Use the following reactions to find H when 1 mole of HCl gas forms from its elements:
N2(g) + 3 H2(g) 2 NH3(g) H = 91.8 kJ
N2(g) + 4 H2(g) + Cl2(g) 2 NH4Cl(s) H = 628.8 kJ
NH3(g) + HCl(g) NH4Cl(s) H = 176.2 kJ
we need:
1/2H2(g) + 1/2Cl2(g) = HCl(g)
therefore...
invert rxn 3
NH4Cl = NH3 + HCl H = 176.2
divide rxn2 so we can cancel NH4Cl
1/2N2 + 2H2 +1/2Cl2 = NH4Cl H = -628.8/2 = - 314.4
add previous 2 reactions
1/2N2 + 2H2 +1/2Cl2 + NH4Cl = NH3 + HCl + NH4Cl H = 176.2-314.4 = - 138.2
cancel common terms
1/2N2 + 2H2 +1/2Cl2 = NH3 + HCl H = - 138.2
now.. invert and divide by 2 rxn 1
NH3 = 1/2N2 + 3/2H2 H= -1/2*(-91.8) = 45.9
now add previous 2
NH3 + 1/2N2 + 2H2 +1/2Cl2 = NH3 + HCl + 1/2N2 + 3/2H2 H = - 138.2+45.9
cancel commont erms
1/2H2 +1/2Cl2 = HCl + H = -92.3 kJ/mol
Use the following reactions to find H when 1 mole of HCl gas forms from its elements: N2(g) + 3 H2(g) 2 NH3(g) ...
Given the following information, N2(g) + 4 H2(g) + Cl2(g) 2 NH4Cl(s) H= -628.8 kJ what is the H if 13.8g of hydrogen gas is consumed in the reaction? A) -2.15x10^3 KJ B) -8.61x10^3 KJ C) -1.08x10^3 KJ D) -6.29x10^2 KJ
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I will rate. thank you N2(g)+ 3 H2(g)= 2 NH3 Find delta G of reaction when mixing 4 mol of nitrogen, 12 moles of of h2 and 4 mol nh3 (pressure = 1 bar) temp = 50c