The following thermochemical equation is for the reaction of bromine trifluoride(g) to form bromine(g) and fluorine(g)....
The following thermochemical equation is for the reaction of bromine trifluoride(g) to form Br2(g) and fluorine(g) 2BTF3(g) AH = 542 kJ Br2(g) + 3F2(g) How many grams of BrF3(g) would react if 76.7 kJ of energy were provided? grams Submit Answer 1 question attempt remaining
Use the References to access important values if needed for this question. The following thermochemical equation is for the reaction of bromine trifluoride(g) to form Br2(g) and fluorine(g) 23rF3(8) Bra(g) + 3F2(e) AH = 542 kJ How many grams of BrF3(g) would react if 97.0 kJ of energy were provided? Submit Answer 1 question attempt remaining
The following thermochemical equation is for the reaction of hydrogen chloride(g) with ammonia(g) to form ammonium chloride(s). HCI(g) + NH3(g) NH CH) AH = -176 kJ/mol-rxn How many grams of HCI(g) would have to react to produce 51.9 kJ of energy? grams The following thermochemical equation is for the reaction of hydrogen bromide(r) with chlorine() to form hydrogen chloride) and bromine(g) 2HBr(g) + Cl2(g) +2HCl(g) + Brz(8) AH = -81.1 kJ/mol-rxn When 16.4 grams of hydrogen bromide(g) react with excess...
4) Given the thermochemical equations: (3 points) Br2(l) + F2(g) → 2BrF(g) Br2(1) + 3F2(g) → 2BrF3(g) AH°= -188 kJ/mol AH°= -768 KJ/mol Calculate the AH°rxn for the reaction BrF(g) + F2(g) → BrF3(9)
The following thermochemical equation is for the reaction of nitrogen(g) with oxygen(g) to form nitrogen dioxide(g). N2(g) + 2O2(g)2NO2(g) H = 66.4 kJ How many grams of N2(g) would be made to react if 19.5 kJ of energy were provided? grams?
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...
The following thermochemical equation is for the reaction of ammonium chloride(s) to form ammonia(g) and hydrogen chloride(g). NH4Cl(s) NH3(g) + HCl(g) H = 176 kJ How many grams of NH4Cl(s) would be made to react if 49.8 kJ of energy were provided? _____grams
The following thermochemical equation is for the reaction of hydrogen(g) with oxygen(g) to form H2O(g). 2H2(g) + O2(g) 2H2O(g) AH=-484 kJ How many grams of H2(g) would have to react to produce 61.5 kJ of energy? grams
The following thermochemical equation is for the reaction of carbon dioxide(g) with hydrogen(g) to form C2H2(g) and water(g). 2CO2(g) + 5H2(g) C2H2(g) + 4H2O(g) H = 46.5 kJ How many grams of CO2(g) would react if 5.32 kJ of energy were provided?
The following thermochemical equation is for the reaction of iron(III) oxide(s) with hydrogen(g) to form iron(s)and water(g). Fe2O3(s) + 3H2(g)—2Fe(s) + 3H2O(g) AHexn98.8 kJ How many grams of Fe2O3(s) would react if 36.2 kJ of energy were provided? grams Submit Answer