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CEM 141 Study Guide - Midterm Guide: Scale Of Temperature, Guitar Tunings

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4 Feb 2020

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10 c to 50 c: the kinetic energy of water molecules increases, making the molecules collide more forcefully with the thermometer. This forces the mercury up the capillary tube causing an increase in the temperature scale: the water molecules speed up, and collide with the thermometer, transferring energy to the thermometer. This energy causes the mercury atoms in the thermometer to vibrate more, and the liquid expands. Thus showing an increase in the temperature scale: the water molecules expand until some of the bonds holding the atoms together break, the water molecules move faster and bump into each other. Which gas corresponds to the distribution marked by the arrow: ne, ar, kr, xe. Use this diagram to answer questions 5 . 6: for the process shown h (for the system) is: [vaporize]?: ch3oh, ch4, 25 g of a metal are heated to 79 c and, of2, naf added to 25 g water at 20 c.

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Related Questions

1. A substance decomposes in a first-order reaction with a rate constant of 6.70 x 10â4 s â1 . If the initial concentration of the substance is 1.50 M, what is its concentration after 500. s?

Please show all work and explain

2. Which statements about the behavior of gaseous H2 molecules in a container at 1 atm and 298 K are correct?

I. All H2 molecules are moving at the same speed.

II. The H2 molecules are colliding more frequently with the walls of the container than they would in the same container at 398 K.

I don't understand why neither of the statements are correct.

3. In a well-insulated vessel, 50.0 g ice at 0.0 ÂºC is added to 350. g water at 32.0 ÂºC. What is the final temperature when the mixture reaches equilibrium? (The heat of fusion of ice is 334 J gâ1 .)

(A) 18.0 ÂºC

(B) 20.6 ÂºC

(C) 22.0 ÂºC

(D) 28.0 ÂºC

Please show work and explain

provided to determine AH rxn for the following reaction: urf (klimol) CH4(g) + 3 Cl2(g) â CHCI3() + 3 HCI(g) airrxn-? A)-151 kJ B)33SkJ C) +662kJ D) +117kJ E)-217 kJ A) 4.1 atm B) 5.0 atm c) 6.4 atm D)1.1 atm E) 2.3 atm kg) of the copper sample if the specific heat capacity of copper is 0 CH4(g) 75 CHCI3() -134 HCI(g) -92 8) What pressure will 14.0 g of CO exert in a 3.5 L container at 75 C? 9) A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 50.0Â°C, determine the mass (in .385 J/g C A) 226 kg B) 0.235 kg C)6.64 kg D) 119kg E)5.10 kg 10) Which of the following processes is exothermic? A) the ionization of a melting snow atom B) the breaking of a boiling of water bond C) the boiling of water D) the condensation of water E) All of the above processes are exothermic 11) Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm. B)4.27 x 10-19J C) 2.34 x 10-19J D)6.45 x 10-19J E) 2.83 x 10-19J A)3.54 Ã 10-19J 12) Identify the color of a flame test for potassium D) yellow A) violet B) red C) white E) blue 13) Which of the following statements is TRUE? A) The emission spectrum of a particular element is always the same and can be used to identify the element. B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus. C) The uncertainty principle states that we can never know both the exact location and speed of an electron. D) An orbital is the volume in which we are most likely to find an electron. E) All of the above are true. 14) Calculate the wavelength of an electron (m-9.11 x 10-28 g) moving at 3.66 Ã 106 m/s. A)1.99 x 10-10m B)5.03 x 10-10 m C) 1.81Ã10-10 m D)5.52 Ã 10-9 m E) 2.76 Ã 10-9 m 15) Which of the following quantum numbers describes the shape of an orbital? A) principal quantum number B) magnetic quantum number C) spin quantum number D) SchrÃ¶dinger quantum number E) angular momentum quantum number 16) Determine the energy change associated with the transition from n = 2 to n-5 in the hydrogen atom. A)-218Ã10-19J B)+654 Ã 10-19 J C) +4.58 x 10-19 J D)-1.53 x 10-19 J E) +3.76 Ã 10-19J 17) If two electrons in the same atom have the same value of I, they are A) in the same sublevel, but not necessarily in the same level. me level, but different sublevel. C) in the same orbital. D) in different levels and in different shaped orbitals. E) none of the above.

Please answer to the best of your ability

Show transcribed image text correctly.Completion and turning in of the entire review will result in an additional +3 pts on your final exam. Show all work to get extra credit. Please contact your instructor for clarification or specific questions. Report the following answers to the following problems with the correct number of significant figures and units: 1. 1 (0521 g 0.4953 0098 61â-24.135ë¯¸+1(120 64 g 4.1847 a)(21st-241530 1 (98.61 C-24.135)120.64g 4.1 21.5Â°C-24.153C) 0.0213548 moles b. (00020334-ern) + ((61210 goles Og) 0.002030 moles 1.02 moles (68.79 mlt29.901 ml) (26.3-0.230) c. 2. You are drying a sample of Bas(POsh. After 5 minutes of drying it weighs 1.2034 g. You continue to dry the sample for another 5 minutes and it now weighs 1.9346 g. What is the percent change in mass? 3. What is the percent mass of carbon in sodium carbonate? 4. What is the density of water at 23.1051Â°c? Use Table 1.1 on page 27 of your lab manual to help. 5. Based on the following reacts, predict the products. Write the balanced molecular equation, total ionic equation, and net ionic equation. All reactions are done in water a. Sodium chloride +silver (I) nitrate b. Calcium bromide + iron (III) sulfate c. Ammonium phosphate+ nickel (II) nitrate d. Hydrochloric acid+ calcium carbonate 6. Write the two balanced chemical reactions for a. Copper (II) oxide reacting with methane under high heat b. Copper (1) oxide reacting with methane under high heat 7. You analyze a mixed sample of copper (1) oxide and copper (II) oxide. The plot and trendline for mass of copper versus mass of mixture yields a slope of 0.8031. What are the mass percents of copper (0) oxide and copper (II) oxide in the mixture?
8. During week 1 of the Empirical Formula Lab you extinguished your "L-tube" flame without waiting 9. 20.00 ml of a 0.30 M potassium phosphate solution is combined with 20.00 mL of a 0.40 M solution 10. An Erlenmeyer flask is capped with a rubber stopper at room temperature (25 C) and atmospheric 11. The first step of the copper cycle lab was reacting solid copper with nitric acid. The copper ends up 12. What are the spectator ions in the 6 reactions performed during the copper cycle lab? for the reaction to cool and did NOT relight the "L-tube" flame. How would this affect your calculated percent mass compared to the true percent mass? of calcium chloride. What is the limiting reactant? What is the identity of the precipitate formed in the reaction? How many grams of product should be collected? pressure (1 atm). What temperature does the Erlenmeyer flask need to be heated to for the stopper to pop off? Assume it needs to exceed external pressure by 0.5 atm to release the stopper. oxidizing to copper (ll). What is the oxidizing reagent in this reaction? 13. The known specific heat capacity of aluminum is o g mo 25.316 g of aluminum is placed in 99.134 of water at a starting temperature of 22.45Â°C. The metal has a AT-84.02c what is the final 14. The AH, of cobalt (U) nitrate is +47.7 kJ/mol. What is the AHr of solid cobalt (1) nitrate? 15. 5.000 g of aluminum (Il) chloride is dissolved in 60.0 mL of water. The temperature changes by 16. Draw the Lewis dot symbols for the following atoms: temperature of the water? ÎÎ(Nouql)--205.00 kJ/mol ÎÎ,(Co2"m)--58.2 kJ/mol 0.331 Â°C. The specific heat capacity of aluminum (III) chloride is 0.903 Wat s AH.? what is ÎÎ a Ð°, Ð½Ðµ Ñ, Ñ c. Ar d. P e. H 17. Draw the Lewis structures for the following molecules: a. NHa b. O2 XeF d. NF