Lithium Hydroxide is used for the removal of carbon dioxide in space vehicles. The reaction is given as follows.2LIOH+CO2LizCO3+H2OCompoundMolar MassLIOH23.949 g/molCO244.01 g/molLICO373.892 g/molH2O18.016 g/molFrom the given values, determine which the limiting reactant is; and indicate the amount of excess reactant aftera complete reactionLimiting Reactant(37)(40)Amount of LIOHAmount of CO2Amount of Excess Reactant (g)(38-39)(41-42)3 moles70 g2 moles100 g(43 - 44) What is the theoretical mass (in g) of CO2 that can be removed by using 100 g of LIOH?(45-46) If we want to completely remove 400 g of CO2 from the vessel, how many grams of LIOH do weneed?(47-48) For the removal of 200 g CO2, an excess amount of LIOH was used. The reaction yield was 300 g ofL12CO3.What is the percent yield of the reaction?The safety limit for the vessel requires the removal of at least 180 g CO2.From the given yield of Li,CO; in item (47-48), is the vessel safe?(49)(50 - 51) Suppose that the safety limit for CO; removal in item (47-48) was not reached, propose ways on howto increase the amount of CO, removed. Answer in not more than 3 sentences.1 Add File

As per the policy, we are only allowed to answer only 1st question. To get the answer of other…

Lithium Hydroxide is used for the removal of carbon dioxide in space vehicles. The reaction is given as follows. 2LIOH+ CO2 LizCO3+ H20 Compound Molar Mass LIOH 23.949 g/mol CO2 44.01 g/mol LizCO3 73.892 g/mol H2O 18.016 g/mol From the given values, determine which the limiting reactant is; and indicate the amount of excess reactant after a complete reaction Amount of LİOH Amount of CO2 70 g Limiting Reactant (37) (40) Amount of Excess Reactant (g) (38- 39) (41-42) 3 moles 100 g 2 moles (43 - 44) What is the theoretical mass (in g) of CO2 that can be removed by using 100 g of LIOH?

Lithium Hydroxide is used for the removal of carbon dioxide in space vehicles. The reaction is given as follows. 2LIOH+ CO2 LizCO3+ H20 Compound Molar Mass LIOH 23.949 g/mol CO2 44.01 g/mol LizCO3 73.892 g/mol H2O 18.016 g/mol From the given values, determine which the limiting reactant is; and indicate the amount of excess reactant after a complete reaction Amount of LİOH Amount of CO2 70 g Limiting Reactant (37) (40) Amount of Excess Reactant (g) (38- 39) (41-42) 3 moles 100 g 2 moles (43 - 44) What is the theoretical mass (in g) of CO2 that can be removed by using 100 g of LIOH?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

6.) What is the maximum mass of H20 that Can be produced by Combining 66.4g of each reactant. 4NH3 (g) + 5O₂ (g) → 4NO(g) + 6 H ₂ O (g)
If 15.00ml of a 1.00 M HCI solution is mixed with 25.00mL of a 0.250M NaOH solution in a process that produces 273 mg of NaCl, what is the percent yield?
Balance the following equation: - > 4He + X 8Be 4 O 8He 2 O 12C 6. О 4Не 2 O 4Li 3
Dteremine the limiting reaganet (SHOW THE calculations for determinig the limiting reagent ) and calculate the theoretical mass of PbI2 by using limiting reagent. show your calculations. Balanced Equation: Pb(NO3)2 (aq) + 2KCL(aq) ---> 2KNO3(aq) + PbI2(s) No of moles of Pb(NO3)2 = 0.003 No of moles of KI = 0.007
Data and calculations Balance the reaction first Mass (g ) Crucible ( empty) 48.11 Sample 1.00 Crucible ( after heating ) 48.81 Cuo ( actual in g) 0.70 Cu2CO3 (OH)2 221 g mol molar mass Cuo molar mass 79.5 g mol Mol Cuo produced 0.0088 mol ( actual in mol ) Mol sample used 0.0045 mol Mol Cuo calculated ( Theoretical yield in mol ) g Cuo ( Theoretical yield in g) Percent yield
What is the theoretical yield and the % yield, if 12.0 grams of copper (II) chloride is produced from 63.4 grams of hydrochloric acid and 138 grams of copper (II) sulfide by the unbalanced chemical equation given below. CuS + HCl + CuCl2 + H2S
3 Cu + 8HNO3 --> 3 Cu(NO3)2 + 2 NO + 4 H2O In the above equation how many moles of water can be made when 178.7 grams of HNO3 are consumed?
Balance the following chemical equation. NaN, - Na + N2 Products Reactants Na = Na = N = N = Calculate the Molar Mass for the Following Compounds. Use the Periodic Table ! Periodic Table:https://ptable.com/#Properties Compound / Chemical Formula Molar Mass Example : 0, 32.00 grams = 1 mole NaN, Na N2
A student mixes a solution containing 2.08g BaCl2 with a solution 0.71g Na2SO4 and obtains actually 0.95g BaSO4 what is the percent yield of this percentage BaCl2+NaSO>BaSO4+2NaCl
Consider the following reaction. Na2CO3 + Mg(NO3)2 --> MgCO3 + 2NaNO3 Assuming the reaction goes to completion, when 25 mL of a 0.1 M Na2CO3 solution reacts with 22 mL of a 0.3 M Mg(NO3)2 solution, what is the maximum nuber of grams of MgCO3 that can produce? Which is the limiting reactant in the chemical reaction?
Use the References to access important values if needed for this question. According to the following reaction, how many grams of phosphoric acid will be formed upon the complete reaction of 32.1 grams of water with excess diphosphorus pentoxide? diphosphorus pentoxide(s) + water (1) → phosphoric acid(aq) Mass grams phosphoric acid
If 0.503 mol of zinc reacts with excess lead (IV) sulfate, how many grams of zinc sulfate will be produced in the reaction?