Math  /  Algebra

Question(11) Calculate how many moles of NO2\mathrm{NO}_{2} form when each quantity of reactant completely reacts: 2 N2O3( g)4NO2( g)+O2(g)2 \mathrm{~N}_{2} \mathrm{O}_{3}(\mathrm{~g}) \longrightarrow 4 \mathrm{NO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(g) a. 2.5 mol N2O52.5 \mathrm{~mol} \mathrm{~N}_{2} \mathrm{O}_{5} c. 15.2 g N2O515.2 \mathrm{~g} \mathrm{~N}_{2} \mathrm{O}_{5} b. 6.8 mol N2O36.8 \mathrm{~mol} \mathrm{~N}_{2} \mathrm{O}_{3} d. 2.87 kgN,O2.87 \mathrm{~kg} \mathrm{N,O}

Studdy Solution
a. 5.0 mol NO25.0 \text{ mol NO}_2 b. 13.6 mol NO213.6 \text{ mol NO}_2 c. 0.282 mol NO20.282 \text{ mol NO}_2 d. 53.14 mol NO253.14 \text{ mol NO}_2

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