Question

Name: Section: Date: Worksheet 9 Equation Stoichiometry CHEM 2 Show all work to get full credit 1. The balanced equation for the decomposition of TNT, CH (NO2). is 2 C.H.(NO3)(s) - 7 C(s) + 7 CO(g) + 3 Nxg) - 5 H.O(g) a. How many moles of CO gas are produced from the decomposition of 6.00 moles of TNT? b. How many grams of CO gas are produced from the decomposition of 6.00 moles of TNT? C. How many moles of solid carbon are produced from 1.00 kg of TNT?! d. How many grams of solid carbon are produced from 1.00 kg of TNT? 2. Given the unbalanced equation: CsHg + O2 CO2 + H2O a. How many moles of oxygen gas are required to make 4.00 moles of carbon dioxide? b. How many moles of CsHe must be used to produce 2.00 grams of water?

Answer 1

The balanced reactionis 2 CH (NO2)3(s)—*7C(s) +7C0 ()+31(g)+5H,0 (8) From the above reaction, one moleof TNT produces 7 moles of CO. Calculate the moles of CO produced for 6.0 moles of TNT as follows: 6.0 moles TNT x 6.00 molesco " Imolestit =18.Omoles of Co Therefore, 18.0 moles of CO produces for 6.00 moles of TNT b) Calculaate the mass of CO produces for 6.0 moles of TNT used as follows: 28.01gCo-5,04 x 10 gCO 18.0 moles Cox 28.01gco Imole co +5.0410* gco Therefore, mass of CO produced for 6.0moles of TNT used is 5.04x10° g. Calculate number of molesof C(s) produces for 1.00 Kg TNT as follows: 1.00 Kg TNT x 10°g x Imole TNT 7 moles C(s) nam 1,0 Kg 227.13g TNT” 7 moles TNT = 4.40molesC () Hence, molesof C(s) is 4.40 moles. d) Calculate the mass of C(s) as follows: 12.01g C 4.40 moleCx 52.9gc 1molec Therefore, the mass of solid carbon produces for 1.00 kg TNT is 52.9g.

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