Question

1. A sample of iron is reacted with excess hydrochloric acid and the hydrogen is collected in a 10.L flask at 25°C, where it exerts 73 torr of pressure. What was the mass, in grams, of the iron that was dissolved in the HCl? Fe(s) + 2HCl(aq) --> FeCl2(aq) + H2(g)

2. Nitrogen monoxide reacts with oxygen to produce nitrogen dioxide in the reaction shown below. If you mix oxygen and nitrogen monoxide at the correct stoichiometric ratio, and both gases are at the same temperature and pressure, what volume of gas would you need to completely react with 250 ml of NO, and how much NO₂ will be produced? 2 NO_(g) + O_{2 (g)} --> 2NO_{2 (g)}

Answer 1

760 @ Step 1: Calculation of moles of H2 gas. V=104 T = 25°c - 25+ 273 - 298k. P= 73 Toro = 73 atm = 0.096 atm R=0.0821 Lit-atm = ? PV = nRT = P = 0.096 X 10 = 0.039 RT 0.0821x298 Stop I: Calculation of moles of iron (mass of ison) Iron reacts with Hy by the equation Fe (s) + 2 Hd (aq) Feda (aq) + H₂ (9) from the equation For 1 mole ison 0.039 mol H2 1 mol H₂ is formed 0.089 moles of iron requires mass of iron = moles x Atwt a fe = 0.039x56 = 2.19 g. Given reaction is 2NO (9) + O2(9) 2002 (9) from the eg. 2 - 1 - 2 Given 250 -? – By taking the same 250 ratio) P = 250 125 250 . Volume of O₂ required = 125 ml voly me a No₂ formed - 250 ml 250