisation.

परिभाषा

उत्तर

Enthalpy of ionization is the enthalpy change accompanying the removal of an electron from one mole of a gaseous atom.

shaalaa.com
Thermochemistry
  क्या इस प्रश्न या उत्तर में कोई त्रुटि है?
अध्याय 4: Chemical Thermodynamics - Long answer questions

APPEARS IN

एससीईआरटी महाराष्ट्र Chemistry [English] 12 Standard HSC
अध्याय 4 Chemical Thermodynamics
Long answer questions | Q 2.2

संबंधित प्रश्न

Answer the following in one or two sentences.

What is standard state of a substance?


Answer in brief.

How will you calculate reaction enthalpy from data on bond enthalpies?


Calculate the total heat required

a) to melt 180 g of ice at 0 °C

b) heat it to 100 °C and then

c) vapourise it at that temperature.

[Given: ΔfusH° (ice) = 6.01 kJ mol-1 at 0 °C, ΔvapH° (H2O) = 40.7 kJ mol-1 at 100 °C, Specific heat of water is 4.18 J g-1 K-1]


Calculate enthalpy of formation of HCl if bond enthalpies of H2, Cl2 and HCl are 434 kJ mol-1, 242 kJ mol–1 and 431 kJ mol–1 respectively.


Define the Standard enthalpy of combustion.


State and explain Hess’s law of constant heat summation.


Calculate the standard enthalpy of combustion of CH4(g) if ΔfH°(CH4) = – 74.8 kJ mol–1, ΔfH°(CO2) = – 393.5 kJ mol–1 and ΔfH°(H2O) = – 285.8 kJ mol–1.


Calculate the standard enthalpy of formation of liquid methanol from the following data:

  1. \[\ce{CH3OH_{(l)} + \frac{3}{2} O_{2(g)} -> CO_{2(g)} + 2H2O_{(l)}}\]     ∆H° = – 726 kJ mol–1
  2. \[\ce{C_{(Graphite)} + O_{2(g)} -> CO_{2(g)}}\]          ∆cH° = – 393 kJ mol–1
  3. \[\ce{H_{2(g)} + \frac{1}{2} O_{2(g)} -> H2O_{(l)}}\]          ∆fH° = – 286 kJ mol–1 

Define the Bond enthalpy.


Write an application of Hess’s law.


When 2 moles of C2H6(g) are completely burnt, 3129 kJ of heat is liberated. If ∆Hf for CO2(g) and H2O(l) are −395 and −286 kJ per mole respectively, the heat combustion of C2H6(g) is ____________.


The volume of oxygen required for complete combustion of 0.25 mole of methane at STP is ______.


When 6.0 g of graphite reacts with dihydrogen to give methane gas, 37.4 kJ of heat is liberated. What is standard enthalpy of formation of CH4 (g)?


Daily requirement of energy of a person is 'x' kJ. If heat of combustion of food material (Molecular mass = 100 g) is 'y' kJ, his daily consumption of the food in gram would be ____________.


Enthalpy of formation of two compounds x and y are −84 kJ and −156 kJ respectively. Which of the following statements is CORRECT?


Combustion of glucose takes place as

\[\ce{C6H12O6_{(s)} + 6O2_{(g)} -> 6CO2_{(g)} + 6H2O_{(g)}}\]; ΔH = −72 kcal mol−1

The energy needed for the production of 1.8 g of glucose by photosynthesis will be ___________.


The enthalpy of formation of nitrogen dioxide is +33.2 kJ mol−1. The enthalpy of the reaction \[\ce{2N2_{(g)} + 4O2_{(g)} -> 4NO2_{(g)}}\]; is ____________.


\[\ce{A -> B}\], ∆H = −10 kJ mol−1, Ea(f) = 50 kJ mol−1, then Ea of \[\ce{B -> A}\] will be ______.


What is enthalpy of formation of NH3 if bond enthalpies as (N ≡ N) = - 941 kJ/mol.

\[\ce{(H - H)}\] = 436 kJ/mol and \[\ce{(N - H)}\] = 389 kJ/mol?


Define and explain the term, enthalpy of reaction.


Which of the following reactions defines the enthalpy of formation?


Standard enthalpy of combustion of a substance is given. Then Write thermochemical equation.

ΔcH0[C2H5OH(1)] = - 1409 kJ mol-1


The enthalpy of combustion of S (rhombic) is − 297 kJ mo1-1. Calculate the amount of sulphur required to produce 29. 74 kJ of heat.


Draw energy profile diagram and show:

  1. activated complex
  2. energy of activation for forward and backward reactions
  3. enthalpy of reaction

For the reaction, H2 + I2 ⇌ 2HI; ΔH = 12.4 kcal. The heat of formation of HI, ΔHf = ______.


Calculate the standard enthalpy of combustion of methane if the standard enthalpy of formation of methane, carbon dioxide and water are −74.8, −393.5 and −285.8 kJmol−1 respectively.


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×