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The standard enthalpy of formation of phenol is -165.0 k) mol-I. Calculate its standard enthalpy of combustion.
From the following data, determine ∆f Ho for diborane, B2H6 (g), at 298 K:
(I) B2H6 (g) + 3 O2 (g) → B2O3(s) + 3 H20 (g) ∆t Ho=-1941 kJ mol-1
(2) 2 B(s) + t Oh) → B2O3(S)
∆t, Ho = -2368 kJ mol-1
(3) H2 (g) + + 02(g) → H2O (g)
∆t, Ho = -241.8 kJ mol-1
When 2.25 mg of anthracene, CI4HlO(s), was burned in a bomb calorimeter the temperature raised by 1.35 K. Calculate the calorimeter constant. By how much will the temperature rise when 135 mg of phenol, C6HsOH(s), is burned in the calorimeter under the same conditions? (∆.c H (C14H1O, s) =-7061 k) mol-1)
Calculate the standard enthalpy of solution of AgBr(s) in water from the enthalpies of formation of the solid and the aqueous ions.
Given that the standard enthalpy of combustion of graphite is -393.51 kJ mol-1 and that of diamond is -395.41 kJ mol-1, calculate the enthalpy of the graphite-to-diamond transition.
Given the reactions (1) and (2) below, determine
(a) ∆Ho and ∆Uo for reaction (3),
(b) -∆Ho for both HI (g) and H20 (g) all at 298 K.
(1) H2 (g) + I2(s) → 2 HI (g)
∆, H" = +52.96 kJ mol-1
(2) 2 H2 (g) + 02(g) → 2 2 H20 (g)
∆, H= -483.64 k] mol-1
(3) 4 HI (g) + 02(g) → 2 I2(s) + 2 H2O (g)
For the reaction 2 C6HsCOOH(s) + 13 02(g) → 12 CO2 (g) + 6 H20 (g), -∆Uo= -772.7 k) mol-1 at 298 K. Calculate -∆1Ho.
Calculate the standard enthalpy of formation of NOCI (g) from the enthalpy of formation of NO given in Table 2.5, together with the following information:
2 NOCl (g) → 2 NO (g) + Clz (g)
∆1 Ho = + ∆Uo= +75.5 kJ mol-1
Use the information in Table 2.5 to predict the standard reaction enthalpy of2 H2 (g) + 02(g) → 2 H2O (1) at 100°C from its value at 25°C.
Calculate ∆tHo and ∆tUo at 298 K and ∆Ho at 348 K for the hydrogenation of ethyne (acetylene) to ethene (ethylene) from the enthalpyof combustion and heat capacity data in Tables 2.5 and 2.7. Assume the heat capacities to be constant over the temperature range involved.
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