NAMES Aan 1) Which of the a syok o heat from E) None of these of these represent
ID: 906632 • Letter: N
Question
NAMES Aan 1) Which of the a syok o heat from E) None of these of these represent the system referenced above 2) Foe 2) For AEsys to always be - what mast he true? Define heat capacity. °C substance byrc substance by 1°C the quantity of heat required to raise the temperature of 1 mole of a substance by 1 the quantity of heat required to change a sysem's temperature by 1C the quantity of heat regard to raise the temperaure of i gram of a C) the D) the quanmity of heat required to raise the temperature of 1 g of a sutstance by E) the quantity of heat required to raise the temperature of I liner of a 4) Calculate the amount 385.0 K. The specific heat capacity of e amount of heat (in kJ) required to raise the temperature of a 79.0 g sample of ethanol from 298.0 K so C) 736 kJ D) 284 k E) 12.9 kJ 5) A 498 g sample of aniline (CSHSNH2, molar mass 93.13 /mol) was combasted in a bomb calorimeter with a beaf capacity of 4.23 urC. If the temperature rose If the temperature rose from 29.5'C to 69.8"C, determine the value of AH comb for aniline. )+781 103 kmol C) +1.71×103 kJ/mol D)-1.71 x 103 kJ/mol -3232.2 3232 )-7.81 x 103 kJ/mol l mo l ) Using the following thermochemical equation, determime the amount of heat produced from the combustion of enzene (C6H6). The molar mass of benzene is 78.11 g/mole. ) 3910 kJ ) 1950 kJ 977 J 40.1kJ D 027.1Explanation / Answer
1) A) q +ve and W -ve
2) D) -w > +q
3) B) The quantity of heat required to change a systems temp. by 1 degree C
4) Q = 79 x 2.42 x (385 - 298) = 16632.7 J = B) 16.6 KJ
5) Heat Relesed during reaction = 4.25 x (69.8 - 29.5) = 171.275 KJ
Moles of aniline combusted = 4.98 / 93.13 = 0.05347 moles
=> delta H combustion = - 171.275 / 0.05347 =B) - 3.2 x 10^3 KJ (-ve since exothermic reaction)
6) According to the reaction,
Heat produced for combustion of 2 moles of Benzene = 6278 KJ
Moles of Benzene = 24.3 / 78.11 = 0.311 moles
=> Heat produced = 6278 x 0.311 / 2 = 976.5 KJ = C) 977 KJ
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