Mg(s) + 1/2 O2(g) ==> MgO(s) 0000002630 00000 n 0.019 mol B. ! 0000003153 00000 n Steve O. Lv 7. H2+ 1/2O2 -> H2O delta H = -285.8 kJ Using Hess' Law find both the missing delta H values. (s). Ag 2 S(s)-40. Then use the results with Hess's Law to 1 decade ago. Assuming the specific heat of the aqueous Arrange the, I'm trying to calculate the enthalpy of the reaction Mg(s) + 2HCl(aq) -> MgCl2(aq) + H2 (g) however I cannot find the enthalpy of the compound MgCl2 (aq) and I cannot calculate the total enthalpy without it. 1. Calculate the enthalpy for the following reaction: 4 NH3 (g) + 5 O2 (g) into 4 NO (g) + 6 H2O (g). 1) MgO(s) +2HCI(aq)→ MgCl2(aq) +H2O(l) -411. Ag(s) 0. I don’t really understand what you are asking here, but i hope i can sufficiently answer. DIU, 2) Mg(s) + 2HCI(aq) → MgCl2(aq) + H2(g) 401 .08 3) H2(g) + ½O2(g) → H2O(l) e95.8 4) Use your data and Hess' law to calculate AHreaction for: Mg(s) + ½Odg) → MgO(s). 0 + 2(-167.159) -> 0 + 0 The answers seems strange. Delta H2 for eqn 2 is the delta H you measured but since you reversed the equation you want to change the sign. Eqn 3 as is & 0000005155 00000 n 0000002184 00000 n Mg (s) = 2HCl (aq) = MgCl2 + H2 (g) / Data- mass of empty calorimter: 11.19 g, mass of HCl=25.14g, mass of HCl + calorimter:36.33g, mass of Mg: 0.171 g, temp of HCl: 24.9 degrees Celcius, temperature of HCl +Mg =51.6 degrees Celcius. Your Response. Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq) The appropriate data from the short table of standard enthalpies of formation shown below can be used to calculate the value of Δ H o MgO + 2HCl (aq) -> MgCl2+ H2O delta H = ? trailer <<4F67E61BCBFE11DE9659001124D80958>]>> startxref 0 %%EOF 86 0 obj<>stream Respond to this Question. 0000004861 00000 n Mg + 2HCl -> MgCl2 +H2 delta H = ? A] 2Mg(s) + O2(g) -> 2MgO(s) Delta G = -1137 kJ/mol .. B] NH3(g) + HCl(g) -> NH4Cl(s) Delta G = -91.1 kJ/mol ... C] AgCl(s) -> Ag+(aq) + Cl-(aq) Delta G = 55.6 kJ/mol, What is Delta H rxn for the following chemical reaction? Write equn 1 as is/ 203 0. Mg(s) + 2HCl(aq) -> MgCl2(aq) + H2(g) delta H1? 0000003938 00000 n For the reaction , MgO+2HCl-->MgCl2 + H2O moles of Mg = 0.3/24= 0.0125 moles Enthalpy change = (37.43-12.50+0.3)*4.18*(34-24.2)/0.0125 =8. However, we can apply Hess’s law to find the heat of formation for MgO by combining a series of reactions that are much safer and more suitable for a calorimetry experiment. To make these equations add up to the formation reaction of MgO, you will need to include the following: H2(g) + 1/2O2(l) delta H, Mg + 2HCl ----> MgCl2 + H2 What volume of hydrogen at STP is produced from the reaction of 50.0g of Mg and the equivalent if 75g of HCl? temperature of HCl= 24.2 degrees Celcius, temperature of HCl +Mg= Try looking for a table or appendix somewhere in your book to find the standard enthalpies of certain substances. Express the average rate as mol of Mg consumed per minute. The only problem is that when I looked up the thermodynamic values I could not find MgCl2(aq) so would this just be 0? given the thermochemical equations, B2O3 + 3H2O -> 3O2 + B2H6 delta h = -2035 kj H2O -> H2O delta h = 44 kj H2 + 1/2O2 -> H2O delta h = -286 kj 2B + 3H2 -> B2H6 delta h = 36 kj what is the delta hf for 4B + 3O2 -> 2B2O3? Then deltaH3 = -241.8 For the first equation I did © 2003-2020 Chegg Inc. All rights reserved. Calculate the delta H rxn for the following reaction: CH4(g)+4Cl2(g)-->CCl4(g)+4HCl Use the following reactions and given delta H's: 1) C(s)+2H2(g)-->CH4(g) delta H= -74.6 kJ 2) C(s)+2Cl2(g)-->CCl4(g) delta H= -95.7 kJ 3), Classify the following reactions as precipitation reactions, oxidation-reduction reactions, or acid-base reactions.