e. Co2(g)- + 2LIOH(s) → Lİ2CO3(aq) + H2O(1) 40. 9 In a one-person spacecraft, an astronaut exhales 880g of CO2(g) (molar 240 g mass 44g/mol) per day. To prevent the buildup of CO2(g) in the spacecraft, a device containing LIOH(s) is used to remove the 960 g Co2(g), as represented by the equation above. What mass of LIOH(s) (molar 480 g mass 24g/mol) is needed to react with all of the CO2(g) produced by an astronaut in one

e. Co2(g)- + 2LIOH(s) → Lİ2CO3(aq) + H2O(1) 40. 9 In a one-person spacecraft, an astronaut exhales 880g of CO2(g) (molar 240 g mass 44g/mol) per day. To prevent the buildup of CO2(g) in the spacecraft, a device containing LIOH(s) is used to remove the 960 g Co2(g), as represented by the equation above. What mass of LIOH(s) (molar 480 g mass 24g/mol) is needed to react with all of the CO2(g) produced by an astronaut in one

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

2HCl(aq)+ Mg(s) —> MgCl2 (aq) + H2(g)
710 10. The formula of rust may be represented most simply as Fe(OH)3. The balanced equation when iron corrodes is: Try @home d. 60 e. 150 Page | 4 4Fe +302 + 6H₂O → 4Fe(OH)3 a. (2 points) What are the percentages by weight of the elements in rust? b. 5-points) How many grams of rust are formed when one kg of iron corrodes?
In the textile industry, chlorine is used to bleach fabrics. Any of the toxic chlorine that remains after the bleaching process is destroyed by reacting it with a sodium thiosulfate solution, Na2S2O3(aq)- NazS203{aq) + 4C12(g) + 5H2O1) - 2NaHS04(aq) + 8HCI{aq) If 141.88 kg of Na2S203laq) reacts with 45.34 kg of Cl2 and excess water, how many kilograms of NaHSO4 are expected? Your Answer: Answer units
40
Consider the reactions represented by equations below: I. 4NACIO:(s) – 3NACIO:(s) + NaCI(s) II. 3Cu(s) + 8HNO:(aq) 3Cu(NO)2(aq) + 2NO(g) + 4H20 III. 2NO2 (g) + H20(1) HNO,(aq) + HNO2(aq) Which of the reactions involve 34. disproportionation? I and II Il and II I and III 1, Il and III A B
8:58 PM Thu Oct 5 Question 9 of 19 What mass of precipitate (in g) is formed when 45.5 mL of 0.300 M K3PO4 reacts with 52.5 mL of 0.200 M Cr(NO3)3 in the following chemical reaction? 1 4 7 K3PO4(aq) + Cr(NO3)3(aq) → CrPO4 (s) + 3 KNO3(aq) g 2 3 5 6 8 9 Submit X с
A water-soluble salt formed by Hg2+ and chlorate 106.49 g was dissolved in a solution containing 15.488 g of sodium sulfide, which gave rise to an insoluble mercury salt. How much insoluble mercury salt is formed? (g) How much of the excess reagent remains? (g)
2. A chemistry student is doing a titration lab in D314 and needs to make up 2 liters of NaOH for the class and standardize the NaOH with the organic acid KHP (MW 204.2 g/mol). The instructions say 5 grams/ liter of NaOH pellets which is - 0.1 M by the molar mass of NaOH. The student weighs out 10 grams of NaOH and dissolves it in 2 liters of water. The student then weighs out 0.4120 g of KHP and puts the organic acid in 50 mL of water and adds ~ 3 drops of 1% phenolphthalein indicator. To reach the endpoint (pink) where moles KHP are used up with NaOH, he adds 17.5 mL of the NaOH from the buret. What is the concentration of the NaOH? If he repeats this 2 more times an adds 16.9 mL and 18.2 mL what is the average concentration of the NaOH and the % difference? K
5. When 5.0 moles of potassium metal reacts with an excess of H₂0, 3.5 g of H2 are produced. 2 K (s) + 2 H20 (1) 2 KOH (aq) H₂ (g) a. Calculate the number of moles of water needed to react with all of the potassium metal. (Ans: 5 mol) + b. Calculate the theoretical yield of H2, in grams, formed when all 5.0 moles of potassium metal are consumed. (Ans: 5.04 g) c. Calculate the percent yield of the reaction, given 3.5 g (actual yield) are produced. (Ans: 69.4%)
13. Hydroxyapatite is the main mineral component of bone. How many grams of hydroxyapatite will dissolve in 1.00 L of H20? Ksp = 2.34 x 10-59; Molar mass = 502.3 g/mol Cas (PO4)30H (s) 5 Ca2+ (aq) + 3 PO43- (aq) + OH- (aq)
What gas do you get when you add CuCO3(s) and H2SO4 (aq) together
Calculate the final molarity of H2O2H2O2 if 5.9 mL5.9 mL of a 3.0% w/w H2O23.0% w/w H2O2 solution, which has a density of 1.0 g/mL,1.0 g/mL, is added to 5.9 mL5.9 mL of a starch-iodide solution. final [H2O2]=[H2O2]= MM Calculate the final molarity of H2O2H2O2 if 1.6 mL1.6 mL of the 3.0% w/w H2O23.0% w/w H2O2 solution is diluted with 3.4 mL3.4 mL water, then added to 5.0 mL5.0 mL of a starch-iodide solution. final [H2O2]=[H2O2]= M