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Be sure to answer all parts. Consider the following balanced thermochemical equation for the decomposition of...
Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3(s) -...
Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3(s) - MgO(s) + CO2(g) AHrxn - 117.3 kJ (a) Is heat absorbed or released in the reaction? released o absorbed (b) What is AHfor the reverse reaction? (@) What is AH when 4.20 mol of CO, reacts with excess MgO? kJ (d) What is AH when 30.0 g of CO, reacts with excess MgO?
Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3() – MgO(s)...
Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3() – MgO(s) + CO2(g) AH = 117.3 kJ (a) Is heat absorbed or released in the reaction? released absorbed (b) What is AHrn for the reverse reaction? (c) What is AH when 3.10 mol of CO2 reacts with ercess Mgo? kJ (d) What is AH when 33.5 g of CO, reacts with excess 190? kJ
Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3 (s) LaTeX:...
Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3 (s) LaTeX: \longrightarrow ⟶ MgO (s) + CO2 (g) LaTeX: \Delta Δ Hrxn = 117.3 kJ If MgO is produced this way, how many grams of MgO can form when 1.000 x 103 kJ of heat is transferred? Show your work.
Pb.8. Consider the following balanced thermochenmical equation for the decomposition of the mineral magnesite: MgCOs(s) MgO(s)+CO2(g)...
Pb.8. Consider the following balanced thermochenmical equation for the decomposition of the mineral magnesite: MgCOs(s) MgO(s)+CO2(g) AHn 117.3 kJ a) Is heat absorbed or released in the reaction? b) What is AHnn for the reverse reaction? c) What is AH when 5.35 mol of CO2 reacts with excess MgO? d) What is AH when 35.5 g of CO2 reacts with excess MgO? Page 3 of 4 CHE 120 Pb.9. Liquid hydrogen peroxide, an oxidizing agent used in many rocket fuel...
CHE 120 Pb.3. A 295- aluminum engine part at an initial temperature of 13.00'C absorbs 75.0...
CHE 120 Pb.3. A 295- aluminum engine part at an initial temperature of 13.00'C absorbs 75.0 kJ of heat. What is the final temperature of the part? (Specific heat capacity of Al = 0.900 Jig K). Pb.4. When 155 mL of water at 26°C is mixed with 75 mL of water at 85°C, what is the final temperature? (Assume no heat lost to the surroundings; density of water = 1.00 g/mL and specific heat capacity of water = 4.184 J/g.K)....
Be sure to answer all parts. Consider the following balanced thermochemical equation for a reaction sometimes...
Be sure to answer all parts. Consider the following balanced thermochemical equation for a reaction sometimes used for H2S production: =Sg(s) + H2(g) → H2S() AH rxn = -20.2 kJ his an exothermic or endothermic reaction? endothermic exothermic (b) What is AH rxn for the reverse reaction? KJ (c) What is AH when 3.10 mol of Sg reacts? kJ
Be sure to answer all parts. Consider the following balanced thermochemical equation for a reaction sometimes...
Be sure to answer all parts. Consider the following balanced thermochemical equation for a reaction sometimes used for H,S production: (BH-H+ (a) Is this an exothermic or endothermic reaction? AH--20.2kJ endothermic exothermic (b) What is AH for the reverse reaction? kJ (c) What is AH when 4.30 mol of Ss reacts? kJ draw HIR < Prey 10 of 16 Ne: hp
1 attempt left. please do with perfection 1 attempts left Check my work Be sure to...
1 attempt left. please do with perfection
1 attempts left Check my work Be sure to answer all parts. Magnesia ( MgO) is used for fire brick, crucibles, and furnace linings because of its high melting point. It is produced by decomposing magnesite (MgCO3) at around 1200°C. (a) Write a balanced equation for the magnesite decomposition being sure to include states for the species. MgCO3 (5) MgO(s) +CO2(g) (6) Use AH° and Asº to find Agº at 298 K. 65.2...
The following thermochemical equation is for the reaction of ammonium nitrate(s) to form dinitrogen monoxide(g) and...
The following thermochemical equation is for the reaction of ammonium nitrate(s) to form dinitrogen monoxide(g) and water(g) NH,NO3() N2O(g) + 2H2O(g) AH = -35.9 kJ How many grams of NH NO,(s) would have to react to produce 12.1 kJ of energy? grams The following thermochemical equation is for the reaction of hydrogen sulfide(g) with oxygen(g) to form water(g) and sulfur dioxide(g). 2H2S(g) + 302(g)—2H2O(g) + 2802(8) AH=-1.04x109 kJ When 9.64 grams of hydrogen sulfide(g) react with excess oxygen(g), -588.8 kJ...
Be sure to answer all parts. When 1 mol of NO(g) forms from its elements, 90.29...
Be sure to answer all parts. When 1 mol of NO(g) forms from its elements, 90.29 kJ of heat is absorbed. (a) Write a balanced thermochemical equation. (Include phases in your equation.) (b) What is AH when 4.02 g of NO decomposes to its elements? kJ
Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3(s) - MgO(s) + CO2(g) AHrxn - 117.3 kJ (a) Is heat absorbed or released in the reaction? released o absorbed (b) What is AHfor the reverse reaction? (@) What is AH when 4.20 mol of CO, reacts with excess MgO? kJ (d) What is AH when 30.0 g of CO, reacts with excess MgO?
Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3() – MgO(s) + CO2(g) AH = 117.3 kJ (a) Is heat absorbed or released in the reaction? released absorbed (b) What is AHrn for the reverse reaction? (c) What is AH when 3.10 mol of CO2 reacts with ercess Mgo? kJ (d) What is AH when 33.5 g of CO, reacts with excess 190? kJ
Pb.8. Consider the following balanced thermochenmical equation for the decomposition of the mineral magnesite: MgCOs(s) MgO(s)+CO2(g) AHn 117.3 kJ a) Is heat absorbed or released in the reaction? b) What is AHnn for the reverse reaction? c) What is AH when 5.35 mol of CO2 reacts with excess MgO? d) What is AH when 35.5 g of CO2 reacts with excess MgO? Page 3 of 4 CHE 120 Pb.9. Liquid hydrogen peroxide, an oxidizing agent used in many rocket fuel...
CHE 120 Pb.3. A 295- aluminum engine part at an initial temperature of 13.00'C absorbs 75.0 kJ of heat. What is the final temperature of the part? (Specific heat capacity of Al = 0.900 Jig K). Pb.4. When 155 mL of water at 26°C is mixed with 75 mL of water at 85°C, what is the final temperature? (Assume no heat lost to the surroundings; density of water = 1.00 g/mL and specific heat capacity of water = 4.184 J/g.K)....
Be sure to answer all parts. Consider the following balanced thermochemical equation for a reaction sometimes used for H2S production: =Sg(s) + H2(g) → H2S() AH rxn = -20.2 kJ his an exothermic or endothermic reaction? endothermic exothermic (b) What is AH rxn for the reverse reaction? KJ (c) What is AH when 3.10 mol of Sg reacts? kJ
Be sure to answer all parts. Consider the following balanced thermochemical equation for a reaction sometimes used for H,S production: (BH-H+ (a) Is this an exothermic or endothermic reaction? AH--20.2kJ endothermic exothermic (b) What is AH for the reverse reaction? kJ (c) What is AH when 4.30 mol of Ss reacts? kJ draw HIR < Prey 10 of 16 Ne: hp
1 attempt left. please do with perfection
1 attempts left Check my work Be sure to answer all parts. Magnesia ( MgO) is used for fire brick, crucibles, and furnace linings because of its high melting point. It is produced by decomposing magnesite (MgCO3) at around 1200°C. (a) Write a balanced equation for the magnesite decomposition being sure to include states for the species. MgCO3 (5) MgO(s) +CO2(g) (6) Use AH° and Asº to find Agº at 298 K. 65.2...
The following thermochemical equation is for the reaction of ammonium nitrate(s) to form dinitrogen monoxide(g) and water(g) NH,NO3() N2O(g) + 2H2O(g) AH = -35.9 kJ How many grams of NH NO,(s) would have to react to produce 12.1 kJ of energy? grams The following thermochemical equation is for the reaction of hydrogen sulfide(g) with oxygen(g) to form water(g) and sulfur dioxide(g). 2H2S(g) + 302(g)—2H2O(g) + 2802(8) AH=-1.04x109 kJ When 9.64 grams of hydrogen sulfide(g) react with excess oxygen(g), -588.8 kJ...
Be sure to answer all parts. When 1 mol of NO(g) forms from its elements, 90.29 kJ of heat is absorbed. (a) Write a balanced thermochemical equation. (Include phases in your equation.) (b) What is AH when 4.02 g of NO decomposes to its elements? kJ
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