The coffee cup calorimeter was determined to have a heat capacity of 8.5 J/ °C. The initial and final temperatures match the solution, at 21.50 °C and 28.25 °C, respectively. What is the heat change for the calorimeter during the dissolving process? acal = (Ccal) (Tf - T;) qcal = (8.5) (28.25 - 21.50) acal = [?] J Enter either a + or - sign AND the magnitude. Use significant figures.

The coffee cup calorimeter was determined to have a heat capacity of 8.5 J/ °C. The initial and final temperatures match the solution, at 21.50 °C and 28.25 °C, respectively. What is the heat change for the calorimeter during the dissolving process? acal = (Ccal) (Tf - T;) qcal = (8.5) (28.25 - 21.50) acal = [?] J Enter either a + or - sign AND the magnitude. Use significant figures.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The British thermal unit (Btu) is commonly used in engineering applications. A Btu is defined as the amount of heat required to raise the temperature of 1 lb of water by 1 °F. There are ________ Btu in one Joule. 1 lb = 453.59 g; °C = (5/9)(°F - 32°); specific heat of H2O (l) = 4.184 J/g-K.
How many calories of heat are required to lower the temperature of 550 grams of water from 64.4℉ to 53.6℉ if the specific heat of water is 1 cal/(g ∙ ℃)?
A piece of unknown substance weighs 55.8 g and requires 1910 J to increase its temperature from 21.7°C to 87.4°C. (a) What is the specific heat (in J/g-°C) of the substance? 4.0 J/g.°C (b) If it is one of the substances found in the table below, what is its likely identity? Specific Heats of Common Substances at 25°C and 1 bar Substance Symbol (state) Specific Heat (J/g-°C) O gold Au(s) 0.129 O copper Cu(s) 0.384 O iron Fe(s) 0.449 O argon Ar(g) 0.521 O silicon Si(s) 0.712 O carbon dioxide Co,(0) 0.843 O aluminum Al(s) 0.904 O nitrogen N2(g) 1.039 water H20(1) 4.1801 O helium He(g) 5.196 Type here to search hp 112 fs f6 144 sc & 8 Q E A J K B. FL %24
A chemist measures the enthalpy change AH during the following reaction: 4 Fe(s) + 3 02(g)→2 Fe,O3(s) AH =-320. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ x10 Fe(s) + 0,6) - Fe,0,(1) O kJ 2Fe,0; (s) – 4Fe(s) + 30, (3) O kJ 4Fe,0, (s) - 8Fe(s) + 60, (3)
Per x M Inb x 31799#/7231799/2/0 ted 13 out of 16 16 P11 Essentials of General, Organic, and Biochemistry Denise Guinn THIRD EDITION The table lists the specific heat values for brick, ethanol, and wood. Specific Heats of Substances Substance Brick Ethanol Wood heat added: P S per: X 20 effe x CDC He: X JA 6 Specific Heat 0.20 0.58 0.10 B 10 X 4 gºC Calculate the amount of heat, in calories, that must be added to warm 96.8 g of brick from 21.3 °C to 42.4 °C. Assume no changes in state occur during this change in temperature. W 4 Calculate the amount of heat, in calories, that must be added to warm 96.8 g of ethanol from 21.3 °C to 42.4 °C. Assume no changes in state occur during this change in temperature. ○바 8 No X 9 EC eth X 0 Sm X 00 39 HR MIN SEC 0/R Sm x Resources + presented by Macmillan Learning G ا ا ا 200 L Next Qu cal 40 1
What is the proper set up to find how much heat in kJ is released when 147 grams of NO2 (g) is dissolved in excess water? 3 NO2 (g) + H20 (g) ---> 2 HNO3 (aq) + NO (g) AHrxn = -138 kJ 1 mol NO2 -138 KJ 147 g NO2 x 46.01 g NO2“ 1 mol NO2 1 mol NO, -138 KJ 147 g NO, x 22.4 g NO2"1 mol NO2 1 mol NO2 -138 KJ 147 g NO, x 22.4 g NO2 * 3 mol NO2 1 mol NO2 -138 KJ 147 g NO2 x 46.01 g NO, * 3 mol NO2
(Q5) Consider an endothermic reaction that takes place in 251 mL of solution. If the reaction requires 4,423 J of energy and the initial temperature of the solution is 23.9, what will the final solution temperature be? (3 sf) The density of solution is 1.00 g/mL and the specific heat of the solution is the same as that of water.
Si + 2F2→SIF4(g) F2(3) SiF 4(2) Substance: Sis) -1615.0 H (kJ/mol) Final Answer: Solutions: 2C(s)+2H2+O2→ CH3COH C(s) H2 CH;CO;H@ Substance: -484.3 | H° (kJ/mol) Final Answer: Solutions:
What is the change in heat (in kJ to one decimal place) when 1.75 L of H2O condenses under 1 atm pressure at 100 °C? ΔHvap = 40.7 kJ mol–1 d(H2O) = 0.958 g mL–1 (at 100 °C)
27. When 0.0500 mol of CH4 (g) burns, 40.1 kJ of heat is produced. What is the change in enthalpy (AH) in kJ for the following reaction: CH4 (g) (a) +802 kJ/mol + 202 (g) (b) -802 kJ/mol , CO₂ (g) + 2H₂O(g) + Heat (c) +40.1 kJ/mol (d) -40.1 kJ/mol
CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? exothermic endothermic (b) Calculate the amount of heat transferred when 45.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = ____kJ(c) If the enthalpy change is 18.0 kJ, how many grams of hydrogen gas are produced?____g(d) How many kilojoules of heat are released when 11.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = ____kJ(e) Calculate E when 750.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K _____kJ HopHelpCh5N1
TUMU Consider these reactions: Reaction 1: H₂(g) + Cl₂(g) → 2HCl(g) AH = -184.6 kJ Reaction 2: 20F 2(g) → O₂(g) + 2 F₂ (g) Reaction 3: N₂(g) +202(g) →→→ 2NO₂(g) Use Reaction 1. Answer: AH = -49.4 kJ Determine the mass, in grams, of chlorine gas consumed (with excess H₂) when 1,152.0 kJ of energy is released from the system. Round to the nearest whole number. g AH = +66.4 kJ