Chemistry Help! Stoichiometry?
Having trouble with these questions - please help! Solid lithium hydroxide (LiOH) is used in space vehicles to remove exhaled carbon dioxide (CO2). The lithium hydroxide reacts with carbon dioxide to form solid lithium carbonate (Li2CO3) and liquid water. The balanced chemicial equation is given by: 2 LiOH (s) + CO2 (g) --> Li2CO3(s) + H2O (I) a. If only 1 mole of LIOH is available to react with CO2, how many moles of liquid water are produced? Assume that CO2 is not limiting. b. If 3 moles of Li2Co3 are produced, how many grams of LiOH were consumed? c. How many grams of CO2 can be absorbed by 12.50 g of LiOH? Please show your work. Thank you so much!
AP Chemistry Stoichiometry Help?
I have a homework problem I can't get! It's: In a laboratory , 7.52g of Sr(NO3) is dissolved in enough water to form .750L. A .1L sample is withdrawn from this stock solution and addd to a .0425 solution of Na2CrO4. What volume of Na2CrO4 solution is needed to precipitate all the Sr2+ as SrCrO4? Please help me by explaining it! Answers aren't needed, by an outline is please! Also, what are the colors of different precipitates? lead? iodine? Thanks so much! God Bless!
Chemistry: Stoichiometry, HELP!!!?
For all these questions, first write the balanced chemical equation, so you can get the mol ratio. Find the number of moles of each substance that have been given in grams. For that, you need to find the Molar Mass of each substance, by adding up the atomic mass of all the atoms in the compound (or element). 15) 2Al + Fe2O3 --> Al2O3 + 2Fe Find the mol ratio between Al and Fe: 1 mol Al ~ 1 mol Fe Find the number of mol of Al given = g, Al/MM, Al Find the number of mol Fe2O3 given = g, Fe2O3/MM, Fe2O3 See the molar ratio from the equation between Al and Fe2O3. For every 2 mol Al, you should have 1 mol Fe2O3. If you don't then Fe2O3 is the limiting reactant. If you have more than enough Fe2O3, then Al is the limiting reactant. Choose the limiting reactant, and find the mol ratio with Fe, freom th balanced equation. For every mol of Fe2O3, there will be 2mol Fe, if Fe2O3 is the limiting reactant. Find mol Fe. mol Fe = #mol Fe2O3 x 2 mol Fe/1mol Fe2O3 = mol Fe OR: mol Fe = #mol Al x 2 mol Fe/2 mol Al = mol Fe Choose the one that gives you the *least* amount of mol Fe. THEN find g, Fe = #mol Fe x MM, Fe = g, Fe As you can see, there are several steps to doing this. Good luck.
CHEMISTRY/STOICHIOMETRY HELP!!!! ?
The equations: N2 + O2 -> 2 NO NO + 2O2 -> 2NO2 You only need this last one nO2=m/MM=384/32= 12 mol 2 mol O2_______2 mol NO2 12 mol O2______ n mol NO2 n mol NO2= 12 mol m (NO2)=n*MM=12*46= 552 g NO2 1 mol NO ________2 mol O2 n mol NO________12 mol O2 n mol NO= 12/2= 6 mol m NO= n*MM= 6*31= 186 g NO
Help with ap chemistry stoichiometry?
Convert 2 g of Cu3(PO4)2 to moles. Always use moles in these calculations. moles = mass / molar mass molar mass Cu3(PO4)2 = (3 x 63.55) + (2 x 30.97) + (8 x 16.00) = 380.52 g/mol moles Cu3(PO4)2 = 2 g / 380.52 g/mol = 0.005256 moles of Cu3(PO4)2 The balanced equation states that 3 moles of Cu(NO3)2 react with 2 moles of K3(PO4) to produce 1 mole of Cu3(PO4)2. So moles of Cu(NO3)2 required to produce 0.005256 moles of Cu3(PO4)2 = 3 x 0.005256 moles = 0.01577 moles of Cu(NO3)2 moles = mass / molar mass molar mass Cu(NO3)2 = 63.55 + (2 x 14.01) + ( 6 x 16.00) = 187.55 g/mol Therefore mass Cu(NO3)2 = mol x molar mass = 0.01577 mol x 187.55 g/mol = 2.958 g of Cu(NO3)2 = 3 g Moles of K3(PO4) required to produce 0.005256 moles of Cu3(PO4)2 = 2 x 0.005256 moles = 0.01051 moles of K3(PO4) mass = moles x molar mass molar mass K3(PO4) = (3 x 39.10) + 30.97 + (4 x 16.00) = 212.27 g/mol mass K3(PO4) = 0.01051 moles x 212.27 g/mol = 2.23 g
Help with Stoichiometry Chemistry homework!?
A chemist reacts 120.0 ml of a .250 M solution of NaOH with an excess amount of a BaCl2 solution. What mass of Ba(OH)2 would you expect to get under ideal stoichiommetric conditions? 2 NaOH (aq) + BaCl2 (aq) ----> Ba(OH)2 (aq) + 2 NaCl (aq)
Chemistry / stoichiometry help needed (:?
You can easily calculate the total amount of hydrogen sulfide to be dealt with; just mulitply the concentration by the total volume of liquid. Divide by the molecular weight to get moles. From the equation (is it balanced? Yes. But you ALWAYS check.) the number of moles of chlorine is the same. Multiply by the molecular weight of chlorine to get the amount required to remove all the sulfide. If this exceeds one gram, then you have a proportion: the ratio of sulfide removed to sulfide supplied equals the ratio of chlorine supplied to chlorine required to remove all of the sulfide.
Chemistry: Stoichiometry Problem help (10pts)?
I agree with the first answer. 1/10 of the sampe is C4H10 and 9/10 is O2 So you have 1 ml of C4H10 and 9 ml of O2 The equation is already balanced, just add all the atoms up and make sure there are the same number of each atom on each side. The ideal gas law states that 1 mole of any ideal gas occupies the same volume as 1 mole of any other ideal gas under the same conditions of Temp and pressure. What this means is that your volume ratio (1 : 9) is exactly the same as your mole ratio (1 : 9) So 1 ml C4H10 needs 6.5 ml O2 to fully react There will be 9 - 6.5 = 2.5 ml of O2 left over
What is stoichiometry and why is it used in chemistry?
In chemistry, stoichiometry is a kind of math that helps you measure and calculate amounts of chemicals. There are several quantity units used in stoichiometry. Some of them, like grams and liters, will be familiar even to people who have not studied chemistry. One unit, the mole, is generally only used in a chemistry setting. A mole is a counting unit, like a dozen or a score. A mole is approximately [math]6.022 \times 10^{23}[/math] units. That is the number of atoms in exactly 12 grams of carbon-12, but it can apply to any atom, molecule, or particle.Stoichiometry can be used in many different ways:To calculate how much product a chemical reaction is expected to produce.To calculate the percent yield of a chemical reaction that failed to produce its expected output.To calculate how much of a reactant is necessary to react with another reactant.To determine which of two reactants will be consumed first in a chemical reaction.To determine the formula of an unknown compound.To determine the formula mass of an unknown compound.To determine the concentration of a solution.And there are many other applications. Stoichiometry is one of the most practical applications in chemistry, because it allows researchers to bridge the gap between the macroscopic quantities that their instruments can measure, and the raw numbers of atoms and molecules swirling around inside their test tubes.
Help with a chemistry problem about stoichiometry can someone explain this to me?
You said you have a balanced equation (I'm assuming you're correct). From each N2O5 you get 2 x HNO3. Therefore, from one mole of N2O5 you get 2 moles HNO3 Next step; calculate molecular mass of HNO3 (by adding up the individual atomic masses: 1xH + 1xN + 3xO). Now , if you started with .8874 moles of N2O5, you produced twice this number of moles of HNO3 (ie 1.775 moles). Now multiply this by molecular mass to determine grams.