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)
For the balanced equation shown below, how many moles of O2 be produced by 0.7236 moles...
Based on the balanced equation below, if 26.1 moles of O2 are used, how many moles of CO2 will be produced? CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
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.
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?
The balanced equation for the detonation of nitroglycerin is shown below. If 10.0 moles of C3H5O9N3 react, how many moles of H2O should form? 4C3H5O9N3() ► 12CO2(g) + 6N2(g) + O2(g) + 10H2O(g) 4.0 180 25 10 2.5 Consider the balanced equation for the following reaction: Pb(s) + 2AgNO3(aq) - Pb(NO3)2(aq) + 2Ag(s) If 7.0 g of lead metal react by the following reaction, what mass of silver metal would we expect to be produced, assuming 100% yield? 3.7 g...
How many moles of water can be produced using 100.0 g of Oxygen, O2? The balanced equation is given as: 4 NH3 +502 — 4 NO + 6H2O 2.00 1.00 2.60 3.75
Consider the balanced chemical equation: 4 Na(s) + O2(g) - 2 Na2O(s) How many moles of Na2O could be produced from 2.18 g of Na? 0.0948 mol 0.0474 mol 4.36 mol 2.00 mol
The "roasting" of 48.7 g of ZnS at constant pressure gives off 220. kJ of heat. Calculate the DH for this reaction.2ZnS(s) + 3O2(g) ® 2ZnO(s) + 2SO2(g)A.) -110 kJ/mol rxnB.) -293 kJ/mol rxnC.) -440. kJ/mol rxnD.) -881 kJ/mol rxnE.) +440. kJ/mol rxn
For the reaction shown, calculate how many moles of each product form when the given amount of each reactant completely reacts. Assume that there is more than enough of the other reactant. 2PbS(s)+3O2(g)→2PbO(s)+2SO2(g) 1) 2.8 mol O2 . . . ? mol PbO 2) ? mol SO2 3) 6.0 mol O2 . . . ? mol PbO 4) ? mol SO2
For the balanced equation shown below, how many grams of C2H3O2Cl will react with 14.5 grams of HCl? 2C2H3O2Cl(g) + 3O2 (g) -->4CO2 (g) + 2H2O(g) + 2HCl (g)
a For the following balanced chemical equation, calculate how many moles of products would be produced if 0.666 mol of the first reactant were to react completely CO (9) + 4H2(g) + CH (9) + 2H, 0(1) mol CH mol H2O b For the following balanced chemical equation, calculate how many moles of products would be produced if 0.441 mol of the first reactant were to react completely. BaCl, (aq) + 2AgNO, (aq) + 2ACI(8) + Ba(NO), (aq) mol AgCI...