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How would you make 350 mL of 26% (w/v) NaCl?

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  1. How would you make 350 mL of 26% (w/v) NaCl? Be sure to include final volume of water needed. Explain
  2. What does 10% (w/v) NaCl mean? Explain
  3. You have a stock solution of 25X Buffer. How would you prepare 500 mL of TAE Buffer at working concentration (1X) from the 25X stock? Explain
  4. what is the density in g/L of neon at standard temperature and pressure (STP)? Explain
  5. An average dairy cow produces 10896 grams of methane gass, CH4 each year. What volume of CH4 is produced at 25 degrees celsius and 740 mmHg? (Hint: convert grams to moles of CH4) explain
  6. Determine the oxidation number of each element : a) N2 N=_____, B) H2SO4 H= ____, S=_____,O=_______ C) PCl3 P=_____, Cl=______ D)HClO4 H=____, Cl=_____, O=_______
  7. you will fill an inflated balloon with 18 grams of solid CO2 (dry ice, M= 44.0 g/mol.) What volume will dry ice occupy when it vaporizes at 25 degrees celsius and 1.02 at,? The balloon has capacity of 6.5 liters, will it pop?
  8. Determine which of the following has the longest bond length? A) H-H B)F-F C) Cl-Cl D) Br-Br E) I-I
  9. Draw the lewis dot structure for each of the following molecules? a) _N_OF B)H2 _C_O
  10. determine the lewis structure , Vespr, and name of the shape for following? a) _C_H2O B)BeCl2
  11. Determine the bond energy of the H-Cl bond given in the following: The bond energy of H-H bond is 434 kJ/mol and the bond energy of the Cl-Cl bond is 232 kJ/mol
  12. Determine which of the molecules below contain polar covalent bonds and use the appropriate symbols to represent the positive and negative poles: a) H-F b) N-N C)H-O-H D) H-Cl

Can you explain the process of Glycolysis?

Question Can you explain the process of Glycolysis?

Find the standard reduction potential for the half-reaction: X

Question Find the standard reduction potential for the half-reaction:                             X é —-> X  given that Cu 2X —-> Cu2 2X Eo = 0.46 V                         a)                                             0.12 V                                                          b)                                            -0.12 V                                                          c)                                             0.80 V                                                          d)                                            -0.80 V                                                                                                                                                          For question above, what does “X” represent?                                                       a)                                            Tin                                                     b)                                            Lead                                                  c)                                            Cobalt                                               Silver        

For the following problem, show all work and units (I-C-E

Question For the following problem, show all work and units (I-C-E Table if required): style=”background-color:transparent;color:rgb(0,0,0);”>The Ka for acetic acid, CH3COOH, is 1.8 x 10-5 . What is the [H3O ] for a 0.350 M solution of acetic acid? Also, what is the pH of the solution?CH3COOH H2O ↔ H3O CH3COO-

22. How many moles of gas are in 1.0 L

Question 22. How many moles of gas are in 1.0 L bottle of air at a pressure of 2.0 atm and a temperature of 20°C? (Ideal gas constant = 8.31 J/mol K OR 0.0821 L atm / mol K)

For the following two problems, use the following balanced reaction:

Question For the following two problems, use the following balanced reaction: N2 3H2 → 2NH3a. How many liters of H2 are needed to react with 2.0 L of N2 at STP? b. How many grams of NH3 can be produced from 4.0 L of H2 at STP? c. A tire’s pressure is 30 psi when 0.40 mol of air fill it at 100 K. If the temperature rises to 300 K and 0.20 mol of air are let out of the tire, what is the new pressure?

How many milliliters of a 6 M HCl solution do

Question How many milliliters of a 6 M HCl solution do you need to make 1 L (1000 mL) of 0.5 M HCl?

You want to react to two 1-Liter gas samples in

Question You want to react to two 1-Liter gas samples in a sealed flask but you want the reaction to proceed very SLOWLY. To accomplish accomplish this, you should: a. Increase the concentration of each gas. b. Keep the flask. c. Use a larger flask. d. All of these e. None of these.

2H2 style=”color:rgb(0,0,0);background-color:transparent;”>(g) O2 ↔ 2H2O(g) Reaction is highly exothermicPart

Question 2H2 style=”color:rgb(0,0,0);background-color:transparent;”>(g)  O2 ↔ 2H2O(g) Reaction is highly exothermicPart a: When the reaction above reaches equilibrium, which of the following will always be equal?: The rate of product formation equals the rate of reaction formation, the concentration of product equals concentration of reactants, both of these, or none of these?Part b: Which way will this reaction shift if the reaction container is heated?Part c: Which way will this reaction shift if the volume of the container is decreased?Part d: Which way will this reaction shift if you add more oxygen?Part e: Which way will this reaction shift if you take away the water molecule as it is produced?Part f: The equilibrium constant (Keq) for this reaction tells you what?

Samples of two bases, PCl3 style=”background-color:transparent;color:rgb(0,0,0);”> and Cl2, are reacted

Question Samples of two bases, PCl3 style=”background-color:transparent;color:rgb(0,0,0);”> and Cl2, are reacted together in a flask to make gaseous  PCl5 the balanced reactions below. The initial concentration of  PCl3 is 0.10 M and the initial concentration of Cl2 is 0.20 M.At the very beginning of the reaction, what is the concentration of PCl5 in the flask?When equilibrium is reached, the concentration of PCl5  is 0.03 M. What are the equilibrium concentrations of PCl3 and Cl2?

I need some help with find the half-reactions for the

Get college assignment help at Smashing Essays Question I need some help with find the half-reactions for the oxidation-reduction reaction for Fe(C2H3O2)2 H2O2 = Fe(C2H3O2)3

What is the concentration of H2SO4 if 10.0 mL of

Question What is the concentration of H2SO4 if 10.0 mL of it will neutralize 20.0 mL of 1.0 M NaOH?NOTE: 1 H2SO4 2NaOH → 2HOH Na2SO4

style=”background-color:transparent;color:rgb(0,0,0);”>Use the diagram of the voltaic cell to answer each

Question style=”background-color:transparent;color:rgb(0,0,0);”>Use the diagram of the voltaic cell to answer each of the following questions.Part a: The electrons will flow where?Part b: Which ½ is occurring at the anode?Part c: Which electrode will gain mass as a result of this reaction?Part d:  What does the proper ½ reaction involving N look like?NO3- Ag → NO2- Ag Part e: In the reaction above, what species is being reduced ATTACHMENT PREVIEW Download attachment Salt.PNG

In Discussion # 2, you determined the theoretical enthalpy of

Question In Discussion # 2, you determined the theoretical enthalpy of your explosive reaction. This is can also be termed the heat of explosion, but when it is termed heat of explosion, the units are traditionally kJ/kg of substance. Convert your enthalpy of reaction (kJ/mol) to heat of explosion (kJ/kg) using the molar mass of your explosive. List that value here and use it to calculate the explosive energy of 5.00 kgExplosive is TATB —> Enthalpy is -154kJ/mol

In Discussion #1, you calculated the volume of gas that

Question In Discussion #1, you calculated the volume of gas that your explosive would produce if 1 g of it was used, assuming standard temperature and pressure (STP)and any water produced in the gaseous state. Is this actually accurate, as the gas is usually heated as a result of the explosion, resulting in a much larger volume of gas? But what temperature will the gas reach? Calculate the final volume of the gas produced from 1.00 g of your explosive using Charles’ Law, and assuming your explosion reaches a temperature of 3000 K.   Remember Charles’ law? V1/T1 = V2/T2volume of gas from previous answer =0.78L

Please explain steps (like how cathode and anode are determined

Question Please explain steps (like how cathode and anode are determined and calculation steps) src=”/qa/attachment/9101715/” alt=”practise question 4.png” /> ATTACHMENT PREVIEW Download attachment practise question 4.png For each of the following cells, use the Nernst equation and the data below, as needed, to calculate: i. the cell potential, Ecell ii. the thermodynamic equilibrium constant, K, for the cell reaction, when the cell reaction is balanced using the smallest whole number coefficients. Enter your answers with 3 significant digits. Do not include units. Enter scientific notation as 1.23E4. Note: 1 M = 1 mol L-1 (a) Mn(s) | Mn2 (aq, 0.350 M) | | Cr3 (aq, 0.190 M), Cr2 (aq, 0.480 M) | Pt(s) Ecell = Number K = Number (b) Mg(s) | Mg2 (aq, 0.0600 M) | | [AI(OH)4] (aq, 0.280 M), OH-(aq, 0.01000 M) | Al(S) Ecell = Number V K = Number Half reaction E / V Cr2072-(aq) 14 H*(aq) 6 e- = 2 Cr3 (aq) 7 H20(1) 1.33 Mn04 (aq) e- – Mn042-(aq) 0.56 2 H ( aq) 2 e- – H2(8) 0.000 Cr3 (aq) e- – Cr2 (aq) -0.424 Cr2 (aq) 2e- – Cr(s) -0.90 Mn2 (aq) 2 e- – Mn(s) -1.18 Al(OH)4 (aq) 3 e- – Al(s) 4 OH-(aq) -2.310 Mg2 (aq) 2e- – Mg(s) -2.356 Mg(OH)2(S) 2 e- – Mg(s) 2 OH (aq) -2.687

45.0 grams of F2 react according to the following balanced

Question 45.0 grams of F2 react according to the following balanced chemical equation: I2 2Naf. As a result of this reaction ??? grams of I2 are produced. How would I figure this out?

Please write out all steps and explain how cathode and

Question Please write out all steps and explain how cathode and anode were identified. alt=”practise question 5.png” /> ATTACHMENT PREVIEW Download attachment practise question 5.png For the electrochemical cell below, the half-cell on the left is the anode and the cell potential is 0.178 V at 25 .C. What is the concentration of H*, x, in mol L-1? Note: The symbol M is an abbreviation for mol L-1. Pt(s) | V2 (aq, 0.720 M) , V3 (aq, 0.650 M) | | H*(aq, XM ) | H2(g, 1.10 bar) | Pt(s) Half reaction E /V 2 H (aq) 2 e- – H2(8) 0.000 V3 (aq) e- – V2 (aq) -0.255 Enter a value accurate to 3 significant figures. X = [H*] = Number mol L-1

Question 1 style=”color:rgb(73,76,78);”>Hydrolysis of the disaccharide sucrose gives the following

Question Question 1   style=”color:rgb(73,76,78);”>Hydrolysis of the disaccharide sucrose gives the following monosaccharides: 1)  fructose and ribose. 2)  fructose and glucose. 3)  ribose and glucose. 4)  ribose and galactose. 5)  fructose and lactose. Question 2  Iodine can be used to detect the presence of __________ in solution. 1)  maltose. 2)  fructose. 3)  starch. 4)  galactose. 5)  xylose. Question 3  In the R- isomer of glucose, the -OH group furthest from the carbonyl is written ___________ of a Fischer projection. 1)  on the left of the top chiral carbon. 2)  on the right of the top chiral carbon. 3)  on the left of the middle chiral carbon. 4)  on the left of the bottom chiral carbon. 5)  on the right of the bottom chiral carbon. Question 4  The monosaccharide that is contained in both cellulose and starch is: 1)  glucose. 2)  galactose. 3)  fructose. 4)  lactose. 5)  sucrose. Question 5 Glucose does not undergo hydrolysis because it is a 1)  aldose. 2)  hexose. 3)  reducing sugar. 4)  monosaccharide. 5)  disaccharide. Question 6  What type of reaction would result in soap? 1)  hydrogenation 2)  reduction 3)  hydration 4)  oxidation 5)  saponification Question 7 Unsaturated fatty acids have lower melting points than saturated fatty acids because 1)  they have fewer hydrogen atoms. 2)  they have more hydrogen atoms. 3)  their molecules fit closely together. 4)  the cis double bonds produce a shape that reduces contact between molecules. Question 8 Polyunsaturated fatty acids contains more than one 1)  carboxyl group. 2)  hydroxyl group. 3)  carbonyl group. 4)  long carbon chain. 5)  double bond. Question 9 Lipids are compounds that are soluble in 1)  distilled water. 2)  normal saline solution. 3)  glucose solution. 4)  nonpolar solvents. 5)  oxygen. Question 10  A lipoprotein’s main function in the body is to 1)  dissolve polar lipids for excretion. 2)  metabolize lipids into new substances. 3)  dissolve polar lipids in urine. 4)  transport nonpolar lipid to body cells. 5)  store lipids in the tissues. Question 11  Sucrase, the protein that catalyzes the hydrolysis of sucrose, would be classified as a ________ protein. 1)  transport 2)  hormonal 3)  enzyme 4)  structural 5)  contractile Question 12 What kinds of interactions are not part of tertiary protein structure? 1)  α-helix 2)  disulfide bonds 3)  hydrophilic interactions 4)  salt bridges 5)  hydrophobic interactions Question 13 An enzyme-catalyzed reaction ___________ than reactions that are not catalyzed. 1)  uses less substrate. 2)  produces different products. 3)  occurs at a faster rate. 4)  requires more energy. 5)  requires a higher temperature. Question 14 If an amino acid is in its zwitterion form, the amine end is 1)  positively charged. 2)  negatively charged. 3)  neutral. 4)  soluble in a nonpolar solvent. 5)  attached to an amine. Question 15 The bonds that link amino acids in a protein are 1)  ester bonds. 2)  ether bonds. 3)  peptide bonds. 4)  glycosidic bonds. 5)  sulfide bonds. Question 16 The reactant is an enzyme catalyzed reaction is called the: 1)  substrate. 2)  cofactor. 3)  coenzyme. 4)  isozyme. 5)  allostere. Question 17  Which of the following is a primary protein structure? 1)  β-sheet 2)  Ser-Met-Ala-Gly-Ile-Gly 3)  disulfide bond 4)  α-helix 5)  hydrophobic interactions Question 18 The following are all characteristic of a competitive inhibitor except: 1)  It occupies the active site. 2)  It cannot be converted to products. 3)  It has a structure similar to the substrate. 4)  Increasing the substrate concentration can reverse competitive inhibition. 5)  It binds to the enzyme at a site remote from the active site. Question 19  The function of the enzyme-substrate complex is to 1)  lowers the energy of the products. 2)  lowers the energy of the substrate. 3)  changes the concentration of the substrate. 4)  decreases the activation energy for the reaction. 5)  changes the possible product formed. Question 20 What is the process that  occurs when heat, acids, bases, or heavy metal ions cause a loss of biological activity of a protein? 1)  denaturation 2)  saponification 3)  hydrogenation 4)  amidation 5)  esterification Question 21 What type of carbohydrate is pictured below? an R-isomer of a monosaccharide an L-isomer of a monosaccharide a beta isomer of a monosaccharide an alpha isomer of a monosaccharide Question 22 What type of lipid is shown below? steroid wax fatty acid tryacylgliceride Question 23  What type of lipid is shown below? steroid wax fatty acid tryacylgliceride Question 24 What type of lipid is shown below? steroid wax fatty acid tryacylgliceride Question 25 Which of the following lipids would have the lowest melting point?a) b) c) Question 26 Which form of ion is the following amino acid shown? zwitterion anion cation isoanion Question 27 What type of amino acid is shown below? acidic amino acid polar amino acid nonpolar amino acid basic amino acid Question 28 What type of amino acid is shown below? acidic amino acid polar amino acid nonpolar amino acid basic amino acid Question 29  Which of the following are produced by the hydrolysis of maltose? One molecule each of D-galactose and L-glucose Two molecules of L-fructose One molecule each of D-glucose and D-fructose Two molecules of D-glucose One molecule each of L-galactose and D-fructose Question 30 Which of the following disorders results from the absence of an enzyme needed to convert galactose to glucose? Lactose intolerance Glucose-galactose malabsorption Galactosemia Hypoglycemia Phenylketonuria Question 31  Maltose is sweeter than sucrose. True False Question 32  Which of the following reagents is used to detect the presence of starch in a solution? Tollen’s reagent Iodine Potassium dichromate Benedict’s solution Copper(II) acetate Question 33 Which of the following monosaccharides is a ketohexose? Fructose Glucose Xylose Galactose Ribose Question 34 Starch is more easily digested than dextrins and is therefore used extensively in the commercial preparation of infant foods. True False Question 35 Which of the following types of glycosidic linkages is responsible for the branching in the structure of amylopectin?Question 35 options: α-1,4 glycosidic linkages β-1,6 glycosidic linkages α-1,3 glycosidic linkages α-1,6 glycosidic linkages α-1, β-2 glycosidic linkages Question 36 The hydrolysis of fats and oils in the presence of a base is used to make soap and is called _____. saponification transesterification desiccation olefination glycosidation Question 37  Pure fats and oils are colorless, odorless, and tasteless. True False Question 38  Cerebrosides resemble sphingomyelins but have a sugar unit in place of the choline phosphate group. True False Question 39  The major function of bile salts is to aid in the digestion of dietary lipids. True False Question 40  A triglyceride is called a fat if:Question 40 options: it has no carbon-to-carbon double bonds in its structure. it is a liquid at room temperature. it has three different fatty acid units attached to glycerol. it has three saturated fatty acid units attached to glycerol. it exists as a solid at 25° C. Question 41 Peripheral proteins are a type of membrane proteins that span the hydrophobic interior of the bilayer. True False Question 42  _____ are lipids with four fused ring structures. Sphingolipids Phospholipids Steroids Enzymes Gangliosides Question 43  _____ are double strata of lipids arranged so that the hydrophobic tails are sandwiched between an inner surface and an outer surface consisting of hydrophilic heads. Bilayers Micelles Emulsions Transferomes Suspensions Question 44  Which of the following refers to the fixed arrangement of the polypeptide backbone? Quinary structure Quaternary structure Tertiary structure Secondary structure Primary structure Question 45  The structure of an amino acid allows it to act as both an acid and a base, but not simultaneously.Question 45 True False Question 46  Which of the following proteins performs the biological function of providing strength and structure? Hemoglobin Ovalbumin Keratin Myosin α-Amylase Question 47 Humans can synthesize only about half of the needed amino acids and the remainder must be obtained from the diet. True False Question 48  A(n) _____ is a molecule that contains an amino group and a carboxyl group.Question 48 options: amide nitrile amine amino acid imine Question 49  What denaturation effect do alkaloid reagents have on proteins? They cause protein atoms to vibrate more rapidly and crystallize the protein. They combine with positively charged amino groups in proteins and disrupt ionic bonds. They engage in intermolecular hydrogen bonding with protein molecules, strengthening intramolecular hydrogen bonding within the protein. They supply kinetic energy to protein molecules and disrupt relatively strong hydrogen bonding and dispersion forces. They form strong bonds with the carboxylate anions of the acidic amino acids or SH groups of cysteine, disrupting ionic bonds and disulfide linkages. Question 50 Which of the following amino acids has the highest isoelectric point? Lysine Threonine Histidine Arginine Alanine Attachment 1 Attachment 2 Attachment 3 Attachment 4 Attachment 5 Attachment 6 Attachment 7 Attachment 8 ATTACHMENT PREVIEW Download attachment 00.png ATTACHMENT PREVIEW Download attachment 1.jpg ATTACHMENT PREVIEW Download attachment 2.jpg ATTACHMENT PREVIEW Download attachment 3.png ATTACHMENT PREVIEW Download attachment 4.png ATTACHMENT PREVIEW Download attachment 6.png ATTACHMENT PREVIEW Download attachment 7.png ATTACHMENT PREVIEW Download attachment 8.png

Just need some assistance with these questions, would appreciate the

Question Just need some assistance with these questions, would appreciate the help!12d style=”color:rgb(0,0,0);”>1)Here are the solubilities of a particular solute at two different temperatures.Temperature (c) Solubility (g/100 g h2O)20.0 44.830.0 68.9Suppose that you have made a saturated solution of this solute using 51.0 g of water at 20.0 °C. How much more solute can you add if the temperature is increased to 30.0 °C?g?2)At 25 °C only 0.0240 mol of the generic salt AB3 is soluble in 1.00 L of water. What is the Ksp of the salt at 25 °C?AB3(s) –><— A^3 (aq) 3B^- (aq)Ksp?

The first ionization energy of cesium is 376 kJ mol1.

Question The first ionization energy of cesium is 376 kJ mol1. What is the maximum wavelength of light that can be used to ionize a cesium atom?A. 5.281031 mB. 1.761030 mC. 7.97102 mD. 3.18107 m*E. 1.50104 m

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