@X@user.full_name@X@ @GMU: Using bond energies from the table below, estimate ΔH for the reaction below. The two oxygens in the product are each bound to the carbon. One of the hydrogens is bound to the carbon.H2(g) + CO2(g) → HCOOH(g) Bond Energies, kJ/mol Single Bonds   H C N O S F Cl Br I H 432                 C 411 346               N 386 305 167             O 459 358 201 142           S 363 272 — — 286         F 565 485 283 190 284 155       Cl 428 327 313 218 255 249 240     Br 362 285 243 201 217 249 216 190   I 295 213 — 201 — 278 208 175 149   Multiple Bonds C=C 602 C=N 615 C=O 799 CºC 835 CºN 887 CºO 1072 N=N 418 N=O 607 S=O (in SO2) 532 NºN 942 O2 494 S=O (in SO3) 469

@X@user.full_name@X@ @GMU: From the reaction below, calculate the free energy of formation for CH4(g) at 25°C, if ΔGfo(C3H8(g)) is -23.467 kJ/mol.3CH4(g) → C3H8(g) + 2H2(g) ΔGo = 128.902 kJ/mol

What gas law was used to calculate the answer in question 5?

@X@user.full_name@X@ @GMU: What is the total concentration of ions in a solution consisting of 0.2283 M HClO4?

@X@user.full_name@X@ @GMU: Determine the rate of formation of NH3 if the initial concentration of N2 was 0.4170 M and decreased to 0.3362 M after 0.2474 hours. Use the reaction below.N2(g) + 3 H2(g) → 2NH3(g)

Whose Law is used in Question #16?

  If a given mass of a gas is maintained at a constant temperature, what will decreasing its pressure do?

@X@user.full_name@X@ @GMU: Determine the rate of formation of NH3 if the initial concentration of N2 was 0.4170 M and decreased to 0.3362 M after 0.2474 hours. Use the reaction below.N2(g) + 3 H2(g) → 2NH3(g)

@X@user.full_name@X@ @GMU: ACS-What mass of iron would be plated on an electrode from a solution of Fe(NO3)3 at a current of 5.00 A for 1402.37 s?

@X@user.full_name@X@ @GMU: The density of a particular gas is 3.0431 g/L at 723.02 mm Hg and 35.10 °C. Which gas is it?