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![3 clance equation AH = -943.2 kJ 2 Pt203 mor of Pt₂ oz = 302 + 4 pt man = 2.481x1029 [img=1039] MW 438.115 g/mol 0.5 6 8 mol](http://img.homeworklib.com/questions/a5ce0e80-d854-11eb-a56c-fdcf3a02ee5e.png?x-oss-process=image/resize,w_560)
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Determine the amount of heat, in kJ,...
5. Heat of Reaction under standard conditions : Determine the amount of heat (in kJ) given...
5. Heat of Reaction under standard conditions : Determine the amount of heat (in kJ) given off, when 1.26 x 104 g of ammonia ( NH3 ) are produced according to the equation : N2 (g) + 3 H2 (g) → 2 NH3 (g) ....... AH ºrx = - 92.6 kJ Assume that the reaction occurs at Standard State conditions at 25 C. ANSWER : Total Heat Given Off: _ (units ?) 6. Standard Enthalpy of Formation and Reaction :...
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...
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) -...
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?
Given the balanced chemical equation, 2 H(g) → H2(g) ΔH0rxn = −436 kJ/mol Determine the mass...
Given the balanced chemical equation, 2 H(g) → H2(g) ΔH0rxn = −436 kJ/mol Determine the mass (in grams) of H(g) produced when 823 kJ of heat is released.
Be sure to answer all parts. Consider the following balanced thermochemical equation for the decomposition of...
Be sure to answer all parts. Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3(s) - MgO(s) + CO2(g) AH - 117.3 kJ (a) Is heat absorbed or released in the reaction? absorbed released (b) What is A n for the reverse reaction? -1173 EJ (c) What is AH when 5.20 mol of CO, reacts with excess Mgo? (a) What is AH when 32.5 g of CO, reacts with exces: Mgo?
1. Calculate the quantity of heat released when 8.Sg of hydrogen peroxide decomposes, given: atomic weights...
1. Calculate the quantity of heat released when 8.Sg of hydrogen peroxide decomposes, given: atomic weights 0=16, and H= 1. Hydrogen peroxide decomposes to water and oxygen according to the reaction: H = -196KJ 2. Given the speclflc heat, c,, of water Is 4.18 J/g 0c,how much heat Is needed to warm 200g of water from 22°c to 98°C? q=mC,AT 3. If 20.9KJ of heat were added to 250g of liquid water, how much would its temperature Increase? (Use 4.18 J/goc...
determine the amount of heat (in kj) given off when 4.53 * 10^4 g of ammonia...
determine the amount of heat (in kj) given off when 4.53 * 10^4 g of ammonia is produced according to the equation below. assume that the reaction takes place under standard - state conditions at 25 celsius. N2(g) + 3H2(g) ---> 2NH3 ?H= -92.6 kJ/mol enter the answser in scientific notation
Be sure to answer all parts. Determine the amount of heat (in kJ) associated with the...
Be sure to answer all parts. Determine the amount of heat (in kJ) associated with the production of 1.51 x 104 g of ammonia according to the following equation. N2(g) + 3H2(g) —>2NH3 AH9rxn=-92.6 kJ Assume that the reaction takes place under standard-state conditions at 25°C. Enter your answer in scientific notation. *10 kJ
. Use the equation below to calculate how much heat (in kJ) is evolved when 5.0...
. Use the equation below to calculate how much heat (in kJ) is evolved when 5.0 g of aluminium reacts with a stoichiometric amount of Fe2O3? 2 Al (s) + Fe2O3 (s) —>2 Fe (s) + Al2O3 (s) AH° = -852 kJ Determine the AHPrxn for the following reaction. {AH® (NH3) = -45.9 kJ/mol; AH°(O2) = 0; AH® (NO) = +91.3 kJ/mol; AH° (H2O) = -241.8 kJ/mol; 4 NH3 (g) + 5 O2 (g) — 4 NO (g) + 6...
5. Heat of Reaction under standard conditions : Determine the amount of heat (in kJ) given off, when 1.26 x 104 g of ammonia ( NH3 ) are produced according to the equation : N2 (g) + 3 H2 (g) → 2 NH3 (g) ....... AH ºrx = - 92.6 kJ Assume that the reaction occurs at Standard State conditions at 25 C. ANSWER : Total Heat Given Off: _ (units ?) 6. Standard Enthalpy of Formation and Reaction :...
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...
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) - 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?
Be sure to answer all parts. Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3(s) - MgO(s) + CO2(g) AH - 117.3 kJ (a) Is heat absorbed or released in the reaction? absorbed released (b) What is A n for the reverse reaction? -1173 EJ (c) What is AH when 5.20 mol of CO, reacts with excess Mgo? (a) What is AH when 32.5 g of CO, reacts with exces: Mgo?
Be sure to answer all parts. Determine the amount of heat (in kJ) associated with the production of 1.51 x 104 g of ammonia according to the following equation. N2(g) + 3H2(g) —>2NH3 AH9rxn=-92.6 kJ Assume that the reaction takes place under standard-state conditions at 25°C. Enter your answer in scientific notation. *10 kJ
. Use the equation below to calculate how much heat (in kJ) is evolved when 5.0 g of aluminium reacts with a stoichiometric amount of Fe2O3? 2 Al (s) + Fe2O3 (s) —>2 Fe (s) + Al2O3 (s) AH° = -852 kJ Determine the AHPrxn for the following reaction. {AH® (NH3) = -45.9 kJ/mol; AH°(O2) = 0; AH® (NO) = +91.3 kJ/mol; AH° (H2O) = -241.8 kJ/mol; 4 NH3 (g) + 5 O2 (g) — 4 NO (g) + 6...
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