Calculate the heart of formation for aluminum chloride using the following thermochemical equations:
2Al (s) + 6HCl (aq) ---> 2AlCl3 (aq) + 3H2 (g) . ΔH = -1049 kJ
HCl (g) ---> HCl (aq) . ΔH = -74.8 kJ
H2 (g) + Cl2 (g) ---> 2HCl (g) ΔH = -1845 kJ
AlCl3 (s) ---> AlCl3 (aq) ΔH = -323 kJ
Calculate the heart of formation for aluminum chloride using the following thermochemical equations: 2Al (s) +...
Calculate the enthalpy of decomposition of aluminum chloride in the town 2 AICE() ---> 2Al(s). (g) Use the following four equations: a) 2Al(s) + 6HCl(aq) + 2AICI.(aq) + 3H2(8) AH" --1049 kJ/mol b) HCl(aq) - HC (g) AH':- 74.8 kļ/mol c) H2(g) + Cl:(g) - 2HCI(g) AH", -1845 kJ/mol d) AICI, (s) -- AICI (aq) AH'= -323 kJ/mol
2Al(s) + 3Cl2(8) - 2AICI,(s) AH =? Use the reactions here to determine the AH' for reaction : ® HCI(g) — HCl(aq) AH;, = -74.8 kJ (a) Hz(8) + C1>(- 2HCl(8) AH) = -185 kJ M AICI;(aq) - AICI,(s) AH = +323 kJ/mol M 2Al(s) + 6HCl(aq) - 2AICI,(aq) + 3H2(g) AH = -10:49 J
When aluminum is placed in concentrated hydrochloric acid, hydrogen gas is produced. 2Al(s)+6HCl(aq)⟶2AlCl3(aq)+3H2(g)2Al(s)+6HCl(aq)⟶2AlCl3(aq)+3H2(g) What volume of H2(g)H2(g) is produced when 3.30 g of Al(s) reacts at STP?
Please give the ionic, and net equations and spectator ions of the following molecular equations: 2Al (s) +6HCl (aq) = 2AlCl3(aq) + 3H2 KI (aq) + AgNO3 (aq) = KNO3 (aq) + AgI(s) HCl (aq) + NaOH (aq) = NaCl (aq) + H2O (l) 2HCl (aq) +Na2CO3 (aq) =2NaCl (aq) + CO2(g) +H2O(l)
1.) Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas. 2Al(s) + 6HCl(aq) -> 2AlCl3(aq) + 3H2(g) What mass of H2(g) is required from the reaction of 0.75 g of Al(s) with excess hydrochloric acid? 2.) The reaction of coal and water at a high temperature produces a mixture of hydrogen and carbon monoxide gases. This mixture is known as synthesis gas (or syngas). What mass of water is required for the formation of 175 grams of...
Consider these reactions, where M represents a generic metal. 2M(s)+6HCl(aq)⟶2MCl3(aq)+3H2(g)ΔH1=−600.0 kJ HCl(g)⟶HCl(aq) ΔH2=−74.8 kJ H2(g)+Cl2(g)⟶2HCl(g) ΔH3=−1845.0 kJ MCl3(s)⟶MCl3(aq) ΔH4=−215.0 kJ Use the given information to determine the enthalpy of the reaction 2M(s)+3Cl2(g)⟶2MCl3(s) ΔH= kJ
Consider these reactions, where M represents a generic metal. 2M(s)+6HCl(aq)⟶2MCl3(aq)+3H2(g)Δ?1=−924.0 kJ2M(s)+6HCl(aq)⟶2MCl3(aq)+3H2(g)ΔH1=−924.0 kJ HCl(g)⟶HCl(aq) Δ?2=−74.8 kJHCl(g)⟶HCl(aq) ΔH2=−74.8 kJ H2(g)+Cl2(g)⟶2HCl(g) Δ?3=−1845.0 kJH2(g)+Cl2(g)⟶2HCl(g) ΔH3=−1845.0 kJ MCl3(s)⟶MCl3(aq) Δ?4=−123.0 kJMCl3(s)⟶MCl3(aq) ΔH4=−123.0 kJ Use the given information to determine the enthalpy of the reaction 2M(s)+3Cl2(g)⟶2MCl3(s)
Consider these reactions, where M represents a generic metal 1.) 2M(s)+6HCl(aq) --> 2MCl3(aq)+3H2(g) H=-748.0 kJ 2.) HCl(g) --> HCl(aq) H=-74.8 3.) H2(g)+Cl2(g) --> 2HCl(g) H=-1845 4.) MCl3(s) --> MCl3(aq) H=-317.0 Using the information above to determine the enthalpy of the following reaction 2M(s)+3Cl2(g) --> 2MCl3(s) H=______kJ
Consider the following balanced equation: 6HCl(aq) + 2Al(s) → 3H2(g) + 2AlCl3(s) If 17.3 moles of HCl(aq) and 7.07 moles of Al(s) are allowed to react, and the percent yield is 71.8%, how many moles of AlCl3(s) will actually be produced?
When aluminum is placed in concentrated hydrochloric acid, hydrogen gas is produced. 2Al(s)+6HCl(aq)⟶2AlCl3(aq)+3H2(g) What volume of H2(g) is produced when 3.90 g Al(s) reacts at STP?