a) H2SO4(l)
b) CaSo4*2H20
c) Na2SO4(s)
a) H2SO4(l) b) CaSo4*2H20 c) Na2SO4(s) Review Problem 6.091 Enter the thermochemical equations, including values of...
0 AH; (kl mol-1) 90.37 33.8 81.57 9.67 Ca(s) 0 11 Review Intelligent Tutoring Problem 6.93 Using the data in the table below, calculate AH° in kilojoules for the following reactions. Standard Enthalpies of Formation of Typical Substances Substance AH() mol-1) Substance AH (K) mol-1) Substance Ag(s) H2O2(0) -187.6 CH (8) AgBr() -100.4 HBrg) -36 CH,OH(I) AgCl(s) - 127.0 HCl(g) -92.30 AO) HI(g) 26.6 CaBr20) Al2O3() -- 1669.8 HNO3(1) -173.2 CaCO3(9 CG) (graphite) H2SO4) -811.32 CaCl (5) CO(g) -110.5...
Incorrect. Did you remember to multiply the enthalpy values by the stoichiometric coefficients? Did you do enthalphy of products minus enthalphy of reactants? a) CH4(g)+C2(g) CH3Cl(g) +HCI(g) The number of significant digits is set to 3; the tolerance is +/-2 % x Incorrect. Did you remember to multiply the enthalpy values by the stoichiometric coefficients? Did yoif do enthalphy of products minus enthalphy of reactants? co(NH2) 2(s) + H20() b) 2NH3(g) + Co2(g) kJ The number of significant digits is...
1. 2. * Incorrect. What is the heat of formation of elements in their standard states? Did you use the correct equation of products minus reactants? The amino acid glycine, C2H5NO2, is one of the compounds used by the body to make proteins. The equation for its combustion is 4C2H5NO2(s) + 902(g) + 8C02(g) +10H20(1) +2N2(0) For each mole of glycine that burns, 973.49 kJ of heat is liberated. Use this information, plus values of AHF for the products of...