vessel | volume | temperature | initial rate of reaction |
A | 5.0 L | 1000. oC | 4 |
B | 2.0 L | 1100. oC | 1 |
C | 3.0 L | 1100. oC | 2 |
D | 3.0 L | 1000. oC | 3 |
Explanation
initial rate of reaction is directly proportional to temperature and inversely proportional to volume.
Iron ore is reduced to pure iron by smelting, during which the iron (III) oxide in...
Blast furnaces extract pure iron from the iron(III) oxide in iron ore in a two step sequence. In the first step, carbon and oxygen react to form carbon monoxide: 2C (s) + O2 (g) → 2CO (g) In the second step, iron(III) oxide and carbon monoxide react to form iron and carbon dioxide: Fe2O3 (s) + 3CO (g) → 2Fe (s) + 3CO2 (g) Write the net chemical equation for the production of iron from carbon, oxygen and iron(III) oxide....
Iron (III) oxide reacts with carbon monoxide to produce iron and carbon dioxide. Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Part A What is the percent yield of iron if the reaction of 67.0 g of iron(III) oxide produces 14.3 g of iron?
When 50.1 g iron(III) oxide reacts with carbon monoxide, 31.7 g iron is produced. What is the percent yield of the reaction? Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)
Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) A reaction mixture initially contains 22.90 g Fe2O3 and 15.90 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?
Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) A reaction mixture initially contains 23.00 g Fe2O3 and 15.10 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?
Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) A reaction mixture initially contains 22.55 g Fe2O3 and 15.06 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?
Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) A reaction mixture initially contains 22.85 gg Fe2O3Fe2O3 and 14.26 gg COCO. Once the reaction has occurred as completely as possible, what mass (in gg) of the excess reactant is left? m= ____ g
Iron metal is made from iron ore in a blast furnace, were this chemical reaction occurs: Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g) (a) Is this a redox equation? State why it is or why it is not. (b) If 175 kg of iron ore (Fe2O3) is reacted with excess carbon monoxide (CO), what is the theoretical yield (amount in kg) of iron metal (Fe)? (c) If the actual yield of iron metal is 109 kg, what is the percent...
Iron metal is made from iron ore in a blast furnace, were this chemical reaction occurs: Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g) (a) Is this a redox equation? State why it is or why it is not. (b) If 175 kg of iron ore (Fe2O3) is reacted with excess carbon monoxide (CO), what is the theoretical yield (amount in kg) of iron metal (Fe)? (c) If the actual yield of iron metal is 109 kg, what is the percent...
Iron metal is made from iron ore in a blast furnace, were this chemical reaction occurs: Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g) (a) Is this a redox equation? State why it is or why it is not. (b) If 175 kg of iron ore (Fe2O3) is reacted with excess carbon monoxide (CO), what is the theoretical yield (amount in kg) of iron metal (Fe)? (c) If the actual yield of iron metal is 109 kg, what is the percent...