Question

NAME: 1. For the balanced reaction between nitrogen gas and hydrogen gas to produce ammonia gas: N, (g) + 3H2(g) - 2NH, (g) P= 540 torr V=425 ml T= 31 C P= 1.10 atm V1.15 L T = 23C a. For the given starting reactant values, determine the limiting and excess reactants and show your reasoning. Calculate the theoretical yield of NH3(g) in mol and gram terms. c. Determine the volume of this NH, (g) in liters at STP conditions. 2. Using the appendix tables in your textbook for standard heats of formation, calculate the standard enthalpy change, AH, for the following balanced reaction. 4HF (g) ----à SiF. (g) + Sio, (s) + 2H,0 (g)

Answer 1

Nag! 3H2(g) ) Inhala 40403 pp10nm 425 m2 V-1015L T IC -230 = 396K *21340-3046 - no. of moles of Na = PV ART : 540 foyd X 0.4251 ent. 62:36 LTow kinol 'x 304k. 1220012 mal No. of moles of H2 = 1. loatmo.0820 Latim -- 296.6 x kmor 0.001154 1225.24.10-5 Ratio of moles of N2: 142. moles of H2 = 3N2 - = 3.80.01220.036 But we have 0.000052 moles of H2 so , Ha is limited. and Nz is excess reactants. (b) Theenitical field of NH3__ 2 0.0000 13mails 3.3.46X10no-les

Mass of 113.2 molesx_mola mass = 3.46X105717 3 5. 89.810- volume of NH3 at STP V = nRT = 5.46x10 - 273.1568 Latm- o S - 3-46X10-05x273.150.08.20Z = 0.000774L = 0.7749 ML S:000) + 496g) - Sifu (g) +2H20lgi. LAH= d.Hf (Sify) +2014 (11.2012 ---DH (S102) - Y0H(142 = = -1615 + 2(-241.818) -(-910.862 -46-213.32 -1615 - 483.6379/0.86 +1023.2 -94.57 kJ/mol