Aqueous ethylene glycol is commonly used in car radiators as an antifreeze and coolant. A 50% ethylene glycol solution in a radiator has a specific heat capacity, c, of 3.5 J/gC. If a 4.0 kg quantity of ethylene glycol absorbs 250 kJ of thermal energy, what was the temperature ciange, AT, of the solution? Assume the radiator is a closed system.

Aqueous ethylene glycol is commonly used in car radiators as an antifreeze and coolant. A 50% ethylene glycol solution in a radiator has a specific heat capacity, c, of 3.5 J/gC. If a 4.0 kg quantity of ethylene glycol absorbs 250 kJ of thermal energy, what was the temperature ciange, AT, of the solution? Assume the radiator is a closed system.

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

When the Cacl2(s) is added to water, the following reaction occurs. Cacl (s) – Ca²"(aq) + 2CI"(aq) AH = - 81.5 kJ A 24.1 g sample of Caclz is dissolved in water, with both substances at 25.0 °C. Calculate the final temperature (in °C) of the solution assuming no heat is lost to the surroundings, the final solution, containing Cacl2 and water, has a mass of 100.0 g and the solution has a specific heat capacity of 4.18 J °c-lg-1. The molar mass of CaCl2 = 110.98 g/mol Do not include units in your answer, If you round during your calculations make sure to keep at least 3 decimal places. Report your answer to one (1) decimal place. Answer: 59.0 The correct answer is: 67.3
You are performing an experiment where you place 9.2113 g of Al metal at 205.02 C into a coffee cup calorimeter that contains 98.4 g of water at 25.05 C. The final temperature of the water in the coffee cup is 28.89 C.Calculate the heat (q), in J, gained by the water using the equation, , given cwater= 4.184 J/g°CDo not include units. If you need to express your answer as an exponential number, use this template: 1445 should be typed as 1.445e+003
A 79.1 g sample of an unknown solid is heated to 62.6ºC and placed into a calorimeter containing 92.1 g of water at 22ºC. If the final temperature of the solid sample and the water is 32.5ºC, what is the specific heat of the solid? Please provide your final answer rounded to two decimal places.
A 0.491 kg sample of an unknown metal loses 4.08 kJ of heat. If the change in its temperature was 22.4°C, calculate the specific heat capacity of the J metal in units if g°C
Determine the change in enthalpy (H, in J) transferred when 8.0 g of sucrose (C12H22O11)are dissolved in 92.0 g of water in a coffee cup calorimeter. The temperature of the solution changesfrom 15.0 °C to 14.7 °C Assume the process takes place at constant pressure, the masses areadditive, and the specific heat of the solution is 4.18 J/g∙°C.
A house is built with a granite countertop. The heat capacity of the countertop is 156.0 kJ/°C. A hot pan of water is placed on the countertop, and 7500 J of heat energy is transferred into the countertop. By how much does the temperature of the countertop change?
4
How many grams of an unknown substance, having a specific heat of 1.66 J g ° C, are present if a temperature change of -173.4 K occurs. The heat lost was 35981 J.
What quantity of heat (in kJ) will be released if 0.1673 mol of NH³ are mixed with 0.200 mol of O: in the following chemical reaction? 4 NH (g) + O: (g) → 2 N₂H4 (g) + 2 H₂O (g) AH = -286 kJ/mol
A chemist carefully measures the amount of heat needed to ralse the temperature of a 1.48 kg sample of C,H,0, from 32.9 °C to 50.0 °C. The experlment 4-8 2 shows that 4.02 x 10* J of heat are needed. What can the chemist report for the molar heat capacity of C,H,0,? Be sure your answer has the correct number of significant digits.
A 22.86 g sample of a substance is initially at 26.5 ∘C. After absorbing 574 cal of heat, the temperature of the substance is 194.6 ∘C. What is the specific heat (??)(S⁢H) of the substance?
When one mole of C6H6 is burned, 3.27 MJ of heat is produced. When the heat from burning 5.27 g of C6H6 is added to 5.69 kg of water at 21.0 ∘C, what is the final temperature of the water?