Question

a. 2Al(s)+3Cl2(g)→2AlCl3(s) You are given 19.0 g of aluminum and 24.0 g of chlorine gas.If you had excess aluminum, how many moles of aluminum chloride could be produced from 24.0 g of chlorine gas, Cl2?

b. Determine the balanced chemical equation for this reaction. C8H18(g)+O2(g)→CO2(g)+H2O(g)

c. 3H2(g)+N2(g)→2NH3(g) 1.08 g H2 is allowed to react with 10.3 g N2, producing 1.04 g NH3. What is the theoretical yield for this reaction under the given conditions? What is the percent yield for this reaction under the given conditions?

Answer 1

2Al (s t 3U2 (9) 2Alus (s) (713/mol) Molar Mass from wetl balauced eg, we kuow o u produces mole o Aec3 moles (3 x71) 2 mole oAec o1ch produces C will pro duces 2 mole 24.03 . A1C3 X 24.0 (3x1 0.225 moles ot Aecr 17 Kindly Submit Diffeeut Questeous spledy Please Rate