Number of results: 14,917
424 g of Fe is 424/55.85 = 7.59 moles Is that 0.606 g or 606 g of brown oxide? Recheck your numbers. If it is 606 g, then 182 g or 11.38 moles are oxygen atoms. That is a 1.50:1 O/Fe ratio The empirical formula is Fe2O3
Monday, July 23, 2012 at 7:01am by drwls
if 7.o moles of sulfur atoms and 10 moles of oxygen molecules are combined to form the maximum amount of sulfur trioxide, how many moles of which reactant remain unused at the end?
Tuesday, September 4, 2012 at 7:29pm by Anonymous
figure the moles of each reaction gas from PV=nRT solve for n in each case. Then you have a limiting reactants problem moles H2 and Moles O2. In a complete reaction, you should have 2 moles of H2 to each mole of O2. Examine your ration. If it is higher than that, then oxygen ...
Tuesday, October 2, 2012 at 7:50pm by bobpursley
Hassium (III)oxalate contains 2.25 mol of Carbon atoms. What is the number of moles of oxygen atoms in the sample?
Thursday, October 25, 2012 at 10:45pm by Carina
For the following reaction, 0.431 moles of iron are mixed with 0.293 moles of oxygen gas. iron (s) + oxygen (g) iron(II) oxide (s) What is the FORMULA for the limiting reagent
Sunday, April 15, 2012 at 6:18pm by Anonymous
At a pressure of 2.00 atm, a sample of air consists of 0.20 moles of nitrogen, 0.65 moles of oxygen and 0.15 moles of argon. What is the partial pressure of the oxygen?
Tuesday, October 30, 2012 at 12:37pm by Mickeykalle
How many moles of oxygen are required for the combustion of 25.5 g of magnesium?
Monday, November 26, 2012 at 7:22pm by Kat
a quantity of oxygen occupies a volume of 19.2L at STP. How many moles of oxygen are present?
Tuesday, December 4, 2012 at 3:39pm by Gurjot
You have three moles of oxygen and hydrogen. And 1 mol of aluminum as well as one mole of aluminum hydroxide
Monday, December 10, 2012 at 2:10pm by Katie
how do i find the number of moles of oxygen atoms in: Al(OH)3
Monday, December 10, 2012 at 2:10pm by Gurjot
When iron metal reacts with oxygen, the reaction can form Fe2O3. Write a balanced chemical equation for this reaction, and find the number of moles of oxygen that are needed to form 6 mol of Fe2O3. Show your work.
Monday, January 7, 2013 at 4:41pm by Megan
Just having some trouble with this chemistry problem.. Thanks for help! Toxic carbon monoxide (CO) gas is produced when fossil fuels such as petroleum burn without enough oxygen. The CO can eventually be converted to CO2 in the atmosphere. Automobile catalytic converters are ...
Tuesday, January 15, 2013 at 5:17pm by Sara
a. Write the balanced equation for this conversion. 2CO + O2 ==> 2CO2 b. How many moles of oxygen gas would be needed to convert 50.0 mol of carbon monoxide to carbon dioxide? 50.0 mol CO x (1 mol O2/2 mol CO) = ? mol CO2 c. What volume of oxygen gas would be needed to ...
Tuesday, January 15, 2013 at 5:17pm by DrBob222
Calculate the amount of heat required to raise the temperature of 3 moles of oxygen gas from 298 to 400K. Given that C, of O2 is 29.36 Jmole-'K-'. Please show how to do it.
Friday, January 18, 2013 at 4:07am by Dermot
___NH3+___O2->N2+H2O (this is not balanced) how many moles of oxygen react with 0.23 moles of NH3? HOW many moles moles of N2 will be produced when reacted with 5 mol of O2?
Thursday, January 24, 2013 at 6:10pm by tyneisha
Using the equation 2H2 + O2 ==> 2H2O, determine how many grams of water is produced when 13 moles of oxygen is consumed.
Friday, January 25, 2013 at 2:17pm by thad
# of moles of oxygen in 2 L @ 24 deg C & 750 torr?
Monday, January 28, 2013 at 5:10pm by Annie
calculate the # of moles of oxygen in 2 L @ 24 deg C & 750 torr
Tuesday, January 29, 2013 at 1:28pm by Annie
What volume does 0.25 moles of oxygen gas occupy ar STP?
Thursday, January 31, 2013 at 9:27pm by Help!!
In a certain compound of copper and oxygen, a sample weighing 0.5424g contains 0.4831 g of Cu. How many moles of Cu in the sample? How many grams of Oxygen and how many moles of Oxygen are there in the sample? What is the mole ratio of Cu/O in the sample? What is the formula ...
Monday, February 18, 2013 at 8:35pm by Jester21