1. Change the following word equations to chemical equations and then balance it. Write the coefficients at the end of the equations. Given the equation below: Example Hydrogen reacts with chlorine -----> Hydrogen chloride Coeff. 1,1,2 H2 + Cl2 ----- HCI 1. Arsenous Bicarboate -----> Arsenous Carbonate + carbon dioxide + water Coeff. + CO2 + 2. Cobaltic chloride + oxygen -----> Cobaltic chlorate Coeff. + 3. Platinic oxide + carbon dioxide -----> Platinic carbonate Coeff. +

1. Change the following word equations to chemical equations and then balance it. Write the coefficients at the end of the equations. Given the equation below: Example Hydrogen reacts with chlorine -----> Hydrogen chloride Coeff. 1,1,2 H2 + Cl2 ----- HCI 1. Arsenous Bicarboate -----> Arsenous Carbonate + carbon dioxide + water Coeff. + CO2 + 2. Cobaltic chloride + oxygen -----> Cobaltic chlorate Coeff. + 3. Platinic oxide + carbon dioxide -----> Platinic carbonate Coeff. +

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 123QRT

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please help me The aluminum in a 1.200g sample of impure ammonium aluminum sulfate was precipitatedwith aqueous ammonia as the hydrous Al2O3 · XH2O. The precipitate was filtered and ignitedat 100°C to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysisin terms of % Al.
In the common process for the manufacture of nitric acid, sodium nitrate is treated with aq. sulphuric acid containing 95% H2SO4. In order that the resulting "niter cake" may be fluid; it is desirable to use sufficient acid so that there will be 34% H2SO4 by wt in the final cake. This excess H2SO4 will actually be in combination with the Na2SO4 in the cake, forming NaHSO4, although for purposes of computation it may be assumed to be free acid. The cake will contain 1.5% water and the reaction will go to completion, but 2% of the HNO3 formed will remain in the cake. Assume that the NaNO3 used is dry and pure. Calculate per 100 kg of NaNO3 charged: (a) wt and % composition of the niter cake (b) wt of aqueous acid to be used (c) wt of water vapor and nitric acid distilled from the niter cake.
Pure CO2 may be prepared by treating limestone with sulfuric acid. The limestone used in the process contains CaCO3, MgCO3 and inert. The acid used contains 12% H2SO4 by weight The residue from the process had the following composition. CaSO4 – 8.56%; MgSO4 – 5.23%; H2SO4 – 1.05%; Inert – 0.53%; CO2 – 0.12%; H2O – 84.51%; During the process, the mass was warmed where CO2 and H2O were removed. Calculate the following.a) The analysis of lime stone and b) The % excess acid used.
Mass of Na2CO3.H2O (g) = 2.12g (g) Mass of the CaCl2.2H2O (g) = 1.98g Mass of the top funnel + filter paper (g) = 15.85g Mass of top funnel + filter paper + CaCO3 collected (g) = 17.81g CaCl2 + Na2CO3 ==== CaCo3 + 2NaCl Theoretical yield in moles and grams? Moles of reagent in excess left unreacted? Mass of precipitate? Experimental yield? Percent yield?
Assume that 1.00 mL (1.02 g) of crude product mixture is obtained from the reactionbefore the washing steps, and the distribution constant of the product mixture in brine isK = (Cmixture/Cbrine) = 50.0. Assuming that after mixing the product mixture volume isstill 1.00 mL (i.e., the volume lost is small), and the volume of the first brine wash layeris 2.00 mL. What mass (grams) of product mixture is lost (dissolves) in the first brinewash? (See Technique 13.2, p 53.) Show work.
To determine , by gravimetric analysis, the concentration of barium ions (Ba2+) in a given solution, 25.00cm3 of it are pipetted into a beaker and an excess of dilute sulphuric acid is added to it. The precipitate then obtained (BaSO4) is filtered, dried and weighed. The mass of the precipitate is found to be 1.167g Calculate the concentration of barium ions in the solution? (only 2 decimal places). _________Mol/L
The percent nitrogen (N) in a protein sample can be determined by reacting the protein with sulfuric acid to produce ammonium sulfate. The ammonium sulfate is reacted with concentrated sodium hydroxide to form ammonia gas. The ammonia gas is collected by bubbling it through a known volume of standardized hydrochloric acid solution (all of the ammonia reacts in this step, is consumed). The unreacted hydrochloric acid is then back-titrated with standardized sodium hydroxide solution. The reactions involved are shown below: Protein-N + H2SO4 (aq) ⟶⟶ (NH4)2SO4 (aq) 2 NH4+(aq) + 2 NaOH (aq) 2 NH3 (g) + 2 H2O NH3 (g) + HCl (excess) NH4Cl (aq) + HCl (unreacted) HCl (unreacted) + NaOH (aq) NaCl (aq) + H2OA 1.85 g sample of the protein required 25.00 mL of 0.1535 M HCl and 21.55 mL of 0.0986 M NaOH. How many moles of NH3 were consumed by the standardized HCl? A. 8.55 x 10-4 B. 1.71 x 10-3 C. 2.13 x 10-3 D. 3.84 x 10-3 E. 5.97 x 10-3 What is the mass percent nitrogen in…
Please find the CO2 amount and show the calculation: Air composition (apprx) = 80% N2 and 20% O2 (mol basis only)Average molecular weight of Air = (0.8 x 28 + 0.2 x 32) = 29 g/mol (apprx) Math Sample:2kg pure charcoal (12C) is to be burnt completely with air. Find the air, CO2 andN2 amount in kg’s.Solution:C + O2 = CO2 (you must use a balanced equation)Therefore from the mole ratio of the reaction we write,C : O2 : CO2 = 1:1:1and from air composition we gotO2 : N2 : Air = 1:4:5 Given, 2 kg C = 2000 g/ (12 g/mol) = 166.67 mole CTherefore, similar mole of O2 required. So equivalent Air supposed to be 5times than the mole amount of O2 and released N2 will be 4 times than therequired O2. Therefore, Air amount = 5 x 166.67 moles= 833.34 moles= (833.33x29/1000) kg= 24.17 kg air Similarly N2 released amount will be = (166.67 x 4 x 28/1000) kg = 18.67 kgFind CO2 amount by yourself! (Isn’t it 7.34 kg?)
Complete and balance the following acid-base and acid-carbonate reactions. (Use the lowest possible whole number coefficients.) (a) HCl + Ba(OH)2 → (b) HCl + Al2(CO3)3 → (c) H3PO4 + LiHCO3 → (d) Al(OH)3 + H2SO4 →
The concentration of arsenic in an insecticide can be determined gravimetrically by precipitating it as MgNH4AsO4. The precipitate is ignited and weighed as Mg2As2O7. Determine the %w/w As2O3 in a 1.627-g sample of insecticide that yields 106.5 mg of Mg2As2O7.
A 1.963-g sample of an alloy is dissolved in HNO3 and diluted to volume in a 100-mL volumetric flask. Titrating a 25.00-mL portion with 0.1078 M KSCN requires 27.19 mL to reach the end point. Calculate the %w/w Ag in the alloy. (Mwt of Ag = 107.87 g/mol)
Federal regulations set an upper limit of 50 parts per million(ppm) of NH3 in the air in a work environment [that is, 50molecules of NH31g2 for every million molecules in the air].Air from a manufacturing operation was drawn through asolution containing 1.00 * 102 mL of 0.0105 M HCl. TheNH3 reacts with HCl according to: NH3(aq) + HCl(aq)-------->NH4Cl(aq) After drawing air through the acid solution for 10.0 min at arate of 10.0 L/min, the acid was titrated. The remaining acidneeded 13.1 mL of 0.0588 M NaOH to reach the equivalencepoint. (a) How many grams of NH3 were drawn into theacid solution? (b) How many ppm of NH3 were in the air?(Air has a density of 1.20 g/L and an average molar mass of29.0 g/mol under the conditions of the experiment.) (c) Isthis manufacturer in compliance with regulations?