Expt

Answer number 1,2,3,4,6 only.  True or false

Iron (Fe) 2. When 4.98 g of NaOH was dissolved in 49.72 g of water in a calorimeter at 23.7°C, the temperature of the solution went up to 50.1°C. 99.725 a. Is this dissolution reaction exothermic? es Why? The ran reultd in heet increese H0. of the ti= 23.7% っ 』C b. Calculate quH,0, using Equation 1. CmesAt 5486.76 9= 5486.70J joules c. Find AH for the reaction as it occurred in the calorimeter (Eq. 5). 9emcst -6036.3 joules ΔΗ= *49.72 Hho (E 4= 6636.25ご G036.33 A#ニ-4 ,9=Gのムこ (continued on following page) - (G0363))= -G036.3AF

3. Using this data, calculate a value for Kc for the reaction, A. 2.06 x 104 B. 4.84 x 10-3 C. 0.223 D. 4.49 E. 20.2 2 NO(g) + Cl₂(g) 2. NOCI(g) Kc = 3.20 x 10-³ 2 NO2(g) 2 NO(g) + O₂(g) Kc = 15.5 4. Using the data, NOCI(g) + 1/2O2(g) NO2(g) + ½ Cl₂(g) 3 A (g) + 4 B (g) A3B4 (g) calculate a value for Kc for the reaction, 3 A (g) + 4 B -A3B4 (g) 2 AB (g) + AB2 (g) (g) Kc = 25 Kc = 3.75 2 AB (g) + AB2 (g)

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2. Balance the following equation: BaSO4     +     NiCl4     ------>    BaCl2      +      Ni(SO4)2 answers are listed in order - 1st coefficient, 2nd coeficient, etc. and so on.     Group of answer choices a) 1,1,1,1 b) 2,1,2,1 c) 2,2,2,2 d) 1,2,1,2

1.   Balance the following chemical equation: Fe2O3      +   CO    ------>     Fe     +     CO2, answers are listed in order - 1st coefficient, 2nd coeficient, etc. and so on.    (1st one is in front of Fe2O3, 2nd one in front of CO, etc. and so on)  Group of answer choices a) 1,3,3,2 b) 2,3,2,3 c) 1,3,2,3 d) 1,2,2,2

Barium sulphate forms as a precipitate in the following reaction: Ba(NO3)2 + Na2SO4 = BaSO4 + 2NaNO3 When 35g of Ba(NO3)2 is reacted with excess Na2SO4, 27.1g of BaSO4 is recovered by a chemist a) Calculate the theoterical yield of BaSO4 b) Calculate the percentage yield of BaSO4 c) Calculate the percentage error

Balance the following equations. Show all coefficients including "one."

ourses / S21 CHEM_161 / 9 May - 15 May / Final Exam Sections 1, 5, & 6 Calculate the moles of 02 that will be prepared through the decomposition (see balanced reaction) of 4.7 moles of potassium chlorate, KCIO3 2 KCIO3 - 2 KCI + 3 02 Answer: tion pus page - Front Page of Final Exam DOWNLOAD THIS FIRST Jump to. You are logged in as Helena Agyemang Log.out) S21 CHEM 161 P Type here to search Cbp %24 8. 9. backspace 11 Y. D F H. J K

Worksheet No. 3 Title: Hess Law Day: 3 irections: Answer the following. Refer to your handout on pages 6-7 for your guide. 1. Calculate AH for the reaction 4 NH3 ( + 502 (g) + the following data. N2 (0) + O2 (0) N2 (0) + 3 H2 (g) 2 H2 (9) + O2 (g) 4 NO (9 + 6 H20 (ai, from 2 NO (9) 2 NH3 (e) AH = -180.5 kJ AH = -91.8 kJ 2 H20 (a) AH = -483.6 kJ

How much iron oxide (Fe2O3) is needed to make a 500 mg fuel rich mixture of aluminum (Al) and iron oxide that has an equivalence ration of 1.3? What is the actual F/O ratio for this mixture?   Please provide only typed answer solution no handwritten solution needed allowed

Why is it necessary to provide a temperature with the value of Kc when doing a report?

20) What is the value for Kc if [CO] = 0.025, [H2]= 0.013 and [CH3OH] = 0.0028 for the following reaction? %3D CH3OH(g) =CO(g) +2 H2(g) A) 0.12 В) 1.5 х 10-3 C) 9.1 x 10-7 D) 6.6 × 102 E) 8.6

Please help thank you this is analytical chem

Perform the following calculations to the correct number significant figures. (23.4813 x 2.52) + 374.99

Cl2 FeCl3 H₂ (excess Ni

Molten iron and carbon monoxide are produced in a blast furnace by the reaction of iron(lI) oxide and coke (pure carbon). The reaction is: Fe203 + 3 C ---> 2 Fe + 3 CO If 25.0 kilograms of pure Fe203 is used, how many kilograms of iron can be produced? Paragraph В I U v A + v の EQ Lato (Recom... 19px ... Record Video Add a File Record Audio -13°C 99+

The below reaction is the chemical process of silver tarnishing over time: 4??(?)+2?2?(?)+?2(?)⟶2??2?(?)+2?2?(?)Fill in the blanks below with the correct responses: The reaction above is a(n)       _______  reaction. The Ag (s) reactant has an oxidation number of                                . The silver in the product Ag2S (s) has an oxidation number of____                                . The oxidation number of the sulfur in the H2S (g) reactant is ______                             .    ______   electrons are transferred in the overall reaction above. The element which is reduced is the                                   . The reactant   _______          is the oxidizing agent in this reaction.

2. Given the equation: KMNO4 + KCI + H2SO4 - MnSO4 + K2SO4 + H2O + Cl2 Determine a) Limiting Reactant if 50 grams of KMNO4, 100 grams of KCI and 75 grams of H2SO4 are given b) Theoretical amount of M.SO4 and c) percent excess reactant. MW: K= 39.10, Mn = 54.94, CI = 35.45, S = 32, Fe = 55.85

3 Which is the reducing agent in the combustion of methanol? 10.01 E CH3OH + O2 H₂O + CO2 a) 02 b) H₂O $ c) CH3OH O d) CO₂ H A R LL % 5 T CF B Y H W P 30 Rain... 9:15 PM 11/29/202

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KEŚLER SCIENCE Draw a model with shapes to represent the total number of OUTPUTIllustrate It! STATION atoms in the chemical equation: SO3 + H20 > H,SO4 See the next page for help on inserting pictures into the page. Go to Image Help ENotes 品 响 85% 5:47 11/11/ DELL F3 F4 F5 F6 F7 F8 F9 F10 F11 PrtScr F12 Insert Home End Del 2# $ & 4 Backs 6 8 9. E Y P { D J K L N Alt Ctrl Page Up

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What is A Gᵒ for the reaction of iron(II) ions with one mole of permanganate ions? (F= 96,500 C.mol-1) MnO4¯(aq) + 8H¹(aq) + 5e¯ = Mn²+ (aq) + 4H₂O(1) Fe³+ (aq) + e- %media:chapter18_19.jpg% Fe2+ (aq) E'= 1.51 V E°= 0.77 V

For the following reaction, CO(g) H₂O(g) →CO₂ (9) a. Write the Kc expression for this reaction. b. If a 1.00L vessel is charged with 0.250 moles of CO, 0.250 moles of H₂0, 0.750 males of CO₂, and 0.750 males of H₂, what is the value of Q? + H₂ (9) Kc = 1.845 c. In which direction does the reaction progress to establish equilibrium? d. What are the equilibrium concentration of all species?

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Given the following information, calculate the % recovery of copper. Volume of original copper containing solution=20.2ml Concentration of original copper containing solution=25.125 g copper per L Mass of precipitated copper=0.469g

Calculate the solubility at 25 °C of Ni(OH), in pure water and in a 0.0080 M NaOH solution. Round both of your answers to 2 significant digits. solubility in pure water: solubility in 0.0080 M NAOH solution: