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Lithium reacts with nitrogen gas according to the following reaction? 6Li(s)+N2(g) yields 2 Li3N(s) What mass of lithium (in g) is required to react completely with 55.5 mL of N2 gas at STP?

Inali replied: "(1 atm)(.0555L)= n(.0821)(273K) n=.0248mol N2 .00248molN2(6)= .0149molLi .0149molLi(6.941g/mol)=.103grams of Li"

when heated lithium reacts with nitrogen to form lithium nitride. What is the % yield of the reaction if 13.4g? of lithium is heated with 34.8g of N2 and the actual yield Li3N is 7.00g? Please also show me how to do it because I have no clue.. Thanx a lot

Thomas C replied: "3Li + N2 -> 2Li3N no. of mol of N2 = 34.8/28 = 1.24 mol no. of Li = 13.4/7 = 1.91 mol Li is limiting reagent theoretical yield = 2/3 * 1.91 = 1.27 mol of Li3N % yield = 7/(1.27*(21+14) * 100% = 22%"

Lithium metal reacts w/ nitrogen gas to produce lithium nitride? What volume of nitrogen gas at 2atm and 175 degrees C is required to produce 75.0 g of lithium nitride?

j_space17 replied: "Assuming that we have excess Lithium - Since we're going to be doing stoichiometry, we need a balanced equation. 6Li + N2 ---> 2Li3N (75.0g Li3N / 1)*(1 mol. of Li3N / 34.823g Li3N)*(1 mol. of N2 / 2 mol. of Li3N) = 1.077 mol. of N2 Then we use the ideal gas law - PV = nRT (2 atm)(V) = (1.077 mol.)(0.0821)(448K) V = 19.8 L of N2"

theonlybeldin replied: "75 g / 34.8 g/mol = 2.16 mole Li3N Need 1 mol N2 to produce 2 moles Li3N, so moles N2 = 1.08 moles V = nRT / P = 1.08 moles * 0.08206 * 448 K / 2 atm = 19.9 L"

Write a balanced chemical equation when lithium hydroxide reacts with phosphoric acid and the reaction is a do? GOD I HATE THESE TYPE OF PROBLEMS THEYRE SO FKING CONFUSING sry its not do? its double displacement?

Andrew replied: "its double replacement not double displacement 3LiOH + H3PO4 -> Li3PO4 + 3H2O"

What is the symbol equation for : lithium phosphide reacts with lead (III) nitrate? And what is the reaction type ?

isitza replied: "Li3P + Pb(NO3)3---> 3LiNO3 + PbP"

solid lithium oxide reacts with water to form aqueous lithium hydroxide? Complete and balance the following equation: solid lithium oxide reacts with water to form aqueous lithium hydroxide?

Dr.A replied: "Li2O + H2O >> 2 LiOH"

Lithium hydroxide reacts with carbon dioxide as follows:? Okay this is what the question asks: Lithium hydroxide reacts with carbon dioxide as follows: LiOH+CO2-->Li2CO3+H2O What mass in grams of lithium hydroxide is needed to react with 11g of carbon dioxide?

Gabry Hyrule replied: "First, find the molecular weight of your compounds: LiOH = 7 + 16 + 1 = 24g/mol CO2 = 12 + 16*2 = 44g/mol You have 11g of CO2, find n n = 11g / 44g/mol = 11/44mol = 0.25mol Now balance your equation (some people do it first): LiOH + CO2 = Li2CO3 + H2O 2LiOH + CO2 = Li2CO3 + H2O YESZ! For every moles of CO2 you react, 2 moles of LiOH react. So nLi = 2nCO2 nLi = 2*0.25mol = 0.5mol Find the mass, m = 0.5mol * 24g/mol = 12g You'll need 12g of Lithium Hydroxide"

Easy gas pressure chemistry problem? What mass of of lithium is required to react completely with nitrogen gas? Lithium reacts according to the reaction: 6Li (s) + N2 (g) --> 2Li3N (s) What mass of lithium (in g) is required to react completely with 57.2 mL of N2 gas at STP? STP is 1 atm and 273 kelvin. Someone please explain this to me.

Pye replied: "First, you need to know how many moles of nitrogen you have. You're given the volume of nitrogen, its pressure and its temperature. From this information, you can calculate moles using the ideal gas law (pressure times volume equals number of moles times the constant R times temperature in kelvin): PV = nRT (101.3 kPa)(0.0572) = n(8.31)(273) n = 0.00255 moles N2 Now that you have moles of N2, simply use the equation's stoicheometry to find the moles of lithium required: 6 moles Li required per mole N2, therefore: 0.00255 * 6 = 0.0153 moles Li required. And convert to grams: 6.941 g/mol * 0.0153 moles = 0.106 g Li required."

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