Advertisements
Advertisements
Question
Predict the feasibility of a reaction when both ΔH and ΔS negative.
Advertisements
Solution
When both ∆H and ∆S are negative, the reaction is not feasible.
APPEARS IN
RELATED QUESTIONS
The amount of heat exchanged with the surrounding at constant pressure is given by the quantity
C(diamond) → C(graphite), ∆H = –ve, this indicates that
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
The value of ∆H for cooling 2 moles of an ideal monatomic gas from 125°C to 25°C at constant pressure will be `["given C"_"P" = 5/2"R"]`
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)
Predict the feasibility of a reaction when both ΔH and ΔS positive.
Define the calorific value of food.
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.
Calculate the standard heat of formation of propane, if its heat of combustion is −2220.2 kJ mol−1 the heats of formation of \[\ce{CO2_{(g)}}\] and \[\ce{H2O_{(l)}}\] are −393.5 and −285.8 kJ mol−1 respectively.
