4. What is the limiting reactant, theoretical yield, and % yield of iron metal (in kg) if 76.0 kg of Fe2O3 reacts w...
CHEM 100 Meme Avery Meniken DUE Thurs Nox lor Fri Nov 22 Show work with all units, and how your answer (with correct significant figures and its How many MOLES of As) are needed to produce 105 g of Cu in the equation 3CuSO ) +2Al() → C(s) + Al(SO4) () moles A1 hele? Given 10.5gCix ZAL 2. What mass (in grams) of No, is produced when 459 g HNO reacts according to the following balanced equation Cu(e) + 4HNO....
Iron reacts with oxygen at high temperatures to form iron(III) oxide. 4Fe(s)+3O2(g)⟶2Fe2O3(s) Suppose 14.2 g of iron (Fe) is reacted with 18.1 g of oxygen (O2). Select the limiting reagent. Fe2O3 O2O2 FeFe Calculate the theoretical yield of iron(III) oxide (Fe2O3Fe2O3). theoretical yield = The reaction produces 5.40 g of Fe2O3. What is the percent yield of the reaction? percent yield =
Calculate w (in kJ) when 445 g iron (III) oxide (MM = 159.7 g/mol) reacts with excess carbon to produce carbon dioxide gas at 458 K: 2Fe2O3(s) + 3C(s) + 4Fe(s) + 3CO2(g) Answer: 511.64 x
The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product. Consider the reaction: 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) If 16.98 g Fe is mixed with 7.740 g O2, calculate the theoretical yield (g) of Fe2O3 produced by the reaction.
Iron reacts with oxygen to form iron(III) oxide according to the chemical equation below. What is the theoretical yield of product when 5.00 grams of Fe react with excess O2? [Molar masses: Fe, 55.85 g/mol; O, 16.00g/mol] 5 pts 4Fe(s) + 3O2(g) → 2Fe2O3(s)
Question 9 1 pts What is the theoretical yield of iron (55.845 g/mol) when 10.0 g Fe2O3 (159.69 g/mol) reacts with excess carbon (12.01 g/mol)? 2 Fe,03()+3C(5) ► Fe(s)+300,(8) 3.50 g 57.2g 14.3g 6.99 g 1.75 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...
FatA Constants I Periodic Tab Identify the limiting reactant. Mining companies use this reaction to obtain iron from iron ore: Fe2O3 (s) +3CO(g 2Fe(s) +3CO2(g) The reaction of 182 g of Fe2Os with 856 g of CO produces 71.6 g of Fe Fe2Os CO You may want to reference (Pages 299-306) Section 7.5 while completing this problem. Correct More Fe could be formed from the initial mass of Fe2Os than could be formed from the initial mass of moles of...