Chem101 Practice Problems

docx

School

Arizona State University *

*We aren’t endorsed by this school

Course

101

Subject

Chemistry

Date

Jun 9, 2024

Type

docx

Pages

Uploaded by GeneralPorcupineMaster370

Chapter 1 - Mostly Units Stuff Question 1: Convert 1.21 km to mm. Question 2: Convert 2.1 * 10 4 mL to L. Question 3 Convert 0.55 m 3 to L (1 cm 3 = 1mL, 1 m 3 = (1000 cm) 3 , not 1000 cm 3 ) Question 4 Convert 1.21 kg to g. Chapter 2 - Atoms, Ions, and the Periodic Table Question 7 : What changes between isotopes of an element? a. Electrons b. Protons c. Neutrons d. None of the above Question 8: What changes between ions of an element? a. Electrons b. Protons c. Neutrons d. None of the above Question 9: A sample of 0.1 mol of dichloromethane (CH 2 Cl 2 ) has a relative abundance of 58% 35 Cl and 42% 37 Cl. What is the average atomic mass of Chlorine in the sample? Question 10: In the universe overall, the average atomic mass of Chlorine is 35.446 AMUs. Relatively speaking, which of the following is true of the Chlorine in Question 3 compared to the universe as a whole? a. It has more 35 Cl and less 37 Cl b. It has more 37 Cl and less 35 Cl c. It has more of both 35 Cl and 37 Cl d. It has less of both 35 Cl and 37 Cl

e. None of the above Chapter 3 - Chemical Compounds For questions about naming ionic compounds, see the practice worksheet I sent out on Friday. Question 11: Name P 4 O 10 . a. Phosphoric Oxide b. Phosphous Oxide c. Tetraphosphorous Decaoxide d. None of the above Question 12: Name FeO. a. Iron Oxide b. Iron (II) Oxide c. Iron (II) Monoxide d. Iron (I) Oxide Question 13: Name NI 3 . a. Nitrogen Triiodide b. Nitrogen Iodide c. Nitrogen (III) Iodide d. None of the above Question 14: Name H 2 O (The chemical name - I know it’s water). a. Hydrogen oxide b. Dihydrogen oxide c. Dihydrogen monoxide d. Hydrogen (II) Oxide e. None of the above Question 15: Name FeP. a. Monoiron Monophosphide b. Iron (I) Phosphate c. Iron (I) Phosphide d. Iron (III) Phosphate e. Iron (III) Phosphide

f. None of the above Question 16: What is the formula of Copper (II) Oxide? a. CoO b. CoO 2 c. CuO d. CuO 2 e. Cu 2 O Question 17: Name Be 3 N 2 . a. Beryllium Nitrate b. Beryllium Nitride c. Beryllium (III) Nitride d. Beryllium (II) Nitrate e. None of the above Question 18: What is the formula for Copper (I) Sulfate? a. CuS b. CuSO 4 c. Cu 2 SO 4 d. CuS 2 Chapter 4 - Chemical Composition Question 19: A mole is most closely analogous to: a. A kilogram b. A dozen c. A liter d. A mouse Question 20: How many molecules are in 1.4 * 10 -5 mols of CO 2 ? Question 21: How many mols are in a 345.2 g sample of SiO 2 ? Question 22: How many mols are in a 71 g sample of FeO?

Your preview ends here

Eager to read complete document? Join bartleby learn and gain access to the full version

Access to all documents
Unlimited textbook solutions
24/7 expert homework help

Question 23: How many mols of Copper ions are in a 1.34 kg sample of Copper (II) Phosphate? Question 24: How many mols ions are in 0.043 kg of sodium chloride? Chapter 5 - Chemical Reactions and Equations Question 25: What kind of reaction is 3H 2 (g) + 2N 2 (g) -> 2NH 3 (l)? a. Combination b. Decomposition c. Single-replacement d. Double-replacement Question 26: What kind of reaction is BaCl 2 (aq) + Na 2 SO 4 (aq)→BaSO 4 (s) + 2NaCl (aq)? a. Combination b. Decomposition c. Single replacement d. Double-replacement Question 27: What kind of reaction is 2H 2 O 2 (l) -> O 2 (g)+ 2H 2 O (l)? a. Combination b. Decomposition c. Single replacement d. Double-replacement Question 28: What kind of reaction is 2AgNO 3 (aq) + Cu (s) -> Cu(NO 3 ) 2 (aq) + 2Ag(s)? a. Combination b. Decomposition c. Single replacement d. Double-replacement Question 29: What kind of reaction is HCl(aq) + Li(s) -> LiCl 2 (aq) + H 2 (g)? a. Combination b. Decomposition

c. Single replacement d. Double-replacement Question 30: a. Combination b. Decomposition c. Single replacement d. Double-replacement Question 31: Which of the following reactions will take place? Assume all reagents are aqueous unless otherwise specified. a. Sodium Chloride and Hydrochloric Acid b. Potassium Nitrate and Sulfuric Acid c. Silver Nitrate and Carbonic Acid d. Iron metal and Barium oxide e. All of the above f. a, b, and c g. a and d h. a, c, and d i. None of the above Question 32: Which of the following reactions will form a precipitate? a. Reaction of Sodium Hydroxide with Sulfuric Acid b. Reaction of Sodium Hydroxide with Iron (II) Sulfate c. Reaction of Nitric Acid with Beryllium metal d. All of the above e. None of the above Chapter 6 (Part 1) - Quantities in Chemical Reactions There will be more questions involving quantities in chemical reactions in later sections and in the Putting It All Together section. Question 33: Balance the following reaction: H 2 O (l) + AlCl 3 (s)-> Al(OH) 3 (s) + HCl (aq) Question 34: Balance the following reaction: AgNO 3 (aq) + H 2 SO 4 (aq) -> Ag 2 SO 4 (aq) + HNO 3

Question 35: In the reaction of Hydrobromic Acid and Iron metal to form Iron (II) Bromide, what is the Mole Ratio between Hydrobromic Acid and Iron (II) Bromide? Question 36: a. The reaction of Isopropyl Alcohol (C 3 H 7 OH) and Oxygen gas produces water and CO 2 . Write the balanced equation for the reaction. b. I react 22.1 grams of Isopropyl Alcohol (C 3 H 7 OH) with 2.00 mols of Oxygen gas. What is the limiting reagent? c. In this reaction, H 2 O is released as a gas. I condensed the H 2 O produced by the reaction into liquid form. How many milliliters of H 2 O should I expect to get? (remember: the density of water is 1 g / mL) d. If, after the reaction in Question 36 and the condensation in Question 37, I got XXX mL of H 2 O, what was the percent yield of the reaction? Question 37: a. Ammonia (NH 3 ) reacts with Hydrochloric Acid to form Ammonium Chloride (NH 4 Cl). How many grams of Ammonia do I need to fully react with 1.0 mols of Hydrochloric Acid? b. How many grams of Ammonium Chloride do I produce? Question 38: How many grams of Sodium hydroxide would I need to neutralize (fully react with) 10.0 grams of Phosphoric Acid? Chapter 6 (Part 2) - Energy and Energy Changes Question 39: A reaction that produces heat is: a. Exothermic b. Endothermic c. Homeopathic d. Depends on the situation e. None of the above

Your preview ends here

Eager to read complete document? Join bartleby learn and gain access to the full version

Access to all documents
Unlimited textbook solutions
24/7 expert homework help

Question 40: What is the First Law of Thermodynamics? a. You do not talk about Thermodynamics. b. A thermodynamics in motion will remain in motion unless acted upon by an outside force. c. All stable thermodynamic systems are alike, but each unstable thermodynamic system is unstable in its own way. d. It is a truth universally acknowledged, that a single man in possession of a good fortune, must be in want of thermodynamics. e. Thermodynamics may not harm a human or through inaction allow a human to come to harm. f. Other: _______________________________________________________________ (Bonus points: what are the sources of all these OTHER laws?) Question 41: The reaction of NaOH (aq) + HCl (aq) -> NaCl(aq) + H 2 O(l) has a H of -55.7 kJ / mol HCl. If 𝚫 you mix 0.1 L of 5 M HCl at 21 c C with 0.1 L of 5 M NaOH at 21 o C, what would you expect the final temperature of the solution to be? Remember how negative and positive signs work in heat transfer, and don’t forget that the volumes are being combined! Question 42: a. The temperature of 0.100 L of Ethanol goes from 21 o C to 61 c C. What was the heat change of the Ethanol? The specific heat of ethanol is 2.46 J / mol o C, and the density of ethanol is 0.789 g/mL b. If the source of the heat is a 25.0g copper cylinder, and the final temperature of the copper cylinder was the same as the final temperature of the ethanol, what was the starting temperature of the copper? The specific heat of copper is 0.385 J / mols * o C. Chapter 7 - Electromagnetic Radiation and the Electron Structure of the Atom Speed of Light (c) = 3.00 * 10 8 m / s Planck’s Constant (h) = 6.626 × 10 -34 J * s

Fig. 1: The electromagnetic spectrum. Image From Eye Hortilux Question 43: Place the following colors of light in order from highest to lowest energy: Blue, Yellow, Red, Green, Violet Question 44: Which of the following electron transitions would emit the lowest wavelength photon? n=5 -> n=2, n=4 -> n=2, n=3 -> n=2 Question 45: Which of the following electron transitions would emit the lowest frequency photon? n=6->n=3, n=5->n=3, n=4->n=3 Question 46: a. What is the frequency of light with a wavelength of 420 nm? b. What is its energy? Question 47: What is the wavelength of a photon with an energy of 6.9 * 10 -14 J? Question 48: I’m making a Neon Light! I excite the electrons of 0.01 mols of Neon gas by applying 2.0 kJ of energy, which causes the electrons to jump to a higher energy level. When the electrons fall back down, they emit energy in the form of photons. Assuming every atom releases one photon, what will be the wavelength of the emitted light? Note: this is a simplification; actual Neon lights work on a similar principle but are more complicated Chapter 8 - Chemical Bonding Question 49: What is the molecular geometry of PH 3 ? Question 50: How many valence electrons does Bromine have? Question 51: a. Is ammonia (NH 3 ) polar? b. Is ammonium (NH 4 + ) polar?

Question 52: Is water polar? Chapter 9 - Gas States R = 8.314 kPa * L / (mols * o K) Standard Pressure: 101.325 kPa Room Temperature: 21 o C o K = o C + 273 Question 53: What is the volume of 2.5 L of O 2 gas at room temperature and standard pressure? Question 54: In an ideal gas, are the Pressure and Temperature: a. Inversely proportional b. Directly proportional c. Unrelated Question 55: In an ideal gas, are the volume and molecular weight: a. Inversely proportional b. Directly proportional c. Unrelated Question 56: a. I pump 2.24 liters of an ideal gas starting at standard pressure into a 1 L container of fixed size. What is the pressure of the container? Assume room temperature throughout the experiment. b. Following up on the previous question, I check my handy-dandy thermometer and determine that the temperature of the gas in the container has actually fallen to -4 o C. Given this information, what is the actual pressure of the gas? Chapter 10 - Liquid and Solid States Question 57: What is vapor pressure? a. The force that keeps a gas in a pre-med program because its parents want it to become a doctor, even though it really just wants to get a degree in business and a boring office job b. The force that makes it difficult to breathe during a final exam c. The pressure of the atmosphere d. I have no dang idea

Your preview ends here

Eager to read complete document? Join bartleby learn and gain access to the full version

Access to all documents
Unlimited textbook solutions
24/7 expert homework help

e. The pressure created by the evaporation of small amounts of a liquid off the surface of the liquid Question 58: Rank the following intermolecular forces from strongest to weakest : I. Hydrogen Bonding II. Dipole-dipole interactions III. London Dispersion Question 59: Which of the following molecules would you expect to have the highest boiling point? a. CH 3 OH b. C 2 H 5 OH c. C 3 H 7 OH d. C 4 H 10 e. They should all have the same boiling point Question 60: Free space! Circle “correct” to get a point here! Don’t you with the exam was like this? Question 61: Which of the following molecules would hydrogen-bond? a. H 2 Se b. CaH 2 c. H 2 NOH d. CH 4 e. Both a. and c. f. All of the above g. None of the above Question 62: Which of the following would exhibit only London Forces of attraction? a. Cl 2 b. HF c. CH 3 Cl d. All of the above Question 63: Which would exhibit dipole-dipole intermolecular forces? a. BCl 3 b. CCl 4

c. HCl d. None of the above Question 64: The substance expected to have the highest boiling point is a. CH 2 b. C 2 H 8 c. C 3 H 8 d. C 4 H 10 . (these last four questions are adapted from Dan Eddy’s study guide at Louisiana Tech) Chapter 11 - Solutions Question 65: Are solubility and temperature: a. Directly proportional b. Inversely proportional c. Unrelated d. Question 66: What is the general rule for solubility? Three words. Question 67 Which of the following is soluble in water? a. Be(OH) 2 b. AgNO 3 c. C 6 H 14 d. C 2 H 6 O e. b. and d. f. All of the above g. None of the above h. Both f. and g. Question 68: How does pressure affect the solubility of a gas? Question 69: You made it this far! Nice!

Question 70: I have 250.0 mL of a 5.5 M solution of Calcium Chloride. In order to extract the CaCl 2 , I boil off 150 mL of the solution, leaving 100 mL behind (the CaCl 2 does not boil off). I then cool the solution back to room temperature. The solubility of CaCl 2 at room temperature is 81.1 g / 100 mL. What will be the mass of the CaCl 2 precipitate? Chapter 12 - Equilibrium Question 71: Which of the following statements is true? a. A reaction in equilibrium has no reactants remaining b. A reaction in equilibrium always has the same amount of reactants and products c. The equilibrium constant is dependent on the temperature d. The equilibrium constant is dependent on the current zodiac sign Question 72: If the equilibrium constant of a reaction K eq = 7.3 * 10 -4 , would I expect the equilibrium to favor: a. The products b. The reactants c. Both d. Neither (Questions 73 - 78 sourced from Minnesota State University Moorhead Prof.Craig P. Jasperse) Question 73: Consider the acid dissociation of mercaptoethanol (HSCH 2 CH 2 OH): HSCH 2 CH 2 OH(aq) H+ (aq) + SCH ⇋ 2 CH 2 OH – (aq) K eq = 1.91 x 10 -10 Which of the following statements is true regarding this equilibrium? I. The reaction is product favored. II. The reaction is reactant favored. III. Equilibrium lies far to the right. IV. Equilibrium lies far to the left. a. I and III b. I and IV c. II and III d. II and IV

Your preview ends here

Eager to read complete document? Join bartleby learn and gain access to the full version

Access to all documents
Unlimited textbook solutions
24/7 expert homework help

e. None are true, as the concentrations of reactants and products are comparable. Question 74: The equilibrium constant for the formation of hydrogen iodide from hydrogen and iodine is 45 at a certain temperature. H 2 (g) + I 2 (s) 2 HI(g) K eq = 45 Which of the following is true regarding this equilibrium? I. The reaction is product favored. II. The reaction is reactant favored. III. Equilibrium lies to the right. IV. Equilibrium lies to the left. a. I and III b. I and IV c. II and III d. II and IV e. None are true, as the concentrations of reactants and products are essentially the same Reminder: solutes (aq) or gases (g) appear; solvents (l) or solids (s) do not. Question 75 Write an expression for the equilibrium constant for the formation of two moles of ammonia gas (NH 3 ) from nitrogen and hydrogen in their standard states. __ N 2 (g) +__ H 2 (g) __ NH ⇋ 3 (g) Question 76: Write the correct K eq expression for the following reaction? ___ C 3 H 8 (g) + __ O 2 (g) __ CO ⇋ 2 (g) + __ H 2 O(g) Question 77: Write an expression for the equilibrium constant for this reaction.

__ N 2 O 4 (g) + __ O 3 (g) __ N ⇋ 2 O 5 (s) + __ O 2 (g) Question 78: For the reaction 2A + B 2C the appropriate form for the equilibrium constant expression ⇋ is: a. [A][B] 2 /[C] b. [A] 2 [B]/[C] 2 c. [C] 2 /[A] 2 [B] d. [A][B] 2 [C] e. none of the above Chapter 13 - Acids and Bases Question 79 According to the Bronstead-Lowry definition, an acid is: a. A proton acceptor b. A proton donor c. A neutron donor d. An electron donor e. None of the above Question 80 True or false: by definition, a strong acid is more dangerous than a weak acid. Question 81 What is the pH of a 1 M solution of hydrochloric acid? Question 82 What is the conjugate base of Nitric Acid (HNO 3 ) ? Question 83 What is the pH of pure water? What does that mean in terms of equilibrium of the reaction H 2 O(l) H ⇄ + (aq) + OH - (aq)? Question 84 If I have a solution of Nitric Acid (a weak acid) and add sodium nitrate, will the pH: a. Go up b. Go down c. Go sideways?

d. Stay the same Combination / Challenge / Fun Questions Question 87: It is Copenhagen, Denmark in 1940 and I am chemist and future Nobel laureate Georgy de Hevesy A few years ago, my friends Max von Laue and James Franck illegally sent their golden Nobel Prize medals to me to keep them safe from the Nazis, but now the German army is bearing down on Copenhagen and I need to hide the Nobel Prizes, fast. Since I - future Nobel Prize winner Georgy de Hevesy - am a very good chemist, I know that one of the only things that can dissolve gold is the medieval alchemical substance aqua regia (Latin for Royal Water), a solution of Nitric Acid and Hydrochloric Acid. Reaction 1 Au (s) + 3NO 3 - (aq) + 6H + (aq) ➔Au 3+ (aq) + 3 NO 2 (g) + 3 H 2 O (l) Reaction 2 Au 3+ (aq) + 4 Cl - (aq) ➔ AuCl 4 - (aq) a. If each of my two Nobel medals weighs 200 g and is 95% gold by weight (disregard other elements), how many mols of HNO 3 do I need to fully perform Reaction 1? Assume that the reaction will run to completion. b. How many mols of HCl do I need to complete reaction 2? c. In order to avoid it being noticed by the Nazis ransacking my lab, I want my solution of dissolved Nobel Prize to be 1 L. Once the reactions are complete, what will be the concentration of AuCl 4 - in my 1L solution? Question 88: Real problem from my lab work: I’m trying to construct a DNA nanostructure - a three-pointed star. The star consists of three DNA strands: A, B, and C. a. The strands of the DNA react in the following way: A (aq) + __ B (aq) + ___ C (aq) ➔ AB 3 C 3 (aq) Balance the reaction with the correct coefficients for A, B, and C. b. If I want my concentration of AB 3 C 3 to be 1.8 µM, what should my concentrations be of A, B, and C? Use mole-to-mole ratios, and assume a complete reaction. (µM = micromolar, 1 µM = 10 -6 M).

Your preview ends here

Eager to read complete document? Join bartleby learn and gain access to the full version

Access to all documents
Unlimited textbook solutions
24/7 expert homework help

c. To begin, I’m going to create 100 µL stock solutions of A, B, and C with concentrations of 5µM each. Fill in the following table: C 1 V 1 C 2 V 2 V Water V Total Strand A 59.81 µM 5 µM 100 µL Strand B 28.58 µM 5 µM 100 µL Strand C 55.49 µM 5 µM 100 µL d. I’m going to use colorimetry to check the concentrations of my solutions. DNA has its highest absorbance at 260 nM. To get a more accurate reading, I measured the absorbance twice. Fill in the following table to calculate the actual concentrations of A, B, and C. Remember Beer’s Law: A = ε * l * c The path length is 1 µm (micrometer). Remember: 1 µM = 1 µmol / L A 260 (1) A 260 (2) Avg. A 260 ε c Strand A 3.546 3.574 0.6625 * 10 6 L / µmol * µm Strand B 2.170 2.175 0.4121* 10 6 L / µmol * µm Strand C 1.062 1.054 0.2076 * 10 6 L / µmol * µm e. Now, I need to set up my reactions. To fully test the formation of the DNA star, I’m testing every possible combination of A, B, and C. I also need to add TAE buffer. My TAE buffer is at a concentration of 10X, which means I need to dilute it by 1:10. Fill in the following table. Hints: i. Your C 1 values should be taken from the table you just filled out in part d. ii. Your C 2 values should be the ones you calculated in part a. iii. The volume of H 2 O in each reaction should be 20µL- the sum of all the numbers in the V 1 column. iv. The volume of the TAE buffer to add should be the same in each reaction.

Rxn A + B A + C B + C A + B + C All C 1 V 1 C 2 C 1 V 1 C 2 C 1 V 1 C 2 C 1 V 1 C 2 V 2 Strand A 0µM 0µL 0µM 20µL Strand B 0µM 0µL 0µM 20µL Strand C 0µM 0µL 0µM 20µL TAE buffer 10X 1X 10X 1X 10X 1X 10X 1X 20µL H 2 O n/a n/a n/a n/a n/a n/a n/a n/a Total 20µL 20µL 20µL 20µL

f. If all goes as planned, after the reaction your nanostructure should look like this! It’s worth noting that it didn’t go as planned for me; this image is from my second attempt. Fig. 2: Atomic Force Microscopy image of DNA nanostructures forming a hexagonal pattern. You can see the physical DNA! Isn’t that SO COOL? Source for Procedure: Self-Assembly of Hexagonal DNA Two-Dimensional (2D) Arrays

Your preview ends here

Eager to read complete document? Join bartleby learn and gain access to the full version

Access to all documents
Unlimited textbook solutions
24/7 expert homework help

Yu He, Yi Chen, Haipeng Liu, Alexander E. Ribbe, and Chengde Mao Journal of the American Chemical Society 2005 127 (35), 12202-12203 DOI: 10.1021/ja0541938 Question 88: Real problem from lab work: I have a 55 mL solution of bacteria. To make them express the protein I want them to express, I need to add 7-hydroxycoumarin amino acid (7-HCAA for short), which has a formula of C 13 NO 5 H 13 . The bacteria need the 7-HCAA at a concentration of 1 millimolar (mM, 1000mM = 1M). a. The first thing I do is make a 1.500 mL stock solution of 7-HCAA. How many milligrams (1000mg = 1g) of 7-HCAA do I need to weigh out to make a 1.500 mL solution of 100 mM 7-HCAA? (Hint: You can calculate the molar mass of 7-HCAA using the formula I gave you earlier) b. In order to dissolve the 7-HCAA, my stock solution needs to have a 200 mM concentration of NaCl. How much of my 1M NaCl solution and how much water should I use to make a 1.500 mL solution of 200 mM NaOH? c. I accidentally weighed out 47.1mg of 7-HCAA. I don't want to waste the 7-HCAA (which is very expensive) and my tube can't hold more than 1.5 mL of solution, so I'm going to make my stock solution more concentrated but add less of it to my bacteria. What's the molarity of the solution I made with 47.1mg of 7-HCAA and 1.500 mL of the 200mM NaOH solution? d. How much of the solution from part d. do I need to add to my 55mL bacterial culture to make the culture have a 1mM concentration of 7-HCAA? e. What will be the concentration of NaOH in my 55mL bacterial culture once I add my solution in? (I didn't bother calculating this so I have no idea what the answer is) Question 89: I reacted 2 micromols of H2 with 4 mols of O2 in a sealed, insulated container with a volume of 80L. No other gasses were present. I’ve placed an excess of a desiccating agent which will absorb any water that is produced. The gasses started at 293 oK. What will the pressure of the gas be after the reaction?

For the purposes of your calculations, the specific heat of oxygen gas is 0.92 J / g oK. The gas constant is 0.082 atm / mols * oK. The H of the reaction of H2 and O2 is -2.8577 * 105 kJ / formula unit 𝚫 Question 90: It’s 1914, and Fritz has just figured out how to make Ammonia from Hydrogen gas and Nitrogen gas - the trick is very high temperature and pressure! If has 10 mols of Hydrogen gas and 30 mols of Nitrogen gas, how small a volume does he need to compress them to for the gas to reach the 800 o K and 200 atm needed to produce ammonia, so the Kaiser can make explosives to win WWI despite being cut off from his vital supplies of South American bird poop? Question 91: In water, Carbon dioxide reacts to form Carbonic Acid with the equation CO 2 (aq) + H 2 O (l) H ⇄ 2 CO 3 (aq) Carbonic Acid is a weak acid, which dissociates with the equation H 2 CO 3 (aq) H ⇄ + (aq) + HCO 3 - (aq) a. If I increase the concentration of Carbon Dioxide, what will happen to the pH? b. Keeping this in mind, does it seem like maybe increasing the concentration of CO 2 in the atmosphere could cause Problems? Question 92: You’re given a material that absorbs high-energy photons and then emits the same number of low-energy photons. You have an instrument to record the wavelength of the photons emitted so you’ve attached a 100 mL beaker of water with a starting temperature of 20 o C to the material (assume perfect energy transfer with no loss). You shine 100 millimols of photons at the material at a wavelength of 420 nm and measure the temperature of the water again. It is now 47.22 o C. What was the wavelength of the photons emitted by the material? Reminder: Specific heat of water is 4.184 J / g * o C Hint: Don’t get overwhelmed - just take it step by step! You’ve learned everything you need to know to solve this problem!