4. Andy has a bath and uses 1500g of water heated from 10°C to 40°C and with a specific heat capacity of 42001/kg C. How much energy does he use? 5. An electric kettle supplies 20,000] of energy to heat 0.5kg of water. What is the temperature change? The specific heat capacity of water is 42001/kg C. 6. A piece of lead with a specific heat capacity of 126J/kg°C is given 5000] of energy to heat it from 20°C to 250°C. What was the mass of the piece of lead? 7. A2 kg metal cylinder is supplied with 1600J of energy to heat it from 5°C to 13°C. What is the specific heat capacity of the metal?

4. Andy has a bath and uses 1500g of water heated from 10°C to 40°C and with a specific heat capacity of 42001/kg C. How much energy does he use? 5. An electric kettle supplies 20,000] of energy to heat 0.5kg of water. What is the temperature change? The specific heat capacity of water is 42001/kg C. 6. A piece of lead with a specific heat capacity of 126J/kg°C is given 5000] of energy to heat it from 20°C to 250°C. What was the mass of the piece of lead? 7. A2 kg metal cylinder is supplied with 1600J of energy to heat it from 5°C to 13°C. What is the specific heat capacity of the metal?

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...

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2.Can you help me solve this
2. A 32.5g cube of aluminum initially at 45.8°C is submerged into 105.3 g of water at 15.4°C. The final temperature is 17.3°C. What is the heat capacity of aluminum? Swater = 4.184 J/g°C.
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A chemistry student dissolved 4.51 g of sodium hydroxide in 100.0 mL of water at 19.5 ºC (in a calorimeter cup). As the sodium hydroxide dissolves, the temperature of the surrounding water increases to 31.7 ºC. Determine the heat of solution of the sodium hydroxide in J/g. Specific heat of water = 4.184 J/g•ºC Select one: a.– 1182 J/g b.+1132 J/g c.+1180 J/g d.– 1132 J/g
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An 87.9 g sample of chromium metal at 99.1°C is placed in a calorimeter containing 100.00 g of water at 21.0°C The contents of the calorimeter come to a temperature of 25.7°C. The heat capacity of water is 4.18 J/(g* °C) a. Is this process exothermic or endothermic? b. Calculate the amount of heat released by the metal (q metal) in Joules. Show your work.
Can you explain where did I go wrong, I keep getting the same answer.
A 50.0-g piece of metal at 80.0 °C is placed in 100 g of water at 22.0 °C contained in a calorimeter like that shown in Figure 5.12. The metal and water come to the same temperature at 24.6 °C. Water has a heat capacity of 4.18 J/g°C. a. How much heat did the metal give up to the water? b. What is the specific heat capacity of the metal? c. If it is one of the substances found in Table 5.1, what is its likely identity?
Together, a pure gold ring and a pure titanium ring have a mass of 15.07 g. Both rings are heated to 94.90 °C and dropped into 13.0 mL of water at 16.80 °C. The water and the rings reach thermal equilibrium at a temperature of 24.20 °C. The density of water is 0.998 g/mL... The specific heat capacity of water is 4.18, the specific heat capacity of gold is 0.129 and the specific heat capacity of titanium is 0.544 Calculate the mass of each ring. mass of gold ring: mass of titanium ring: 50 60