Given the reaction: 2 HgO(s)-> 2 Hg(1) + O2(g) (a) What weight of elemental mercury should be produced by the decomposition of 94.5 g of HgO? (b) If 75.2 g of Hg is actually collected, what is the percent yield? (Show your work!) For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). B IUS Paragraph Arial 10nt " D

Given the reaction: 2 HgO(s)-> 2 Hg(1) + O2(g) (a) What weight of elemental mercury should be produced by the decomposition of 94.5 g of HgO? (b) If 75.2 g of Hg is actually collected, what is the percent yield? (Show your work!) For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). B IUS Paragraph Arial 10nt " D

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter20: Environmental Chemistry-earth's Environment, Energy, And Sustainability

Section: Chapter Questions

Problem 41PS

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Be sure to answer all parts. Industrially, vanadium metal, which is used in steel alloys, can be obtained by reacting vanadium(V) oxide with caleium at high temperatures: 5Ca + V,0g → 5C2O + 2V In one process, 1.540 × 10° g of V,Og react with 2.040 × 10° g Ca. (a) Calculate the theoretical yield of V. (b) Calculate the percent yield if 781.0 g of V are obtained. Report your answers to the correct number of significant figures.
Be sure to answer all parts. Industrially, vanadium metal, which is used in steel alloys, can be obtained by reacting vanadium(V) oxide with calcium at high temperatures: Hint oints Solution 5Ca + V,05- 5CAO + 2V eBook Guided Solution Print In one process, 1.540 x 10° g of V,O5 react with 2.120 × 10³ g Ca. References (a) Calculate the theoretical yield of V. (b) Calculate the percent yield if 815.0 g of V are obtained. Report your answers to the correct number of significant figures. Next > Mc Graw Hill Prev 4 of 45 31°C Mostly sunny P Type here to search 1080 Jade Pa F12 Prt Sc F11 F10 NumLk F8 F9 F7 F6 E5
What mass of water will be consumed from the reaction of 78 g of calcium carbide, CaC, with water in the following reaction? CaC,(s) + 2H,0(1) C,H;(g) + Ca(OH),(s)
The balanced equation for burning octane is: 2 C8H18(g) + 25 O2(g) For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). BIUS Paragraph Arial X² X₂ , я ¶ V ¶< - + ABC V V 18 H₂O(g) + 16 CO2(g). What weight of oxygen is required to completely bum 19.8 g of octane? 10pt √ V Π " Ω Θ 13 v A V 用く x HH V₂ 8.8 % 0 Ix 88 Q 883
Page < 2 of 2 ZOOM + 7. Write balanced chemical eqess | esc | to exitTO Screen ctions. a. production of ammonia, NH3(g), by combining N2(g) and H2(g) b. production of methanol, CH3OH(1), by combining H2(g) and CO(g) c. production of sulfuric acid by combining sulfur, oxygen, and water 8. Diborane and related compounds were proposed as rocket fuels in the 1950s. A representative reaction for this class of molecules is that of B2H6 and O2 to form B2O3 and H2O. Write the balanced chemical equation for this process. 9. Silicon nitride, Si3N4, is used as a reinforcing fiber in construction materials. It can be synthesized from silicon tetrachloride and ammonia. The other product is ammonium chloride. Write the balanced chemical reaction for this process. 10. Classify the following compounds as electrolytes or nonelectrolytes: a. potassium chloride, KCl b. hydrogen peroxide, H2O2 c. methane, CH4 d. barium nitrate, Ba(NO3)2
1. Given the equation for the combustion of isopropyl alcohol 2 C3H7OH +9 02 6 CO2 +8 H2O Set up the mole ratio of (a) CO2 to C3H7OH (b) C3H7OH to 02 (c) O2 to CO2 (d) H2O to C3H7OH (e) CO2 to H2O (f) H2O to O2
used in the manufacture of cement: ate rock (limestone) is heated to produce the quicklime, i.e., calcium oxide, Carbon dioxide is also released into the atmosphere when calcium carbon- PROBLEM 44 CACO3(s) CaO(s) + CO;(g) Calculate the mass, in metric tons, of CO2 released per metric ton of lime- une used in this process. What is the mass of carbon that the air gains for each of carbon dioxide that enters the atmosphere? Note that at least gram os much carbon dioxide is released from combustion of the fossil fuel needed to heat the limestone as is released from the limestone itself.
5. Answer the following question regarding stoichiometry: How many grams of malachite, CuCO,Cu(OH)2 can be prepared from the reaction of 2.05 g of copper sulfate pentahydrate, CuSO-5H2O and 10.3 g of sodium carbonate, NaCO, according to the following chemical equation? Show work for credit. Cuso 5H;0(aq) + 2NACO3(aq) CuCO,-Cu(OH)2(s) + 2Na;SO.(aq) + CO (g) + 9H20(1)
6. In one experiment, a mixture of 0.250 mol of methane gas was burned in 1.25 mol of ogen sina sealed container. Find the limiting reactant and calculate the theoretical yield of water produced. 2.34 g of water was actually produced in the experiment, what is the percentage yield? (9) CH,(g) + 02(9) Co,(g) + H20G) Reply... :
7. For sequential reaction: A > B + C .(i) 2B —> С +2D If % yield of (i) and (ii) reactions are 90% and 80% respectively, then the overall % yield is expected to be: (A) 90% ...(ii) (B) 80% (С) 72% (D) 10%
Consider the following reaction: 6HCI + 2AI→ 2AICI3 + 3H2 Calculate the mass (in grams) of AICI3 produced by reacting 19 g of HCI and 15 g of Al. (MW (g/mol): HCl = 36.5, Al = 27, AICI3 = 133.3, H2 = 2) Express your answer with 1 decimal place. A
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