58. A 54 cm³ ice cube at -25.0 °C is added to a thermally insulated container with 400.0 mL H2O(1) at 32.0 °C. What will be the final temperature in the container and what state(s) of matter will be present? (Specific heats: H2O(s), 2.01 J ¬1°C¯1; H0(1), 4.18 Jg °C¯1. Densities: H20(s), 0.917 g/cm³; H2O(1), 0.998 g/cm³. Also, AfusH of ice = 6.01 kJ mol-1.)

58. A 54 cm³ ice cube at -25.0 °C is added to a thermally insulated container with 400.0 mL H2O(1) at 32.0 °C. What will be the final temperature in the container and what state(s) of matter will be present? (Specific heats: H2O(s), 2.01 J ¬1°C¯1; H0(1), 4.18 Jg °C¯1. Densities: H20(s), 0.917 g/cm³; H2O(1), 0.998 g/cm³. Also, AfusH of ice = 6.01 kJ mol-1.)

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

What amount of heat (in kJ) is required to convert 14.7 g of an unknown liquid (MM 67.44 g/ = mol) at 43.5 \deg C to a gas at 128.2 \deg C? (specific heat capacity of liquid = 1.18 J/g. \ deg C; specific heat capacity of gas = 0.792 J/g. \deg C; A Hvap = 30.1 kJ/mol; normal boiling point, Tb = 97.4 \deg C)
2. a) The ingredients contained in grape Kool-Aid can be approximated as: water (H2O, density = 1.000 g/mL), • sugar (sucrose, solid at room temperature, C12H22011), • citric acid (solid at room temperature, CeHsO7), and grape flavouring (methyl anthranilate, liquid at room temperature, C&H&NO2, density = 1.168 g/mL). (The blue and red dyes used to produce the purple colour are present in such small quantities that they can be ignored.) A sample of grape Kool-aid having a final total volume of 500 mL can be prepared from: 485 mL of water, 32.0 g of sugar, 5.00 g of citric acid, and • 3.50 g or grape flavouring. Calculate the molarity and molality of grape flavouring in this mixture (assume that only water is the solvent). Fun fact: methyl anthranilate is also used as a bird repellant (to keep geese away).
How much heat, in joules and in calories, must be added to a 89.1 g chromium block with a specific heat of 0.450 J/g·°C to increase its temperature from 25°C to its melting temperature of 1907°C?
At 307 K, the vapor pressure of a liquid is 15 kPa, and at 389 K, it’s vapor pressure is 121 kPa. Use this information to estimate the enthalpy of vaporization in kJ. R= 8.314 J/(mol*K) (Please type answer)
What amount of heat (in kJ) is required to convert 12.6 g of an unknown liquid (MM = 67.44 g/mol) at 43.5 °C to a gas at 128.2 °C? (specific heat capacity of liquid = 1.18 J/g･°C; specific heat capacity of gas = 0.792 J/g･°C; ∆Hvap = 30.1 kJ/mol; normal boiling point, Tb = 97.4°C)
A 0.528 g0.528 g sample of steam at 103.5 ∘C103.5⁢ ∘C is condensed into a container with 4.51 g4.51 g of water at 15.0 ∘C.15.0⁢ ∘C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18 J g⋅ ∘C,4.18 J g⋅ ∘C, the specific heat of steam is 2.01 J g⋅ ∘C,2.01 J g⋅ ∘C, and Δ?vap=40.7 kJ/mol.
How much heat(in kJ) is absorbed when 75.0g of benzene at -15°C is cooled to 35°C? mp = 5.85°C, c(l) = 1.71 J/g°C,c(s) = 1.51 J/g°C, ΔH(fus) = 9.9 kJ/mol
An ice cube with a mass of 45.4 g at 0.0 °C is added to a glass containing 374 g of water at 45.0 °C. Determine the final temperature of the system at equilibrium. The specific heat capacity of water, C, is 4.184 J/g.°C, and the standard enthalpy of fusion, AH; , of water is 6.01 × 10° J/mol. Assume that no energy is transferred to or from the surroundings. fus T = °C TOOLS x10 Question Source: Atkins 7e - Chemical Principles| Publisher: W.H. Fre
Which equation calculates the temperature change of 100 g of water that absorbs the same amount of heat as it takes to boil 5 g of water? Question 12 options: (100 g / 18 g mol–1 × 40650 J mol–1) / (5 g × 4.184 J g–1 °C–1) (5 g / 18 g mol–1 × 40650 J mol–1) / (100 g × 4.184 J g–1 °C–1) (100 g × 4.184 J g–1 °C–1) / (5 g / 18 g mol–1 × 40650 J mol–1)
Two 20.0 g ice cubes at –16.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T;, of the water after all the ice melts. heat capacity of H,O(s) 37.7 J/(mol·K) Tf = heat capacity of H,O(l) 75.3 J/(mol-K) enthalpy of fusion of H,O 6.01 kJ/mol
What amount of heat (in kJ) is required to convert 10.8 g of an unknown liquid (MM = 83.21 g/mol) at 19.2 °C to a gas at 93.5 °C? (specific heat capacity of liquid = 1.58 J/g. °C; specific heat capacity of gas = 0.932 J/g⋅ °C; AHvap = 22.5 kJ/mol; normal boiling point, Tb = 57.3 °C)
A 0.580 g0.580 g sample of steam at 107.3 ∘C107.3⁢ ∘C is condensed into a container with 4.56 g4.56 g of water at 17.0 ∘C.17.0⁢ ∘C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18 J g⋅ ∘C,4.18 J g⋅ ∘C, the specific heat of steam is 2.01 J g⋅ ∘C,2.01 J g⋅ ∘C, and Δ?vap=40.7 kJ/mol.