Question

5 attempts left Check my work Enter your answer in the provided box. Nitrogen dioxide is used industrially to produce nitric acid, but it contributes to acid rain and photochemical smog. What volume of nitrogen dioxide is formed at 725 torr and 28.2°C by reacting 3.31 cm of copper (d=8.95 g/cm) with 229 mL of nitric acid (d - 1.42 em 68.0% HNO, by mass)? Cu(s) + 4HNO3(aq) + Cu(NO3)2(aq) + 2NO2(8) + 2H20(1) 23.04 10

Answer 1

Equation : Cu + 4HNO —— Cu(NO3), + 2NO, + 2H,0 1 mol Cu 2 mol NO, Amount of Cu(NO3), formed from Cu = 3.31 cm x 8.95g cm 63.55 g 1 mol Cu = 0.932 mol NO, Amount of Cu(NO3), formed from HNQ = 229 mLx1cm x 1.42 g 1 mL cm? = 325.18 g x? 1 mol HNO3, 2 mol NO, 63.02 g 4 mol HNO, = 2.58 mol NO Since Cu limits the production of NO,, Cu acts as the limiting reactant Amount of NO, that can be produced=0.932 mol - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - No of moles of NO,, n = 0.932 mol NO, Pressure of the gas, P = 725 torr Temperature, T = 28.2°C +273 = 301.2K L.torr Gas constant, R= 62.4 K.mol According to ideal gas equation, PV = nRT Volume of the NO, gas, V = (0.932 moi)( 624 En toen) (30126) 725 torr = 24.2 L