Calculate the heat evolved (in kJ) when 1.00 g of ZnS is roasted. The first step

Question

Calculate the heat evolved (in kJ) when 1.00 g of ZnS is roasted. 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: 2 ZnS_(s) + 3 O_2(g) rightwards arrow 2 ZnO_(s) + 2 SO_2(g) H = -879 kJ Calculate the heat evolved (in kJ) when 1.00 g of ZnSs roasted. -4.51 kJ Determine the amount of heat (in kJ) released when 1.26 times 10^4 g of NO_2 are produced according to the equation 2 NO_(g) + O_2 (g) rightwards arrow 2NO_2(g) H = -114.6 kJ This is an exothermic reaction. The amount of heat released is 1.57 times 10^4 kJ. How much heat is evolved when 320 g of SO_2 is burned according to the chemical equation shown below? 2 SO_2(g) + O_2(g) rightwards arrow 2 SO_3(g) capital delta H degree_rxn = -198 kJ This is an exothermic reaction. The amount of heat released is 5.0 times 10^-2 kJ The heat of aluminum is 0.214 cal/g^. degreeC. Determine the energy, in calories, necessary to raise the temperature of a 55.5 g piece of aluminum from 23.0 to 48.6 degree C. 304 cal What is the specific heat of lithium if adding 304 J of energy causes the temperature of a 10.0-g

Explanation / Answer

4) the amount of heat released when 1 gr of ZnS is roasted is:

2ZnS+3O2-----> 2ZnO + 2SO2 heat released = -879KJ

According to balanced equation 2 moles of ZnS = 97.474 gr of ZnS releases -879KJ

1.0 gr of ZnS releases -879KJ/194.94= -4.51KJ of energy

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