Based on the following N2 + 3H2 ---> 2NH3. When 298.03 g of N2 reacts how many grams of NH3 are produced? (3-5 sig figs; report to two decimal places) g N2 --> mol N2 --> mol NH3 --> g NH3 Species MM, g/mol N2 28.01 H2 2.02 NH3 17.03
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Q: ( avestion) J - What mass 15.0 of NH3 of №₂ and 12.5g of H₂ is produced ??? are reacted,
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- Done < HIIL Attempts done: 0/2 O Zn²+ O Zn O Zn²- O Zn+ What is the most common oxidation state for zinc? > AA A practice.flatworld kn Read the related chapter ? View available hints Report an errorA 0.4852g sample of an iron ore was dissolved in acid to the 3+ state, then precipitated as Fe2O3 x H2O. The pp was filtered, washed and calcined to Fe2O3, which gave a weight of 0.2481g. Calculate the Fe % in the sample.Pls give with reason, the type and name of the reaction.
- Mo in a 0.2711g sample was precipitated giving 1.1682g of (NH4)2PO4.12 MoO3. Find the percentage Mo , P (at wt = 30.97), N=14,Mo=95.9,H=1,O=16An impure sample of Na3PO3 weighing 0.1 g is dissolved in 35 mL of water. A solution containing 45 mL of 3% w/v HgCl2, 30 mL of 10% w/v sodium acetate, and 10 mL of glacial acetic acid is then prepared. After digesting, filtering, and rinsing the precipitate, 0.2857 g of Hg2Cl2 is obtained. Report the purity of the original sample as % w/w Na3PO3.The mercury in a 0.8142-g sample was precipitated with an excess of paraperiodic acid, H5IO6: 5 Hg 2+ + 2 H5IO6 ---> Hg5(IO6)2 (s) + 10 H + The precipitate (MW = 1448.8 g/mol) was filtered, washed free of precipitating agent, dried, and weighed, and 0.4114 g was recovered. Calculate the a) % Hg (200.6 g/mol) b) % Hg2Cl2 (472.1 g/mol)
- The use of silica to form slag in the production of phospho-rus from phosphate rock was introduced by Robert Boyle morethan 300 years ago. When fluorapatite [Ca₅(PO₄)₃F] is used inphosphorus production, most of the fluorine atoms appear in theslag, but some end up in toxic and corrosive SiF₄ (g).(a) If 15% by mass of the fluorine in 100. kg of Ca₅(PO₄)₃F forms SiF₄, what volume of this gas is collected at 1.00 atm andthe industrial furnace temperature of 1450.°C?(b) In some facilities, the SiF₄ is used to produce sodium hexa-fluorosilicate (Na₄SiF₆) which is sold for water fluoridation: 2SiF₄(g)+Na₂CO₃(s)+H₂O(l) →Na₂SiF₆(aq)+SiO₂(s)+CO₂(g)+2HF(aq) How many cubic meters of drinking water can be fluoridated toa level of 1.0 ppm of Fusing the SiF₄ produced in part (a)?Excessive nutrients dumped into waterways can create “algae blooms” that rapidly consume all of the dissolved O2 and trigger production of enough H2S to create “dead zones” like the ones that exist off the coast of Denmark and in the Gulf of Mexico immediately south of the Mississippi River delta. a. Since Group 16 element substitution is a recurring theme in that Group’s chemistry –e.g., oxygen substituting for Se and Te in the production of H2Se and H2Te, respectively –maybe molecular oxygen (O2) could be bubbled into these dead zones and react with the H2S.Write out a balanced chemical equation for the reaction between H2S and O2 to form elemental sulfur (S8) as a product that would precipitate out. b. Using bond dissociation energies, calculate if this reaction would be thermodynamically favorable. c. If your answer to part (b) is “yes”, do you think that simply bubbling O2 into these waters would work? Justify your answer.56g of the coal was kjeldahlized and NH3 gas evolved was absorbed in 50 ml of 0.1 N sulphuric acid. After absorption, the excess acid required 6.25 ml of 0.1 N NaOH for exact neutralization. 2.60g of the coal sample in a quantitative analysis gave 0.1755 g of BaSO4. Calculate the percentage of nitrogen and Sulphur in coal sample.
- The molecular weight of hemoglobin is 64,500 daltons (= g mol-1). A. How much oxygen can be bound per g of hemoglobin? Express the values as mL per g of hemoglobin, where mL is the volume of O2. R =0.082 L atm mol-1 oK-1, oK =273 + oC. The molar volume of O2 is given as V = nRT/P where P = 1 atm and n= 1 mol. (Hint: 1.0 mol x 0.082 L atm mol-1 oK-1 x 273.2 oK / 1 atm = 22.4 L mol-1) (Hint: The number of moles of O2 that can be bound per g of hemoglobin is 4 x the moles of Hb in 1 g). B. The blood in a person contains 15 g of hemoglobin per 100 ml blood. How much oxygen does the blood contain at 95 mm Hg if hemoglobin is 98% saturated and the solubility of O2 is 0.003 mL dL-1 mmHg-1? (Hint: Total O2 content = HbO2 + free dissolved O2) C. Suppose the venous PO2 is 40 mm Hg, and that hemoglobin is 75% saturated at this point. What is the oxygen content of venous blood? D. Suppose the cardiac output is 5 L min-1. Calculate the oxygen delivery to the tissues from B and C. (Hint: Rate of…A. 1.4639 g sample of limestone was analyzed for Fe, Ca and Mg. The iron was determined as Fe2O3, yielding 0.0357 g Calcium was isolated as CaSO4, yileding a precipitate of 1.4058 g and Mg was isolated as 0. 0627 g of MgP2O7. Report the amount of Febas %w/w Fe2O3, Ca as %w/w CaO and Mg in the limestone sample as % w/w MgOkeAssignment/takeCovalentActivity.do?locator=assignment-take n progress Q Search 40 eaction is Submit Answer In the following equation for a chemical reaction, the notation (s), (I), or (g) indicates whether the substance indicated is in the solid, liquid, or gaseous state. 2NO(g) + 2H₂(g) →→→ N₂(g) + 2H₂O(l) + energy Identify each of the following as a product or a reactant: NO(g) H₂0(1) H₂(g) N₂(g) When the reaction takes place energy is V2 7 L Retry Entire Group = 18 + Use the References to access important values if needed for this question. fg 0 OWLv2 | Online teaching and lear X hp 9 8 more group attempts remaining f10 MO f11 PAI + 112 G ins prt sc Ⓡ ✰ FRIEVIDUS Next> ^ @ ¹0 delete backspace home lock 5:- 5/14