Thefollowingequationdescribestherustingofiron.Note:rustisFe2O3(s)
Fe(s) + O2(g) Fe2O3(s)
a. Balance the above equation.
b. If you start with 100.0 grams of iron, how many moles of iron do you have?
c. If you start with 100.0 grams of rust, how many moles of rust do you have?
d How many moles of rust could be formed from 5.00 moles of iron?
e. How many moles of rust could be formed from 5.00 moles of oxygen?
f. If 50. moles of rust formed, how many grams of rust does this represent?
g. If 10.0 moles of oxygen is consumed in the reaction, how many grams of oxygen was consumed?
Thefollowingequationdescribestherustingofiron.Note:rustisFe2O3(s) Fe(s) + O2(g) Fe2O3(s) a. Balance the above equa...
7. Iron is produced from its ore by the reactions: 2C(s) + O2(g) → 2CO(g) Fe2O3 (s) + 3 CO(g) → Fe(s) + CO2(g) How many moles of O2(g) are needed to produce 4.6 moles of Fe(s)? a. 2.3 b. 3.5 C. 4.6 d. 6.9 e. 13.8
Given the equation, which may or may not be balanced: Fe2O3(s) + CO(g) → Fe(s) + CO2(g) How many grams of Fe could be produced from the complete reaction of 3.196 grams of Fe2O3 with excess CO? grams Fe What is the percent yield of the reaction if only 1.571 grams of Fe are recovered after the reaction has completed? %
Consider the following equation: Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g) How many moles of Fe will be formed from 5.2 moles of CO? Enter only the numeric value for your answer (no units).
Consider the following equation: Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g) How many moles of Fe will be formed from 6.4 moles of CO? Enter only the numeric value for your answer (no units).
b Using the equation: Fe2O3(s) + 3 CO(g) + 2 Fe(s) + 3 CO2(g) How many moles of Fe2O3 are required to produce 45.9 mol of Fe? How many grams of CO are required to produce 45.9 mol of Fe? 1 pt nFe2O3) - mol 1 pt m(CO) -
6) Balance the following equation (1) Fe2O3(s) + CO(g) ® Fe(s) + CO2(g) 7) If 150.0 grams of Fe2O3 react in excess carbon monoxide, what mass of iron will be produced? If in an experiment only 87.9 grams of Fe were recovered, what is the percent yield of this reaction. (5)
Consider the following equation: Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g) How many moles of Fe will be formed from 4.6 moles of CO? Enter only the numeric value for your answer (no units).
Metallic iron can be made by the electrolysis of molten Fe2O3. (a) What mass of Fe is formed by passing a current of 9.15 A through molten Fe2O3 for 4.70 days? The unbalanced chemical reaction representing this electrolysis is shown below. Fe2O3 --> Fe + O2 ____ g of Fe is formed by this electrolysis. (b) How many minutes are needed to plate out 10.00 g of Fe from molten Fe2O3 using 7.29 A current? ____ minutes are needed.
4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) AH = -1652 kJ (a) How much heat is released when 3.54 mol iron are reacted with excess O2? Ok] (b) How much heat is released when 1.48 mol Fe2O3 is produced? CJ) (c) How much heat is released when 2.50 g iron are reacted with excess O2? DJ (d) How much heat is released when 12.6 g Fe and 1.02 g O2 are reacted? CkJ
1) A) If I want to make 225.0 g of Fe, how many grams of C will I need for my experiment? B) If I want to make 225g of Fe, how many grams of Fe2O3 will I need for my experiment? 2) There are 3.00 moles of oxygen gas and 6.00 moles of nitrogen gas in a 10.0 L container at 300K. A) What is the total pressure (in atm) of the gas mixture? B) What is the partial...