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16 Nov 2019

can someone help me understand the first three with steps and the charges? I don't understand why at the end aliuminum problems is 2albr3 +3cl2 yield 2alcl3 3brw?? and help me out with the other problems please.

aluminum bromide chlorine-9 aluminum chloride bromine sodium phosphate calcium chloride calcium phosphate sodum aluminum hydrogen chloride aluminum chloride hydrogen calcium hydroxide phosphoric acid calcium phosphate +water aluminum hydroxide +calcium sitate aluminum sulfate calcium hydroxide n dioxide t water

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Elin HesselLv2

12 Jul 2019

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Show transcribed image text Chemistry 2 online Final exam review(1) Saved to this PC es Mailings Review View Help Tell me what you want to do talled, but first we need to close some apps. Update now Chemistry 2 online Final exam review/extra credit (50pts) Write the following word equation using the correct formulas, balance and classify as double/single replacement, combustion, synthesis or decomposition: 1) Decane reacts with oxygen to produce carbon dioxide and water 2) Rubidium plus rubidium nitrate yields rubidium oxide and nitrogen 3) Aluminum hydroxide reacts with carbonic acid to produce aluminum carbonate and water Describe the following equations in terms of: 4) Grams: 5) Moles: 6) Liters: (all substances in the equation are in liters) N3H2NH Complete the following stoichiometry problems Zinc reacts with hydrochionic acid to produce zinc chloride and hydrogen. What volume of hydrogen is produced if you start with 2.5g of zinc? Aluminum chloride decomposes to produce aluminum and chlorine. How many molecules of chiorine are produced from 10.0g of aluminum chloride? 7) 8) Complete the following conversions: 9) calrulate the mass (o) of 3 13 10monles of S
Chemistry 2 online Final exam review(1) - Saved to this PC ences Mailings Review View Help Tell me what you want to do installed, but first we need to close some apps. Update now Complete the following conversions: 9) Calculate the mass (g) of 3.13 x 10 moles of s 10) Calculate the number of formula units in 42.4 moles KNO Answer the following questions/calculations 11) Calculate the gram formula mass of aluminum tartrate. 12) A sample of silver with a mass of 8.44g reacts with sulfur to form a compound that has a mass 9.69g. What is the percent composition of the compound? 13) Calculate the percent composition of Vitamin E (CsHsoO)) 14)Ibuprofen, a headache remedy, is 75.69% C, 15.51% O and 8.80% H. Calculate the empirical formula. 15) A sample was found to contain 1.062g hydrogen, 133.757g of iodine and 50.589g of oxygen. The mass of the compound is 175.91g/mol. What is the molecular formula? 16) Calculate the mass of 2.63 x 101" molecules of CH20 17) How many moles of oxygen (O) are contained in a 5.0 L cylinder that has a pressure of 175 atm and a temperature of 20 degrees Celsius? (Ideal Gas Law) 18) What is the functional group for an alkane? 19) Ammonia is an acid. True or false?
Chemistry 2 online Final exam review(1) Saved to this PC References Mailings Review View Help ell me what you want to do eady to be installed, but first we need to close some apps Update now 16) Calculate the mass of 2.63 x 10* molecules of 17) How many moles of oxygen (O,) are contained in a 5.0 L cylinder that has a pressure of 175 atm and a temperature of 20 degrees Celsius? (Ideal Gas Law) 18) What is the functional group for an alkane? 19) Ammonia is an acid. True or false? 20) What do the letters lUPAC stand for? 21) Give an example of an Arrhenius base. Write the formulas for the following 22) Aluminum sulfate 23) Sulfuric acid 24) Palladium (1) hydroxide 25) Calcium perchlorate 0åèªç½@#

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Show transcribed image text correctly.Completion and turning in of the entire review will result in an additional +3 pts on your final exam. Show all work to get extra credit. Please contact your instructor for clarification or specific questions. Report the following answers to the following problems with the correct number of significant figures and units: 1. 1 (0521 g 0.4953 0098 61â-24.135ë¯¸+1(120 64 g 4.1847 a)(21st-241530 1 (98.61 C-24.135)120.64g 4.1 21.5Â°C-24.153C) 0.0213548 moles b. (00020334-ern) + ((61210 goles Og) 0.002030 moles 1.02 moles (68.79 mlt29.901 ml) (26.3-0.230) c. 2. You are drying a sample of Bas(POsh. After 5 minutes of drying it weighs 1.2034 g. You continue to dry the sample for another 5 minutes and it now weighs 1.9346 g. What is the percent change in mass? 3. What is the percent mass of carbon in sodium carbonate? 4. What is the density of water at 23.1051Â°c? Use Table 1.1 on page 27 of your lab manual to help. 5. Based on the following reacts, predict the products. Write the balanced molecular equation, total ionic equation, and net ionic equation. All reactions are done in water a. Sodium chloride +silver (I) nitrate b. Calcium bromide + iron (III) sulfate c. Ammonium phosphate+ nickel (II) nitrate d. Hydrochloric acid+ calcium carbonate 6. Write the two balanced chemical reactions for a. Copper (II) oxide reacting with methane under high heat b. Copper (1) oxide reacting with methane under high heat 7. You analyze a mixed sample of copper (1) oxide and copper (II) oxide. The plot and trendline for mass of copper versus mass of mixture yields a slope of 0.8031. What are the mass percents of copper (0) oxide and copper (II) oxide in the mixture?
8. During week 1 of the Empirical Formula Lab you extinguished your "L-tube" flame without waiting 9. 20.00 ml of a 0.30 M potassium phosphate solution is combined with 20.00 mL of a 0.40 M solution 10. An Erlenmeyer flask is capped with a rubber stopper at room temperature (25 C) and atmospheric 11. The first step of the copper cycle lab was reacting solid copper with nitric acid. The copper ends up 12. What are the spectator ions in the 6 reactions performed during the copper cycle lab? for the reaction to cool and did NOT relight the "L-tube" flame. How would this affect your calculated percent mass compared to the true percent mass? of calcium chloride. What is the limiting reactant? What is the identity of the precipitate formed in the reaction? How many grams of product should be collected? pressure (1 atm). What temperature does the Erlenmeyer flask need to be heated to for the stopper to pop off? Assume it needs to exceed external pressure by 0.5 atm to release the stopper. oxidizing to copper (ll). What is the oxidizing reagent in this reaction? 13. The known specific heat capacity of aluminum is o g mo 25.316 g of aluminum is placed in 99.134 of water at a starting temperature of 22.45Â°C. The metal has a AT-84.02c what is the final 14. The AH, of cobalt (U) nitrate is +47.7 kJ/mol. What is the AHr of solid cobalt (1) nitrate? 15. 5.000 g of aluminum (Il) chloride is dissolved in 60.0 mL of water. The temperature changes by 16. Draw the Lewis dot symbols for the following atoms: temperature of the water? ÎÎ(Nouql)--205.00 kJ/mol ÎÎ,(Co2"m)--58.2 kJ/mol 0.331 Â°C. The specific heat capacity of aluminum (III) chloride is 0.903 Wat s AH.? what is ÎÎ a Ð°, Ð½Ðµ Ñ, Ñ c. Ar d. P e. H 17. Draw the Lewis structures for the following molecules: a. NHa b. O2 XeF d. NF

Balance the following Chemical Equations:

____Fe(s) + ____H₂O(g) Â® ____Fe₃O₄(s) + ____H₂(g)

____C₂H₆(g) + ____O₂(g) Â® ____CO₂(g) + ____H₂O(g)

___ C₆H₁₄ (l) + ___ O₂ (g) Â® ___ CO₂ (g) + ___ H₂O (g)

___ C₃H₈O₃ (l) + ___ O₂ (g) Â® ___ CO₂ (g) + ___ H₂O (l)

___ NaN₃ (s) Â® ___ Na (s) + ___ N₂ (g)

__ C₃H₅N₃O₉ Â® __ CO₂ + ___ N₂ + ___ H₂O + ___ O₂

Write and Balance the equations:

Aqueous calcium hydroxide reacts with aqueous sodium carbonate to produce solid calcium carbonate and aqueous sodium hydroxide.

Solid iron reacts with Oxygen gas to form solid Iron (II) oxide

Copper(II) sulfide is oxidized by molecular oxygen to produce gaseous sulfur trioxide and solid copper(II) oxide. The gaseous product then reacts with liquid water to produce liquid hydrogen sulfate as the only product. Write the two equations which represent these reactions.

Indicate what type, or types, of reaction each of the following represents: (precipitation, acid-base, and oxidation-reduction.)

(A) H₂O(g) + C(s) â¶ CO(g) +H₂(g)

(B) 2KClO₃(s) â¶ 2KCl(s) +3O₂(g)

(D) Pb(NO₃)₂(aq) + H₂SO₄(aq) â¶ PbSO₄(s) + 2HNO₃(aq)

4. Silver can be separated from gold because silver dissolves in nitric acid while gold does not. Is the dissolution of silver in nitric acid an acid-base reaction or an oxidation-reduction reaction? Explain your answer.

5. Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides.

(A) H₃PO₄

(B) Al(OH)₃

6. Complete and balance the following acid-base equations:

(A) A solution of HClO₄ is added to a solution of LiOH.

(B) Aqueous H₂SO₄ reacts with NaOH.

7. Write the molecular, total ionic, and net ionic equations for the following reactions:

(A) Ca(OH)₂(aq) + HC₂H₃O₂(aq) â¶

(B) H₃PO₄(aq) + CaCl₂(aq) â¶

8. Write the balanced equation, then calculate the number of moles and the mass of Mg required to react with 5.00 g of HCl and produce MgCl₂ and H₂. Ans: 1.67 g Mg

9. H₂ is produced by the reaction of 118.5 mL of a 0.8775-M solution of H₃PO₄ according to the following equation: 2Cr + 2H₃PO₄ â¶ 3H₂ + 2CrPO₄. How many grams of H₂ are produced? Ans: .315 g H₂

10. Automotive air bags inflate when a sample of sodium azide, NaN₃, is very rapidly decomposed.

2NaN₃(s) â¶ 2Na(s) + 3N₂(g)

What mass of sodium azide is required to produce 2.6 ft³ (73.6 L) of nitrogen gas with a density of 1.25 g/L?

Ans: 142 g NaN₃

11. Urea, CO(NH₂)₂, is manufactured on a large scale for use in producing urea-formaldehyde plastics and as a fertilizer. What is the maximum mass of urea that can be manufactured from the CO₂ produced by combustion of 1.00 x 10⁴ grams of CO₂?

CO₂(g) + 2NH₃(g) â¶ CO(NH₂)₂(s) + H₂O(l)

Ans: 1360 g urea

12. What volume o f 0.750 M hydrochloric acid solution can be prepared from the HCl produced by the reaction of 25.0 g of NaCl with excess sulfuric acid? NaCl(s) + H₂SO₄(l) â¶ HCl(g) + NaHSO₄(s)

Ans: .570 L

13. A sample of 0.53 g of carbon dioxide was obtained by heating 1.31 g of calcium carbonate. What is the percent yield for this reaction? CaCO₃(s)â¶CaO(s) + CO₂(s)

Ans: 92.0 %

14. Citric acid, C₆H₈O₇, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger. The equation representing this reaction is

C₁₂H₂₂O₁₁ + H₂O +3O₂ â¶2C₆H₈O ₇+ 4H₂O

What mass of citric acid is produced from the reaction of 150. grams of sucrose if the yield is 92.30%?

Ans: 155 g

15. The phosphorus pentoxide used to produce phosphoric acid for cola soft drinks is prepared by burning phosphorus in oxygen.

(A) What is the limiting reactant when 0.200 mol of P₄ and 0.200 mol of O₂ react according to P₄+5O₂ â¶ P₄O₁₀?

(B) Calculate the percent yield if 10.0 g of P₄O₁₀ is isolated from the reaction.

Ans: 88.0 %

16. What is the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advanced batteries, according to the following unbalanced equation? Li + N₂ â¶ Li₃N

Ans: Li

17. What is the concentration of NaCl in a solution if titration of 15.00 mL of the solution with 0.2503 M AgNO₃ requires 20.22 mL of the AgNO₃ solution to reach the end point?

AgNO₃(aq) + NaCl(aq) â¶ AgCl(s) +NaNO (aq)

Ans: .3374 M

18. In a common medical laboratory determination of the concentration of free chloride ion in blood serum, a serum sample is titrated with a Hg(NO₃)₂ solution.

2Cl^â(aq) + Hg(NO₃)₂(aq) â¶ 2NO₃^â(aq) + HgCl₂(s)

What is the Cl^â concentration in a 0.25-mL sample of normal serum that requires 1.46 mL of .000825 M Hg(NO₃)₂(aq) to reach the end point?

Ans: 0.009636 M

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