What would the effect on the specific heat of your metal if one drop (0.05mL) of water at 100 degrees Celsius remained on your metal? the effect would cause the specific heat to be much higher none of these choices are correct the effect would cause the specific heat to be much lower the effect would be negligible

What would the effect on the specific heat of your metal if one drop (0.05mL) of water at 100 degrees Celsius remained on your metal? the effect would cause the specific heat to be much higher none of these choices are correct the effect would cause the specific heat to be much lower the effect would be negligible

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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Similar questions

Which statement best defines specific heat? The amount of heat required to increase the temperature of 1 mol of a substance by 1 °C. The amount of heat required to increase the temperature of a specific object, such as a calorimeter, by 1 °C. The amount of heat required to increase the temperature of 1 g of a substance by 1 °C. The amount of heat required to increase the temperature of 1 L of a substance by 1 °C.
A hot 105.9 g lump of an unknown substance initially at 154.0 °C is placed in 35.0 mL of water initially at 25.0 °C and the system is allowed to reach thermal equilibrium. The final temperature of the system is 36.2 °C. Using this information and the specific heat values for several metals in the table, identify the unknown substance. Assume no heat is lost to the surroundings. rhodium ○ graphite titanium zinc tungsten aluminum Substance Specific heat (J/(g∙°C)) aluminum 0.897 graphite 0.709 rhodium 0.243 titanium 0.523 tungsten 0.132 zinc 0.388 water 4.184
If the same amount of heat is added to 5.00 g samples of each of the metals below, which metal will experience the largest temperature change? Metal Specific Heat Capacity (J/g-K) A 0.753 B 0.129 C 0.385 D 0.449 E 0.897
How much heat is needed to raise the temperature of a 2.5 g piece of copper wire from 20. °C to 80. °C? How much heat is needed to increase the temperature of an equivalent mass of aluminum by the same amount? Once heated, which metal will cool faster?
Suppose you place equal amounts of 70.0°C and 20.0°C water next to each other in an insulated box with the two samples separated by a thin piece of metal. Assuming no heat is lost to the surroundings, what is the final temperature of the two samples of water? 25.0°C 55.0°C 45.0°C 20.0°C
Specific Heats of Substances Substance Specific Heat g-°C Brick 0.20 Ethanol 0.58 0.10 pooM Calculate the amount of heat, in calories, that must be added to warm 70.9 g of brick from 19.3 °C to 41.0 °C. Assume no changes in state occur during this change in temperature. heat added: cal Calculate the amount of heat, in calories, that must be added to warm 70.9 g of ethanol from 19.3 °C to 41.0 °C. Assume no changes in state occur during this change in temperature. heat added: cal
How many calories are released as 50 g of water cools from 100 °C to 25 °C? Specific heat of water is 1.00 cal/g. °C.
If you drop a 150 gram piece of metal that has a temperature of 125 Celsius into 1000 grams of water at 20 Celsius, what best describes what would occur? More heat will be lost by the metal than gained by the water. The temperature of the water will be greater than the amount of heat lost by the metal. The temperature change of the metal will equal the temperature change of the water. The heat lost by the metal will equal the heat gained by the water.
How much heat would have to be absorbed by 2000 g of water to change its temperature from 20°C to 50°C? Use the value 4.2 J/mol °C for the specific heat of water.
Suppose you place equal amounts of 60.0°C and 20.0°C water next to each other in an insulated box with the two samples separated by a thin piece of metal. Assuming no heat is lost to the surroundings, what is the final temperature of the two samples of water?
A solution is made by mixing 232.0 mL of ethanol initially at 12.7 ∘C with 232.0 mL of water initially at 22.5 ∘C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL. The specific heat of ethanol is 2.46 J/g·°C and the specific heat of water is 4.184 J/g·°C ?f= ∘C
A 10.0g sample of water at 24C is mixed with 30.0 g of water at 48C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The specific heat of water is 4.18J/gC.