हिंदी
तमिलनाडु बोर्ड ऑफ सेकेंडरी एज्युकेशनएचएससी विज्ञान कक्षा ११

C(diamond) → C(graphite), ∆H = –ve, this indicates that - Chemistry

Advertisements
Advertisements

प्रश्न

C(diamond) → C(graphite), ∆H = –ve, this indicates that

विकल्प

  • graphite is more stable than diamond

  • graphite has more energy than diamond

  • both are equally stable

  • stability cannot be predicted

MCQ

उत्तर

graphite is more stable than diamond

shaalaa.com
Measurement of ΔU and ΔH Using Calorimetry
  क्या इस प्रश्न या उत्तर में कोई त्रुटि है?
अध्याय 7: Thermodynamics - Evaluation [पृष्ठ २२२]

APPEARS IN

सामाचीर कलवी Chemistry - Volume 1 and 2 [English] Class 11 TN Board
अध्याय 7 Thermodynamics
Evaluation | Q I. 10. | पृष्ठ २२२

संबंधित प्रश्न

The amount of heat exchanged with the surrounding at constant pressure is given by the quantity


The heat of formation of CO and CO2 are – 26.4 kCal and – 94 kCal, respectively. Heat of combustion of carbon monoxide will be


The enthalpies of the formation of Al2O3 and Cr2O3 are – 1596 kJ and – 1134 kJ, respectively. ∆H for the reaction \[\ce{2Al + Cr2O3 -> 2Cr + Al2O3}\] is


If one mole of ammonia and one mole of hydrogen chloride are mixed in a closed container to form ammonium chloride gas, then


When 15.68 litres of a gas mixture of methane and propane are fully combusted at 0°C and 1 atmosphere, 32 litres of oxygen at the same temperature and pressure are consumed. The amount of heat released from this combustion in kJ is (∆HC(CH4) = – 890 kJ mol−1 and ∆HC(C3H8) = – 2220 kJ mol−1)


Define the calorific value of food.


What is the unit of calorific value?


Explain how heat absorbed at constant volume is measured using a bomb calorimeter with a neat diagram.


In a constant volume calorimeter, 3.5 g of gas with molecular weight 28 was burnt in excess oxygen at 298 K. The temperature of the calorimeter was found to increase from 298 K to 298.45 K due to the combustion process. Given that the calorimeter constant is 2.5 kJ K−1. Calculate the enthalpy of combustion of the gas in kJ mol−1.


A gas mixture of 3.67 lit of ethylene and methane on complete combustion at 25°C and at 1 atm pressure produce 6.11 lit of carbon dioxide. Find out the amount of heat evolved in kJ, during this combustion. (ΔHC(CH4)) = − 890 kJ mol−1 and (ΔHC(C2H4)) = − 1423 kJ mol−1


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×