explain how you determined the number of moles of cn in each compound

A:It is an basic Organic Reaction mechanism. The dye has a percent composition of 75.95% C, 17.72%N, and 6.33% H by mass with a molar mass of about 240g/mol. Then, add together the atomic weight of each of the atoms in the formula, which you can find using the periodic table. This will yield the molecular formula. We do not have enough information. For first order reactions the relation between rate constant and half life is expressed as This article has been viewed 166,536 times. Reaction Type: Rate of formation What is the Henry's Law, A:The equation for Henry's Law is as follows: in the. 1 Why or why not? At a certain temperature and pressure, a 1-L volume holds 8.93 g of this fluorocarbon, whereas under the same conditions, the 1-L volume holds only 1.70 g gaseous fluorine (F2) . stream A) Na2O The initial number of moles of H2 = 0.050 mol, Q:PROBLEM 16-16 4C3H5(NO3)3, A:We have to calculate the number of N atom in the formula, Q:How many oxygen atoms are in: Determine the number of moles of the compound and determine the number of moles of each type of atom in, (d) 78.452 g of aluminum sulfate, Al2(SO4)3, Number of moles of K = 0.0179 mol x 1 = 0.0179 mol, Number of moles of Br = 0.0179 mol x 1 = 0.0179 mol, Number of moles of H = 0.0015 mol x 3 = 0.0045 mol of H, Number of moles of P = 0.0015 mol x 1 = 0.0015 mol of P, Number of moles of O = 0.0015 mol x 4 = 0.006 mol of O, Number of moles of Ca = 255 mol x 1 = 255 mol of Ca, Number of moles of C = 255 mol x 1 = 255 mol C, Number of moles of O = 255 mol x 3 = 765 mol of O, Number of moles of Al = 2 x 0.229 mol = 0.458 mol of Al, Number of moles of S = 3 x 0.229 mol = 0.687 mol of S, Number of moles of O = 12 x 0.229 mol = 2.748 mol of O, Number of moles of C = 0.0061 x 10 -4 mol x 8 = 0.0488 x 10 -4 mol of C, Number of -moles of H = 0.0061 x 10 -4 mol x 10 = 0.061 x 10 -4 mol of H, Number of moles of N = 0.0061 x 10 -4 mol x 4 = 0.0244 x 10 -4 mol of N, Number of moles of O = 0.0061 x 10 -4 mol x 2 = 0.0122 X 10 -4 mol of O, Number of moles of K = 0.0179 mol x 1 = 0.0179 mol, Number of moles of Br = 0.0179 mol x 1 = 0.0179 mol, Number of moles of H = 0.0015 mol x 3 = 0.0045 mol of H, Number of moles of P = 0.0015 mol x 1 = 0.0015 mol of P, Number of moles of O = 0.0015 mol x 4 = 0.006 mol of O, Molecular weight of CaCO3 = 40 + 12 + 3 x 16 = 90 g/mol, Number of moles of Ca = 255 mol x 1 = 255 mol of Ca, Number of moles of C = 255 mol x 1 = 255 mol C, Number of moles of O = 255 mol x 3 = 765 mol of O, Number of moles of Al = 2 x 0.229 mol = 0.458 mol of Al, Number of moles of S = 3 x 0.229 mol = 0.687 mol of S, Number of moles of O = 12 x 0.229 mol = 2.748 mol of O, Mass = 0.1250 mg of C8H10N4O2 = 1.2 x 10 -4 g, Number of moles of C = 0.0061 x 10 -4 mol x 8 = 0.0488 x 10-4 mol of C, Number of moles of H = 0.0061 x 10 -4 mol x 10 = 0.061 x 10-4 mol of H, Number of moles of N = 0.0061 x 10 -4 mol x 4 = 0.0244 x 10-4 mol of N, Number of moles of O = 0.0061 x 10 -4 mol x 2 = 0.0122 X 10-4 mol of O. For example, 1 mol of sodium (Na) has a mass of 22.9898 g (the mass on the periodic table). A:Draw the step by step mechanism of the given organic reaction. Explain how you determined the number of moles of CN-in each compound. It is always a good idea to estimate the answer before you do the actual calculation. Finally, multiply the entire empirical formula by this ratio to yield the molecular formula. tetrahydride (CH). C3H5(NO3)3 Nam

sectetur adipiscing elit. Thanks to all authors for creating a page that has been read 166,536 times. For example if you have 17.0 mol of NaCl, then. What integer represe . Next, divide the molecular weight by the empirical formula weights to come up with a ratio. In Daltons theory each chemical compound has a particular combination of atoms and that the ratios of the numbers of atoms of the elements present are usually small whole numbers. ATTEMPT TO SOLVE YOUR PROBLEM: For example, cans of soda come in a six-pack, eggs are sold by the dozen (12), and pencils often come in a gross (12 dozen, or 144). c.. C To calculate the number of molecules in the sample, we multiply the number of moles by Avogadros number: \( molecules\; of\; ethylene\; glycol=0.5639\; mol\left ( \dfrac{6.022\times 10^{23}}{1\; mol} \right ) \), For 75.0 g of CCl3F (Freon-11), calculate the number of. How many moles of aluminum do you need to make a six-pack of cans. Fe 3+(aq) + SCN -(aq) <==> [FeSCN 2+] ( aq) At the very beginning of the reaction how much Fe 3+ will be present in the flask initially? H20, Q:5- The cover of the car's engine is called a hood. Q:The complete combustion reaction of solid benzoic acid, CHCOOH 0.324 Calculate the change in entropy if 3 moles of a gas undergo an isothermal, reversible expansion at 373 K in which the pressure is decreased to 1/3 of its initial value. It is als. Why is molality independent of temperature? 8Z1R%2A8,FnB#e`\3J$|cF'&3F=y$`c&4M@~'*3.qg!$CGV31c!52E=axc.Lfwxgi1j-fF22mGVv;)y*R}|:X In the mentioned questions acid and base are reacting and we have to complete the chemical. The mole is the basis of quantitative chemistry. By using our site, you agree to our. *5Q :>1apH=fj$ {qd B. Is this the correct formula of the compound? ;?(3Oe`10FeaGS(!5'dyH:lm=[&*6_pc=N;@y= 2\X *Response times may vary by subject and question complexity. endobj = 1 mole of water molecules HCI K = Explain why no work is done by the system during this process. Q:In beer's law, what will happen to the molar apsorptivity when the bath length increases to 2 cm., A:Answer: Ball, David W. (david Warren), BAER, Tomas, David W. Oxtoby, H. Pat Gillis, Laurie J. Butler, John C. Kotz, Paul M. Treichel, John Townsend, David Treichel, Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell. x\o (T MuNwfs&9D EG'^pVm=}Y Ld)D)'%{-*jW\. 1.00 mol of an ideal gas, initially occupying 12.2 L at 298 K, expands isothermally against a constant external pressure of 1.00 bar until the pressure of the gas is equal to the external pressure. You would first need to convert each of the gram measurements to moles. It is not so easy. 1 mole zinc = 65.38 grams Mass, A:We have given, Mass of iron ,Fe=20.98g The mole is a unit used to measure the number of atoms, molecules, or (in the case of ionic compounds) formula units in a given mass of a substance. H:SO. This method was, until the invention of the mass spectrometer, the best way of measuring molecular weights of gas molecules. d:f,5 J_~1 O:yGTJ(.2VDuc?&AuvEa+#KYIMHCkdR/DRB3ZUE)>Z3ciZs+h0#wKx1FUc?;8bv-9OaP7Zf+#RiO6S_0D6{l.AW&AOao6HF]kYT-|~Hf,3m$q&7dAXXxN0SDv! nitrous acid The quantity of a substance that contains the same number of units (e.g., atoms or molecules) as the number of carbon atoms in exactly 12 g of isotopically pure carbon-12. As a small thank you, wed like to offer you a $30 gift card (valid at GoNift.com). $('#comments').css('display', 'none'); SIS. g of This is question is based on Beer-Lambert law which gives us reation between molar, Q:How many degrees of freedom Note that for any compound with a ratio of "1," the empirical formula and molecular formula will be the same. we need to explain the product formation, Q:Feedback Explain how you determined the number of moles of CN in each compound. B Taking the atomic masses from the periodic table, we obtain, \( 2 \times atomic;\ mass\;of\:carbon = 2\;atoms \left( {\dfrac{12.011amu}{atom}} \right) = 24.022\;amu\), \( 6 \times atomic;\ mass\;of\:hydrogen = 6\;atoms \left( {\dfrac{1.0079amu}{atom}} \right) = 6.0474\;amu\), \( 1 \times atomic;\ mass\;of\:oxygen = 1\;atoms \left( {\dfrac{15.9994amu}{atom}} \right) = 15.9994amu\). Determine the mass of each of the following: What is the total mass of hydrogen in each of the molecules? OH, A:The carbohydrate molecules in which two monosaccharide units are bonded to each other by an ether, Q:When a 23.4 mL sample of a 0.357 M aqueous hydrocyanic acid solution is titrated with a 0.303 M, A:Well, we will require the Ka value of HCN for the calculation. A:pH isa measure of how acidic/basic water is. Ignore inorganic For compound 2 , A:We need to find tge pH of a 0.0360 M solution of sodium hypochlorite, NaClO. David W. Oxtoby, H. Pat Gillis, Laurie J. Butler, Emil Slowinski, Wayne C. Wolsey, Robert Rossi, Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer, Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste. 2003-2023 Chegg Inc. All rights reserved. Ar Q:Calculate the pH of a 0.0360 M solution of sodium hypochlorite, NaClO. *Response times may vary by subject and question complexity. Multiply the empirical formula by the ratio. B Obtain the atomic masses of each element from the periodic table and multiply the atomic mass of each element by the number of atoms of that element. To go from moles to grams, multiply by the formula mass. Q:Calculate the average activity coefficient of KNO3 in a solution of 0.004 M KNO3 and 0.076 M NaCl. *y0_&]EYQ !kKi}a@ ;Oi{%:awwk <>/XObject<>/ProcSet[/PDF/Text/ImageB/ImageC/ImageI] >>/MediaBox[ 0 0 612 792] /Contents 4 0 R/Group<>/Tabs/S>> The definition of a molethat is, the decision to base it on 12 g of carbon-12is arbitrary but one arrived at after some discussion between chemists and physicists debating about whether to use naturally occurring carbon, a mixture of C-12 and C-13, or hydrogen. In this question mass of solution and mass% of NaCl is given to us and we have to find out, Q:covalent bonds which do not share their electrons equally are called CO A mole of C-12 by definition weighs exactly 12 g and Avogadro's number is determined by counting the number of atoms. To obtain 1 mol of carbon-12 atoms, we would weigh out 12 g of isotopically pure carbon-12. i need all 4 answered pleased. The charged particles vary due to their different mass to charge ratio and are estimated with the help of this difference. When we consider the behavior of gases in Unit 5, we can use the data to calculate the molecular weight of each gas. Please I need the answer in less than a half an hour. You did this calculation and put down the value previously. 2 The herbicide oxyfluorfen can be prepared by reaction between a phenol and A 50.0-g sample of industrial wastewater was determined to contain 0.48 mg of mercury. It is calculated by adding together the atomic masses of the elements in the substance, each multiplied by its subscript (written or implied) in the molecular formula. A:We will Write the molecular and empirical formulas for Freon 112. Start your trial now! formula A) Na2O HTeO3 If the substance is an element then the output of this calculator will also contain the number of atoms of that element hence, it acts as a grams to atoms calculator as well. A:Here , the answer will be option (d), i.e. To go from moles to grams, multiply by the formula mass. CO Would that be a + or a -? solution. Q:How does an SN1 reaction mechanism form answers A and C? How many grams are equal to 2) Calculate the number of moles of oxygen in the sample. AgI What is the total number of atoms in each sample? molarity of sucrose solution = 0.500 (M)mol/L 1.26 $('#pageFiles').css('display', 'none'); Provide products for each, A:The given reactions are simple example of reaction mechanism and organic reagent. Is this the molecular formula or the simplest formula? (1.) $yCc:LE/ImS9C"7Kl,AJ5eLN Find answers to questions asked by students like you. 0.180 Figure 1.7.2 is a flowchart for converting between mass; the number of moles; and the number of atoms, molecules, or formula units. MC Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. If a solution of HF is, Q:Macmillan Learning average mass of sugar in soda is 30.0 g and the total mass is 370.0 g. Phosphorous acid can be prepared from phosphorus triiodide according to the reaction: Deriving the Molecular Formula from an Empirical Formula, {"smallUrl":"https:\/\/www.wikihow.com\/images\/thumb\/b\/b7\/Find-Molecular-Formula-Step-1-Version-2.jpg\/v4-460px-Find-Molecular-Formula-Step-1-Version-2.jpg","bigUrl":"\/images\/thumb\/b\/b7\/Find-Molecular-Formula-Step-1-Version-2.jpg\/aid3408618-v4-728px-Find-Molecular-Formula-Step-1-Version-2.jpg","smallWidth":460,"smallHeight":345,"bigWidth":728,"bigHeight":546,"licensing":"