In any chemical reaction, a quantity that decrease to a minimum is
free energy
entropy
temperature
enthalpy
Given, H2O (l) → H2O (g); H1 = +43 kJ
H2O (s) → H2O (l); H2 = +6.05 kJ. Calculate the enthalpy of sublimation of ice.
49.75 kJ mol-1
37.65 kJ mol-1
43.7 kJ mol-1
55.23 kJ mol-1
Heat formation of H2O is -188 kJ/ mol and H2O2 is 286 kJ/mol. The enthalpy change for the reaction; 2H2O2 → 2H2O + O2 is
196 kJ
-196 kJ
984 kJ
-984 kJ
When 1 mole of a gas is heated at constant volume, temperature is raised from 298 K to 308 K. Heat supplied to the gas is 500J. Then, which statement is correct?
q= -W = 500J : ΔE= 0
q= W = 500J : ΔE= 0
q = ΔE= 500J , W= 0
ΔE = 0; q= W = -500J
If enthaplies of formation for C2H2(g), CO2(g) and H2O(l) at 25°C and 1atm pressure be 52, -394 and -286kJ mol-1 respectively, then the enthaply of combustion of C2H4(g) will be
-141.2 kJ mol-1
-1412 kJ mol-1
+ 141.2 kJ mol-1
+ 1412 kJ mol-1
The enthalpy of combustion for the H2, cyclohexene and cyclohexane are -241, -3800 and -3920 kJ mol-1 respectively. Heat of hydrogenation of cyclohexene is
121 kJ mol-1
-121 kJ mol-1
242 kJ mol-1
-242 kJ mol-1
Given that N2(g) + 3H2(g) → 2NH3(g): ΔrH° =-92kJ, the standard molar enthalpy of formation in kJ mol-1 of NH3(g) is
-92
+46
+92
-46
D.
-46
N2(g) + 3H2(g) → 2NH3(g): ΔrH° =-92kJ,. Chemical reaction for molar entyhalpy of formation of NH3,
N2(g) + H2(g) → NH3(g) ( therefore, H for N2 and H2 = 0)
Therefore , .
In view of for the following reactions
PbO2 + Pb → 2PbO,
SnO2 + Sn → 2SnO,
Which oxidation state is more characteristic for lead and tin?
For lead +2, for tin +2
For lead +4, for tin +4
For lead +2, for tin +4
For lead +4, for tin +2
The enthalpy of the formation of CO2 and H2O are -395 kJ and -285 kJ respectively and the enthalpy of combustion of acetic acid is 869 kJ. The enthalpy of formation of acetic acid is
340 kJ
420 kJ
491 kJ
235 kJ