Question

Given the following thermochemical equation: 2 Al + Fe_2O_2 rightarrow Al_2O_2 + 2Fe delat H = - 852 kJ What is Delta H when 0.100 mal of Al_2O_3 react with 0.250 mol of Fe? _____ kJ Using the data from Appendix G of the textbook, calculate Delta H for the combustion of 1.00 mole of C_2H_5OH(l). Note that (g) or (l) after the chemical formula denotes whether the compound is a gas or liquid. Some compounds have entries for both. Also, assume that water is formed as a liquid. ______ kJ Diborane is a gaseous chemical which oxidizes to boron oxide as follows: b_2H_5(g) + 3O_2(g) rightarrow B_2O_3(S) + 3H_2O(g) This very exothermic reaction produces 2147.5 kJ of energy. If the Delta H^degree_t for the boron oxide solid is -2509.1 kJ/mol and for the water. it is -241.8 kJ/mol, determine the enthalpy of formation for the diborane. Delta H_f = __________ kJ/mol The sugar glucose is burned in the body to produce energy the combustion reaction proceeds according to the following reaction: C_6H_12O_6(s) + 6O_2(g) rightarrow 6CO_2(g) + 6H_2O(g) Using the data Appendix g of the textbook, calculate the enthalpy of the reaction for 4.7 mol of glucose. Use -1274.5 kJ/mol as the enthalpy of formation of glucose. Delta H degree = ______ kJ

Answer 1

3)

according to reaction, 1 mol of Al2O3 will react with 2 mol of Fe

So,

0.100 mol of Al2O3 will react with 0.200 mol of Fe and remaining are unreacted

The backward reaction will take placeSo, Q will be positive

for 1 mol Al2O3, delta H = 852 KJ (positive because backward reaction will take place)

here,

mol of Al2O3 = 0.100 mol

so,

delta H = 0.100*852 KJ = 85.2 KJ

Answer: 85.2 KJ

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