CO will react with 1.75 moles of Fe2O3?
no it wont sorry i dont know the answer but i tried it and it didnt work for it
How many moles of carbon monoxide (CO) are required to react completely with 1.75 moles of iron (III) oxide (Fe2O3)?
The chemical reaction is: Fe2O3 + 3 CO = 2 Fe + 3 CO2 5,25 moles of carbon monoxide are needed.
If 4.00 kg of Fe2O3 are available to react how many moles of CO are needed and how many moles of each product are formed?
mass / molar mass molar mass Fe2O3 = 159.69 g/mol mass Fe2)3 = 4.00 kg = 4000 g moles = 4000 g / 159.69 g/mol = 25.05 moles Fe2O3 The balanced equation tells you that 1 mole Fe2O3 requires 3 moles CO to react So 25.05 moles needs (3 x 25.05) moles CO = 75.15 moles Co is needed to react 4.00 kg Fe2O3 = 75.2 mol (3 sig figs) b) The equation tells you… Read More
1.5 mole, because 4.5 moles CO need 4.5 moles O atoms from [ 4.5 (mole O) / 3 (mole O/mole Fe2O3) ] = 4.5/3 = 1.5 mole Fe2O3 to become 4.5 moles CO2
There are several different possible reactions of Fe2O3 with CO, depending on temperature and ratio of reactants. The simplest is probably Fe2O3 + CO ==>2FeO + CO21.00 Kg x 1000 g/Kg x 1 mole Fe2O3/160 g = 6.25 moles Fe2O3 moles CO2 produced = 6.25 moles CO2 Volume CO2 at STP = 6.25 moles x 22.4 L/mole = 140 Liters
Depict moles eg: Fe2O3(s) + 3CO(g)--> 2Fe(s) + 3CO2(g) 1 mole of Fe2O3 4 moles of CO 2 moles of Fe 3 moles of CO2
How many moles of carbon monoxide are needed to react with .500 mol of Iron III oxide to produce iron metal and carbon dioxide?
The reaction equation for the production of iron and carbon dioxide is Fe2O3 + 3 CO = 2 Fe + 3 CO2. This means that for 1/2 mole of rust, 1.5 moles of CO is needed.
Theoretically you need 2,527 g carbon. Fe2O3 + 3 C = 3 CO + 2 Fe
the answer you seek is , the limiting reagent is Co, and 8.0mol Fe will be formed!
The needed amount of carbon monoxide is 68,4 g.
160...cant quite grasp HOW though
What is the answer to the following Starting with 3.60 moles of CO calculate the number of moles of CO2 produced if there is enough oxygen gas to react with all of the CO?
Knowing what the answer options are is important for a person to know which is correct. It would be helpful to provide the answer choices as well.
1,4 moles of CO are produced.
How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 53.6 moles of water vapor?
Equation. CO2 + H2 - CO + H2O all one to one, so you need 53.6 moles of hydrogen gas
4,54 L of CO have 0,182 moles.
500 grams of CO is the equivalent of 17,85 moles.
well translate that into the formulas and you have Fe2O3 + CO -> Fe + CO2 two irons on left, one iron on right. so balance the irons Fe2O3 + CO -> 2 Fe + CO2 now... balance the O.. you have 4 O on the left and 2 on the right Fe2O3 + CO -> 2 Fe + 2 CO2 but the carbons arent balanced... sooo make CO and CO2 both 3 Fe2O3 +… Read More
CO is form in high temperatures. 10 moles will form by 5 O2 moles.
Fe2O3(s) + 3CO(g) = 2Fe(s) + 3CO2(g) where (s) = solid, (g) = gas
How many molecules of carbon monoxide are needed to react with excess iron (III) oxide to produce 11.6 g of iron?
The chemical reaction is: Fe2O3 + 3 CO = 2 Fe + 3 CO2 The answer is 1,876.10 ex.23 CO molecules.
How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 30.6 moles of water vapor?
CO2 + H2 -> CO + H2O one to one here 30.6 moles H2O (1 mole H2/1 mole H2O) = 30.6 moles Hydrogen gas needed
2,55 moles of the compound CO have 71,4 grams.
382 g Co contain 6,482 moles.
How many moles of atoms are contained in 382 g Co
How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 65.1 moles of water vapor?
Balanced equation. ( this is a equilibrium reaction ) H2 + CO2 >< H2O + CO this is one to one, so 65.1 moles is the answer. 65.1 mols H2O (1mol H2/1mol H2O ) = 65.1 moles H2
An alternative method for preparing pure iron from fe2o3 is by reaction with carbon monoxide fe2o3 plus co fe plus CO2 unbalanced a balance the equation use the lowest possible coefficients?
Fe2O3 + 3CO -----> 2Fe + 3CO2
The answer is 6,482 moles.
I think that the reaction of CO is with the oxide Fe2O3.
A reaction is: Fe2O3 + 3 CO = 2 Fe + 3 CO2
The reaction is: 2 C + O2 = 2 CO So 2,1 moles are obtained.
How many grams of Co are there in a sample of Co that contains the same number of moles as a 45.6 gram sample of Cr?
The atomic weight of Cr is 52.0 g/mol 1. Convert grams of Cr to moles of Cr: moles Cr = 45.6 g Cr1 mol = 0.877 mol Cr52.0 g Multiply by moles per gram. Grams cancel out. The atomic weight of Co is 58.9 g/mol 2. To convert 0.877 moles of Co to grams of Co: grams Co = 0.877 mol Co58.9 g = 51.7 g Co 1 mol Multiply by grams per mole. Moles… Read More
The reaction is: 2 C + O2 = 2 CO 1,7 moles of carbon monoxide are obtained.
26,3 g cobalt is equivalent to 0,446 moles.
1 mole Co = 58.93320 grams (atomic weight from periodic table in grams) 118g Co x 1mol/58.93320g = 2.00 moles Co
What volume of 0.2500 M cobalt III sulfate is required to react completely with 25.00 ml of 0.0315 M calcium hydroxide?
Co2(SO4)3 + 3Ca(OH)2---> 2Co(OH)3+ 3CaSO4 Co Sulfate and Ca hydroxide react in 1:3 ratio. Moles of Ca Hydroxide=0.0007875mol Moles of CoSulfate needed=0.002625 Volume=1.05
1,4 moles carbon monoxide are produced.
0,83moles glucose are burned.
How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 19.1 moles of water vapor?
38.2 moles . Co2 +2H2 --->2H20 + c Added: The above is incorrect and based on the improper balanced equation. H2 + CO2 -> H2O + CO All one to one and the answer is 19.1 moles H2 needed. Carbon monoxide release is why you will never see this reaction in a school lab.
1 mole CO = 28.00101g CO 14g CO x 1mol CO/28.00101g CO = 0.50 mole CO
C + O2 --> CO 3CO + Fe2O3 --> 2Fe + 3CO2
The equivalence is 1992 moles.
350 g sample of CO contain 12,49 moles.
For this you need the atomic (molecular) mass of CO. Take the number of grams and divide it by the atomic mass. Multiply by one mole for units to cancel. 4.5 grams / 28.0 grams = .161 moles CO
1 mole Co = 58.933g Co (atomic weight in grams) 1 mole Co atoms = 6.022 x 1023 atoms Co Convert grams Co to moles Co. 22.6g Co x (1 mole Co/58.933g) Co = 0.383 mole Co Convert mole Co to atoms Co. 0.383 mole Co x (6.022 x 1023 atoms Co/1 mole Co) = 2.31 x 1023 atoms Co
A mixture of 0.220 moles of CO 0.350 moles H2 and 0.640 moles He has a total pressure of 2.95 Atm what is the pressure of H2?
The partial pressure of the hydrogen will be 0.853 atmospheres.
How many moles of carbon are needed to react with 5.44 mole so 2 in the reaction 5 c plus 2 so 2 arrow cs 2 plus 4 co?
5C + 2SO2 >> CS2 +4CO 5.44 Mol SO2 (5mol C/2mol SO2 ) = 13.6 Moles of Carbon needed.
weight = moles x atomic weight = 7.32 x 58.93 = 431.36 g
The molecular mass of carbon monoxide, CO is 12.0+16.0=28.0 Amount of CO = 1.23/28.0 = 0.0439mol
It is almost balanced, except for 2 moles of CO, so here it is: CO2 + C --> 2 CO