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Solid lithium hydroxide is used in space vehicles to remove exhaled carbon dioxide.? Solid lithium hydroxide is used in space vehicles to remove exhaled carbon dioxide. The products are solid lithium carbonate and liquid water. What mass of carbon dioxide gas can 933g of lithium hydroxide absorb? How many grams of water will be produced?

HPV replied: "First write the balanced equation: 2LiOH + CO2 ==> Li2CO3 + H2O 933 g LiOH x (1 mole LiOH / 23.95 g LiOH) = 39.0 moles LiOH 39.0 moles LiOH x (1 mole CO2 / 2 moles LiOH) x (44.0 g CO2 / 1 mole CO2) = 858 g CO2 39.0 moles LiOH x (1 mole H2O / 2 moles LiOH) x (18.0 g H2O / 1 mole H2O) = 351 g H2O"

What volume of CO2 gas at 218 degrees Celsius and 781 mmHg could be absorbed by 327 g of lithium hydroxide? Lithium hydroxide, LiOH, is used in spacecraft to recondition the air by absorbing the carbon dioxide exhaled by astronauts. The reaction is 2LiOH + CO2 ==> Li2CO3 + H2O What volume of carbon dioxide gas at 218 degrees Celsius and 781 mmHg could be absorbed by 327 g of lithium hydroxide?

Howard V replied: "327 g LiOH x (1 mole LiOH / 24.0 g LiOH) x (1 mole CO2 / 2 moles LiOH) = 6.81 moles CO2 Using the ideal gas law: PV = nRT V = nRT / P = (6.81 moles)(0.0821 L atm / K mole)(491 K) / (781 / 760) atm = 267 L"

Some Body replied: "327 g LiOH * 1 mol LiOH/23.94 g = 13.66 moles LiOH 13.66 moles LiOH * 1 mol CO2 / 2 mol LiOH = 6.83 mol CO2 PV = nRT (781 mmHg)(V) = (6.83 mol)(62.4 L·mmHg·K-1·mol-1)(218 + 273 K) V = 268 liters"

Lithium hydroxide, LiOH, is used in spacecraft to recondition the air by absorbing the carbon dioxide? exhaled by astronauts. The reaction is: 2LiOH(s) + CO2 (g) ==> Li2CO3(s) + H2O(i) What volume of carbon dioxide gas at 218 degree celsuis and 781 mm Hg could be absorbed by 327g of lithium hydroxide?

Robito replied: "1 mole of CO2 absorbed for every 2 moles of LiOH 327 g of LiOH is 327 g / 23.95 g/mol = 13.65 mol, which means 6.83 mol of CO2 can be absorbed. PV = nRT, V = nRT/P V = (6.83 mol)(62.364 L-mm Hg/mol-K)(218+273)K/781 mm Hg V = 268 L"

Lithium hydroxide is used in the space program to remove carbon dioxide (from respiration) in spacecraft.? Specifically, lithium hydroxide, LiOH, reacts with carbon dioxide, CO2, to form lithium carbonate, Li2CO3, and water. 2 LiOH + CO2 ® Li2CO3 + H2O What mass of CO2 can be absorbed by 36 g of LiOH? a. 14.3 b. 18 c. 33 d. 36

Cirric replied: "HI. 36 grams of anhydrous lithium hydroxide can remove 16,200 cm^3 of carbon dioxide gas. At standard temperature and pressure, the density of carbon dioxide is around 1.98 kg/m³. Does this get you started?"

laurahal42 replied: "This is a standard high school chemistry problem, and you know how to solve it. 36 g of LiOH is how many moles? How many moles of CO2 does that react with? What is the mass of that many moles of CO2?"

Space vehicles use solid lithium hydroxide to remove exhaled carbon dioxide according to the equation:? 2LiOH + CO2 --> Li2CO3 +H2O. Determine the mass of carbon dioxide removed if the space vehicle carries 42.0 mol LiOH.

Johnny A replied: "42.0 moles LiOH would react with 21.0 moles CO2 21.0 moles CO2 X 44 g/mole = 924 g CO2"

Volume of CO2 gas absorbed by342 g of lithium hydroxide..? Lithium hydroxide, LiOH, is used in spacecraft to recondition the air by absorbing the carbon dioxide exhaled by astronauts. The reaction is shown below. 2 LiOH(s) + CO2(g) Li2CO3(s) + H2O(l) What volume of carbon dioxide gas at 21°C and 767 mmHg could be absorbed by 342 g of lithium hydroxide?

Humm... Y replied: "Pressure (atm) x Volume (L) = n (mol) x R x Temperature (K) 1 atm = 760 mm Hg ; Pressure = 767/760 = 1.0092 atm Temperature = 273 + 21 = 294 K Mollecular weight of LiOH = 6.9 + 1.008 + 16 = 23.908 For each 2 mol of LiOH that react, 1 mol of CO2 is absorbed. We calculate the number of mol of LiOH in 342 g of LiOH: (342 g LiOH)/(23.908 g/mol LiOH) = 14.30483 mol of LiOH So, if there's 1 mol of CO2 per 2 mol of LiOH... 14.30483/2 = 7.152417 mol of CO2 Now, having all the elements of our initial equation known except one, we proceed to solve it: V = nRT/P = (7.152417 x 0,082 x 294)/1.0092 = 170.85 Litre of CO2 I hope this helps ;)"

Calculate the molarity of a solution prepared by dissolving 1.495 moles of LiOH in enough water to give a fi? Lithium hydroxide is used in alkaline batteries. Calculate the molarity of a solution prepared by dissolving 1.495 moles of LiOH in enough water to give a final volume of 750. mL.

siddique s replied: "750 ml contain number of moles= 1.495 1 will---------------------------------------= 1.495/750 1000 mL .................................= (1.495/750)*1000 = x moles/L means molarity"

NB replied: "=1.495/750x1000=1.99 M"

Can someone please help me with his Chem question? Lithium hydroxide is used in alkaline batteries. Calculate the molarity of a solution prepared by dissolving 1.495 moles of LiOH in enough water to give final volume of 750 mL. ???

jakebubba14 replied: "molarity = mol solute / L solution. you already have the mol solute... 1.495 mol LiOH you also have the solution amount in mL... just convert 750 mL to L 750 mL ( 1 L / 1000 mL) = .75 L so molarity = 1.495 mol LiOH / .75 L = 2 M"

lithium again from wikipedia? Lithium is an alloying agent used to synthesize organic compounds Lithium hydroxide (LiOH) is an important compound of lithium obtained from lithium carbonate (Li2CO3). It is a strong base, and when heated with a fat, it produces a lithium soap. Lithium soap has the ability to thicken oils and so is used commercially to manufacture lubricating greases. How does lithium related to organic compound and why it can make soap .Hydoxide reacts with an organic compund to form soap? Also, for need, is all oxide dissolve in water ? And to form hydroxide?

chem_freak replied: "Li is used in organic chemistry as organolithium compounds, the main use being in bases (like Butyllithium). it can not make soap. LiOH does. any strong base does, since soaps are salts of fatty acids, produced by the hydrolysis of fat. no, not all oxides are well soluble in water. CuO, Ag2O and so on are bad soluble in water. and for an oxide to give a base when reacting with water it needs to be a basic oxide, i.e. of a metal. apart from that you can dissolve SO3 in water (an oxide) and get a hydroxide (take a look at the structure of sulfuric acid). unfortunately this hydroxide is extremely acidic."

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