Questions and Problems gyam Oriollo Q2 When water is heated, the temperature eventually reaches a constant...
Can anyone tell me if my calculations are correct? Water Volume and Temperature Data Water Volume (mL) Temperature (C) Initial 70mL 28.0oC Final 95mL 2.0oC System Heat Data Mass of water (g) 70.0g Mass of ice cube (g) 23.0g Change in water temperature (C) 26.0Co Change in ice temperature (C) 2.0Co Heat lost by water (J) 7618.5J Heat gained by ice after melting (J) 95.827J Heat used to melt ice (J) 7522.7Jsigfig Theoretical heat to melt ice (J) 7656.9J sigfig...
5.175 g of water was heated from 15 °C to 88 °C. How many kilocalories were absorbed by the water? Given water has a specific heat of 1.00 cal/g °C. [10 pts.] 6. What are the products formed in an acid-base neutralization reaction? [3 pts.] A) an acid B) a base C) a salt and water D) an acid and water 7. The anhydrous compound that will absorb water from the atmosphere is. [2 pts.] a) hygroscopic b) a hydrate...
If 80.00 g of water at 22.3°C is heated so that the water reaches a temperature of 33.2°C then how much heat did the water gain? (Q > 0) Use 0.99823 cal/g°C as the specific heat of water. Report your answer to two (2) decimal places.
What mass of ice would it take to lower the temperature of 0.5kg of water from 20°C to 0°C. 7. A 100-g piece of iron is heated to 100°C and then dropped into a cavity in a large block of ice at 0°C. How much mass of ice will melt? 8. 50 grams of hot water at 80°C is poured into a cavity in a very large block of ice at 0°C. The final temperature of the water in the...
What mass of ice would it take to lower the temperature of 0.5kg of water 20°C to 0°C. 7. from A 100-g piece of iron is heated to 100°C and then dropped into a cavity in a large block ofice at 0°C. How much mass of ice will melt? 8. 50 grams of hot water at 80°C is poured into a cavity in a very large block ofice at 0°C. The final temperature of the water in the cavity is...
Initial mass of ice = 150.89 g Final mass of ice = 99.69 g Initial temperature of water = 42 °C Final temperature of water = 0.4 °C Determine the mass of the ice that has melted. Determine the variation of the water temperature (ΔT). a) Calculate the energy (in J) released by 100 g of water when it cooled by ΔT. The specific heat capacity(c) of water is 4.18 J/(g°C). Use the formula Q = mcΔT and the mass...
You have a block of ice at a temperature of -100°C. This block of ice is made from 180g H2O. The block of ice will be heated continually until it becomes super-heated steam at a temperature of 200°C Cice = 2.03 J/g-K ΔHfus=6.01 kJ/mol Cwater = 4.18 J/g-K Csteam = 1.84 J/g-K ΔHvap=40.67 kJ/mol What is the enthalpy change raising the temperature of 180 g of ice at −100 °C to 0°C? What is the enthalpy change upon melting 180...
A 25 g cube of metal was heated in a hot temperature bath to 80oC and then added to 50 mL of deionized water. Using the following graph, explain how you would determine the temperature change that has occurred in the system. The metal was added to the calorimeter (Styrofoam cup with water) at 180 seconds. What is the initial temperature of the water and the metal? What is the final temperature of the metal and the water? What occurred...
How many kilojoules are required to change the temperature of 44.5 g of water from 21.4 °C to 39.3 °C ? 10 APR ?
Jor General, Orgmic, and Biological Chemistry Calculations 8. AT(C) for water (7-6) First run Second run 9. Mass of water (4-3) 52.11 10. Heat (J) gained by water (Show calculations.) TeMp Chonye1-4.87 Temp 5213.91 X41 CNORC 2-3-54C Heat Gan tor waker 9XATXSHH2) 8.4134 -184 11. Heat (J) lost by the metal Heat (J) lost by metal Heat (J) gained by water (10) Th-01O 76-590 13. Specific heat of the metal g "C)3573 27654 9863 12. AT (C) for metal (5-7)...