Question 14 of 20 Submit Using the provided table, determine the enthalpy for the reaction 2...
Question 41 of 50 Submit Using the provided table, determine the enthalpy for the reaction 2 K(s)+2 H20() H2(g) 2 KOH (aq) AHi (kJ/mol) Substance K (s) 0 НаО () -285.8 КОН (ag) -482.4 kJ/mol 1 2 3 4 5 6 С 8 +- 0 x 100 O 7
Question 14 of 14 Submit Using the provided table, determine the enthalpy for the reaction 2 NHs (g) 3 N2O (g) - 4 N2 (g) +3 H2O (I) Днғ (kJ/mo) Substance NH3 (g) -46.2 N2O (g) 81.6 N2 (g) 0 НаО () -285.8 kJ/mol х 1 2 4 5 6 с 7 8 +- 0 x 100 Tap here or pull up for additional resources 32
Question 43 of 50 Submit Using the provided table, determine the enthalpy for the reaction 2 NH3(g) + 3 N20 (g) - 4 N2 (9) + 3 H2O (1) Substance AH (kJ/mol) NH3 (9) -46.2 N20 (g) 81.6 N2 (9) kJ/mol 1 2 3 C +/- : 0 x 100
Question 16 of 20 Submit Using the provided table, determine the enthalpy for the reaction C3H2 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g) Substance AHF (kJ/mol) C3H8 (9) -108.4 O2 (9) CO2 (g) -393.5 H2O (9) -241.8
Question 42 of 50 Submit Using the provided table, determine the enthalpy for the reaction C(s) + CO2(g) – 2 CO (9) Substance AH (kJ/mol) C (s) 0 CO2 (g) -393.5 kJ/mol 1 2 3 C +/- : 0 x 100
Question 14 0414 Using the provided table, determine the enthalpy for the reaction 2 NH3 (g) + 3 N20 (g) - 4 N2 (g) + 3 H20 (1) Substance AHI (kJ/mol) NH3(g) -46.2 N20 (9) 81.6 N2 (9) 0 kJ/mol
(6 pts.) Using Hess’s Law and the values for Standard Enthalpies of Formation from the table provided, calculate the enthalpy of reaction ΔH°rxn (in kJ) for each of the following reactions: Standard Enthalpies of Formation substance ΔHf° in kJ/mol Mg(s) 0 MgO(s) -601.6 HCl(aq) -167.2 MgCl2(aq) -801.2 H2(g) 0 H2O(l) -285.8 Reaction #1: Mg (s) + 2HCl (aq) è MgCl2 (aq) + H2 (g) Reaction #2: MgO (s) + 2HCl (aq) è MgCl2 (aq) + H2O (l) 2. (4 pts.)...
The following table lists some enthalpy of formation values for selected substances. Substance ΔfH∘ΔfH∘ (kJ mol−1)(kJ mol−1) CO2(g)CO2(g) −393.5−393.5 Ca(OH)2(s)Ca(OH)2(s) −986.1−986.1 H2O(l)H2O(l) −285.8−285.8 CaCO3(s)CaCO3(s) −1207−1207 H2O(g)H2O(g) −241.8−241.8 Part A: Determine the enthalpy for this reaction: Ca(OH)2(s)+CO2(g)→CaCO3(s)+H2O(l) C a ( O H ) 2 ( s ) + C O 2 ( g ) → C a C O 3 ( s ) + H 2 O ( l ) Express your answer in kJ mol−1 k J m o l...
Part A Determine the enthalpy for this reaction: Ca(OH)2(s)+CO2(g)→CaCO3(s)+H2O(l) Express your answer in kilojoules per mole to one decimal place. ΔHrxn∘= kJ/mol Part B Consider the reaction Ca(OH)2(s)→CaO(s)+H2O(l) with enthalpy of reaction ΔHrxn∘=65.2kJ/mol What is the enthalpy of formation of CaO(s)? Express your answer in kilojoules per mole to one decimal place. ± Enthalpy Enthalpy H is a measure of the energy content of a system at constant pressure. Chemical reactions involve changes in enthalpy, ΔH, which can be measured...
Complete questions 2-4 using data from table and the answer from question 1 Measuring Enthalpy Results NaHCO3(s) + HC2H3O2(aq) à NaC2H3O2(aq) + H2O(l) + CO2(g) Trial 1 Trial 2 mass of baking soda(NaHCO3) added 5.4g 5.4g mass of vinegar added 20ml 20ml Final temperature, tf 16.7C 16.7°C Initial temperature, ti 21.1°C 21.1°C Change in temperature, ∆t 4.4°C 4.4°C q (water) = mwCwTw 467.6 J 467.6 J q(reaction) -467.6 J -467.6 J moles of NaHCO3 .0642 .0642 ΔH (kJ/mol) -7.27448 kJ/mol...