Organic Chemistry Questions

A metal block of iron with a mass of 9.10 g is at 73.6° C. It is added to 99.3 g of water at 13.9 °C. What is the final temperature of the block and the water? The specific heat of iron is 0.450 J/gº c.

Name the nucleotide dAMP with its complete name. Express your answer as an alphanumeric string. For example, ATP is named as adenosine-5'-triphosphate.

In each of the following groups, which element is least reactive? (Consider Periods 1-6.) (Express your answer as a chemical symbol.) a. Group 1: b. Group 7: c. Group 2: d. Group 6:

A nurse decides to move from England to India. The nurse currently makes 46,800 Euros as their annual salary. How much is this salary in Indian Rupees every month? The conversion factor you will need is: 1 Euro = 95.12 Indian Rupees The nurse's salary will be Indian Rupees per month.

Using the symbol of the previous noble gas to indicate the core electrons, write the electron configuration for each of the following elements. a. selenium, Z = 34. b. titanium, Z= 22. c. rubidium, Z = 37.

Given the following balanced equation, determine how many moles of O2 are needed to completely react with 8 moles of K: 4K+0₂ > 2K₂0 4.0 moles 1.0 moles 2.0 moles 3.0 moles

With respect to deoxyribonucleotide metabolism, dATP inactivates NDPK ATP activates ribonucleotide reductase (RNR) dADP inhibits synthesis of dATP all of the above are true none of the above are true

Using the chemical formula CaO + 2 NaCl Na2O +CaCl2, calculate how many moles of CaCl2 you would produce if you used up 5.4 moles of CaO? ->>

A 0.515 g sample of steam at 103.2 "C is condensed into a container with 4.97 g of water at 15.5 °C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18, the specific heat of steam is 2.01, and A Hvap = 40.7 kJ/mol. T₁ =

In the month of August, your electric bill was $145.68. What is the hourly cost of electricity in your home? The hourly cost for August was cents per hour. (Round to 5 decimal places) I

Which statement concerning proteins is not correct? A) Proteins are long, usually folded, chains. B) The shape of a protein molecule determines its function. C) Proteins can be broken down and used for energy. D) Proteins are bonded together, resulting in simple sugars.

Iron(II) sulfate forms several hydrates with the general formula FeSO4 xH₂O, where x is an integer. If the hydrate is heated, the water can be driven off, leaving pure FeSO4 behind. Suppose a sample of a certain hydrate is heated until all the water is removed, and it's found that the mass of the sample decreases by 11.%. Which hydrate is it? That is, what is x?

With respect to breakdown of fat to the two categories of molecules it contains, lipases are essential fatty acids are released it does not require oxygen, NAD, or FAD all of the above are true none of the above are true

Calculate the mass of 2.5 moles of NaOH. (1 points)

Calculate Volume/volume% of a solution made by dissolving 50 ml Ethanol in 250 ml H₂ (1 point formula, 1 pt units, 0.5 pt answer)

Select all examples where the Law of Conservation of Mass is not being followed. 2 NaCl + MgBr2 → 2 NaBr + MgCl2 H₂SO4 + 2 NaOH → Na₂SO4 + 2 H₂O S8(g) + Ag(s)→ 8 AgS Mg3N2(s) + 3 H₂O(1)→ NH3(g) + 3 Mg(OH)2(s)

If the balanced chemical reaction for the formation of Li₂O is 4 Li(s) + O2(g) → 2 Li₂O(s), how many molecules of Li₂O(s) would you produce if you used up 6 atoms of Li(s)? 6 12 2 3

The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H₂O that can be produced by combining 54.4 g of each reactant? 4 NH, (g) + 50₂(g) 4 NO(g) + 6H₂O(g) mass: - g H₂O

Write the structural formula for the product that forms when 1-methylcyclopentene reacts with Br₂ in H₂O. Include stereochemistry in your answer. Draw only one enantiomer. Note: All structures should be drawn with no bonds between carbon and hydrogen.

Place the atoms and/or ions in order increasing atomic radius, electronegativity, effective nuclear charge, electron affinity and first ionization energy. a. Na, Si Cl Atomic radius: Electronegativity: Effective nuclear charge: Electron affinity: First ionization energy:

Which set of quantum numbers is impossible? 2, 1, 0, -1/2 2, 1,-1, +1/2 3, 0, 0, +1/2 3, 0, -1, -1/2 More than one of these is impossible.

What is the frequency of light having a wavelength of 152 nm? (b) What is the wavelength (in meters) of radiation having a frequency of 10.18 × 107 Hz? (This is the type of radiation used by FM radio stations.) (a) Frequency of light: (Enter your answer in scientific notation) (b) Wavelength of radiation:

The atomic radius of metal X is 1.30 x 10² picometers (pm) and a crystal of metal X has a unit cell that is face-centered cubic. Calculate the density of metal X (atomic weight = 42.3 g/mol).

Why might Jeff and other scientists be working on making electricity from renewable sources, like solar energy? A because it is much more expensive to make electricity from non-renewable sources than to make it from renewable ones B because the sources used most are running out very quickly, and renewable sources will not run out any time soon C because renewable sources can burn more easily, which means we can produce more steam to power more machines D because using energy from renewable sources is a "wild and crazy idea", and scientists prefer to work on very creative projects

Atomic Structure 2: Electronic Structure:Question 6 Read the statement. lodine is on group 17 of the periodic table. Which option describes how iodine most commonly behaves when forming ions? It loses 1 electron. It loses 2 electrons. It gains 2 electrons. It gains 1 electron.

A gas occupies 18.7 L at 2.00 atm pressure and 27°C. How many moles of gas are present in the sample a 3.92 mol b. 3.02 mol c. 16.9 mol d. 0.760 mol e. 1.52 mol

An unknown compound has the following chemical formula: PxCl5 where x stands for a whole number. Measurements also show that a certain sample of the unknown compound contains 5.5 mol of phosphorus and 27.56 mol of chlorine. Write the complete chemical formula for the unknown compound.

An excess of Al and 2.3 mol of Br2 are reacted according to the equation 2A1+ 3Br2 → 2AlBr3 How many moles of AlBr3 will be formed assuming 100% yield? a. 3.5 mol b. 2.3 mol c. 1.2 mol d. 1.5 mol e. 0.8 mol

For the following reaction, determine the equilibrium constant at 700 °C if at this temperature. The equilibrium concentrations are as follows: [H₂] = 0.28 M, [S2] = 1.13 x 10-6M, [H2S] = 0.75 M 2H2(g) + S2(g) → 2H2S(g) A. 1.78 x 106 B. 8.47 x106 C. 6.35 x 106 D. 1.08 x 107 E. 3.22 x106

The balanced equation P4(s) + 6H₂(g) → 4PH3(g) tells us that 7.0 mol H₂ a reacts with 3.5 mol P4 b. cannot react with phosphorus c. reacts with 7.0 mol P4 d. produces 4.7 mol PH3 e produces 14.0 mol PH3

A 10.03g sample of high fructose corn syrup concentrates is burned in a bomb calorimeter containing 200.0 g H₂O. The temperature of the water increased by 15.53°C. If the molar mass of this nutrient substance is 198.17 g/mol, what is the fuel value (in nutritional Cal/g)? [1Cal = 1000 cal = 1 kcal; Specific heat of water = 1.00 cal/(g*°C)] A. 0.159 Cal/g B. 0.310 Cal/g C. 3.11 Cal/g D.3.08 Cal/g E. 0.786 Cal/g

Match each orbital with a description of its general shape. d orbitals s orbitals f orbitals p orbitals a. dumbbell shaped b. clover shaped c. spherical d. none of these

What major assumption (that was analogous to what had already been demonstrated for electromagnetic radiation) did de Broglie and Schrödinger make about the motion of tiny particles? A tiny particle, such as an electron, behaves as a discrete particle. A tiny particle, such as an electron, behaves as a wave. A tiny particle, such as an electron, behaves simultaneously as a wave and as a discrete particle.

In 1913, Niels Bohr proposed that electrons revolve around the nucleus of an atom in discrete orbits, each orbit corresponding to a certain specific level of energy. Which one of the following statements is a consequence of this model? When an electron absorbs energy, it moves a higher orbit, and when it moves to a lower orbit, it emits energy. Electrons are able to move from one orbit to another within the same atom without any gain or loss of energy. The atomic emission spectrum for hydrogen has only one line in the visible region. When an electron emits energy, it moves to a higher orbit, and when it moves to a lower orbit, it absorbs energy. A maximum of only two electrons may simultaneously occupy any orbit.

Rank the types of electromagnetic radiation from least energy to highest. _ gamma _ visible light _ ultraviolet _ infared _ radio _ microwave _ x-ray

What is the frequency (in reciprocal seconds) of electromagnetic radiation with a wavelength of 1.41 cm? Enter your answer in scientific notation.

To which element does each of the following electron configurations correspond? a.[Ne]3s²3p4 b.[Ar]4s² c. [Ar]48²3d¹04p¹

What is the maximum number of electrons possible with n = 4 in an atom?

What angular momentum (1) quantum number indicates an orbital that has a clover shape. 3 1 2 4 0

Which of the following correctly summarizes the Hund's Rule? Matter can neither be created nor destroyed. It only changes form during chemical reactions. It is fundamentally impossible to know both the location and velocity of an electron at the same time. Each electron within an atom will have its own unique set of four quantum numbers. Electrons orbiting an atom fill the lowest available energy levels prior to filling higher energy orbitals. The ground state or lowest energy state of an atom is the one that contains the maximum number of unpaired electrons.

What are the sublevels of the 3rd energy level (n=3)? 3s, 3d, 3f 3s, 3p, 3d 3s, 3p, 3f 3p, 3d, 3f 3s, 3p, 3d, 3f

How much more energy per photon is there in green light of wavelength 526 nm than in red light of wavelength 631 nm? (Enter your answer in scientific notation.)

Identify the following three elements. (Capitalization counts!) An excited state of this element has the electron configuration 1s²2s²2p 3s¹. The ground-state electron configuration is [Kr]5s²4d¹05p². The ground-state electron configuration is [Ar]4s²3d¹04p².

Enter your answer in the provided box. The retina of a human eye can detect light when radiant energy incident on it is at least 4.0 × 10¯17 J. For light of 565-nm wavelength, how many photons does this energy correspond to?

Compare the ionization energies of each pair of atoms. Enter the symbol for the atom with the larger ionization energy. (If both atoms would be expected to have the same ionization energy, enter the word same.) Pairs Symbol of atom with the larger ionization energy H and Li C and N Na and K

Which of the following correctly summarizes the Aufbau Principle? Each electron within an atom will have its own unique set of four quantum numbers. Matter can neither be created nor destroyed. It only changes form during chemical reactions. It is fundamentally impossible to know both the location and velocity of an electron at the same time. The ground state or lowest energy state of an atom is the one that contains the maximum number of unpaired electrons. Electrons orbiting an atom fill the lowest available energy levels prior to filling higher energy orbitals.

A chemist adds 210.0 mL of a 2.68 × 10-5M zinc oxalate (ZnC₂04) solution to a reaction flask. Calculate the micromoles of zinc oxalate the chemist has added to the flask. Round your answer to 3 significant digits.

Give the electron configurations for the following atoms. Do not use the noble gas notation. Write out the complete electron configuration. Example: Mg 1s²2s22p63s² Element Electron configuration P S He B Li

Compare the atomic sizes of each pair of atoms. Enter the symbol for the larger atom of each pair. (If both atoms are the same size, enter the word same.) Pairs Symbol for larger atom H and Li C and N He and Kr

Consider the following reaction for the combustion of octane, Cs H18: 2C8H18(l) +25O2 (g) → 16CO₂(g) + 18H₂O(l) What volume of oxygen gas at STP would be needed for the complete combustion of 13.9 g of octane?