The first step in the industrial recovery of zinc from the zinc sulfide ore is roasting, that is, the conversion of ZnS to ZnO by heating: 2ZnS(s) + 3O2(g) → 3ZnO(s) + 2SO2(g) ∆H = –879 kJ/mol Calculate the heat evolved (in kJ) per gram of ZnS roasted.
Zinc sulfide reacts with oxygen according to the reaction: 2ZnS(s)+3O2(g)→2ZnO(s)+2SO2(g) A reaction mixture initially contains 4.8 mol ZnS and 7.5 molO2. Part A Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?
Zinc sulfide reacts with oxygen according to the reaction: 2ZnS(s)+3O2(g)→2ZnO(s)+2SO2(g) A reaction mixture initially contains 4.6 mol ZnS and 9.4 mol O2. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains? Express your answer using two significant figures.
TC05ЕОЗ Use the enthalpies of formation given in the table below to calculate the standard molar enthalpy change for this reaction at 298K: 2ZnS(s) 302(g) 2ZnO(s) + 2SO2(g) Att / kJ mol at 298K, standard state 1 bar, Substance ZnO(s) -350 SO2(g) -297 ZnS(s) -206 Select one: a. -441 kJ mor1 b. -853 kJ mol1 c. +882 kJ mol 1 d. +441 kJ molr1 e. -882 kJ mol1 TСОЗЕОЗ A chemical reaction carried out at an ambient pressure of 1.02...
For the balanced equation shown below, how many moles of O2 be produced by 0.7236 moles of ZnS? 2ZnS(s) + 3O2 (g) --> 2ZnO(s) + 2SO2 (g)
3) The first step in the industrial recovery of zinc from the zinc sulfide ore is roasting that is conversion of ZnS to ZnO by heating: 2ZNS(s)+ 302[g)2ZnO(s) + 2S02(g) AH--879 KJ/mol Calculate the heat evolved (in KJ) per gram of ZnS roasted. (3 points) 4) Given the thermochemical equations: (3 points) AHO-188 KJ/mol AH-768 KJ/mol Br2)+ F2g) 2BrF(g) Br2)+3F2(g) 2BrF3(g) Calculate the AHm for the reaction BrF(g)+ F2(g) BrF3(g)
13. The burning of 80.3 g of SiH4 at constant pressure gives off 3790 kJ of heat. Calculate AH for this reaction. SiH4(g) + 2 02(g) → SiO2(s) + 2 H2O(1) A) -1520 kJ/mol rxn B) - 47.2 kJ/mol rxn C) - 4340 kJ/mol rxn D) -2430 kJ/mol rxn E) + 4340 kJ/mol rxn
A metal object at 54.0 oC is heated by gaining 30.2 kJ of heat from the environment. The heat capacity, C, of the metal object is 6.30 kJ/ oC When 11.53 g C2H6O (g) is reacted according to the following equation, 368 kJ of heat is released. What is the ΔH of the reaction? C2H6O (g) + 3O2(g) --> 2CO2(g) + 3H2O (l) When 2.45 g of CH3OCH3 is burned at constant Pressure, 77.42 kJ of heat is given off. What is...
Given: C(s) + O2(g) ---> CO2(g) ΔH = −393.5 kJ/mol S(s) + O2(g) ---> SO2(g) ΔH = −296.8 kJ/mol C(s) + 2S(s) ---> CS2(ℓ) ΔH = +87.9 kJ/mol A) Calculate the standard enthalpy change for the following reaction CS2(ℓ) + 3O2(g) ---> CO2(g) + 2SO2(g) ΔH° rxn = -1075 kJ/mol B) Using the equation and standard enthalpy change for the reaction (from part A), calculate the amount of heat produced or consumed when 3.2 mol of CS2 reacts with excess...
Calculate AH° at 25°C for the reaction below.oceano 2ZnS() + 30,(g) +2ZnO(s) + 250,() -206.0 0 -350.5 –296.8 AH; (kJ/mol)