0
This would depend on the temperature of the water before you add the metal and what type of metal it is. if its copper it absorbs heat fast and would not change the temperature much but if you dropped lead into it then it would have to absorb more heat making the temperature lower than the copper. There are too many variables to answer the question.
What else can I help you with?
If a cold piece of metal is placed in an equal mass of warm water will the final temperature be closer to the original temperature of the metal or the water?
The final temperature will be closer to the original temperature of the water. Heat will flow from the water to the metal until they reach thermal equilibrium, resulting in a final temperature between the original temperatures of the two substances.
What effect does the initial temperature of the water have on change in temperature of the water after the hot metal is added?
When hot metal is added into the water then the metal looses its energy into the water and this heat is gained by the water, so the temperature gets increases when hot metal added into it i.e final temperature is greater than initial temperature of water.
What is the final temperature when a 3.0 kg gold bar at 99C is dropped into 0.22 kg od water at 25C?
To find the final temperature, we can use the principle of conservation of energy. We set the heat lost by the gold equal to the heat gained by the water: m_gold * c_gold * (Tf - Ti) = m_water * c_water * (Tf - Ti), where m is mass, c is specific heat capacity, T is temperature, and the subscripts i and f denote initial and final values, respectively. Solving for Tf gives the final temperature of the system.
What is the final temperature when 625 grams of water at 75 degrees loses 7.96?
The final temperature is 59.9°C.
What is the formula for calculating the final temperature when equal masses of water are mixed?
The formula to calculate the final temperature when equal masses of water are mixed is: Final temperature = (m1 x T1 + m2 x T2) / (m1 + m2), where m1 and T1 are the mass and initial temperature of the first sample of water, and m2 and T2 are the mass and initial temperature of the second sample of water.
A hot metal bar is placed into cool water what statement is true?
The temperature of the metal bar decreases.The temperature of the cool water increases.The final temperature of the metal bar will be the same as the final temperature of the water.
If a cold piece of metal is placed in an equal mass of warm water will the final temperature be closer to the original temperature of the metal or the water?
The final temperature will be closer to the original temperature of the water. Heat will flow from the water to the metal until they reach thermal equilibrium, resulting in a final temperature between the original temperatures of the two substances.
What effect does the initial temperature of the water have on change in temperature of the water after the hot metal is added?
When hot metal is added into the water then the metal looses its energy into the water and this heat is gained by the water, so the temperature gets increases when hot metal added into it i.e final temperature is greater than initial temperature of water.
When sodium metal is dropped into a beaker of water a chemical reaction occurs that increases the temperature of the water This is an example of what?
You think probable to an exothermic reaction.
A sample of an unknown metal has a mass of 58.932 g It has been heated to 101.00 C then dropped quickly into 45.20 ml of pure water?
To determine the metal's specific heat capacity, we need more information such as the initial temperature of the metal, the final equilibrium temperature after it's in contact with water, and the temperature change of the water. With this data, we can use the equation q = mcΔT, where q is the heat transferred, m is the mass of the metal, c is the specific heat capacity, and ΔT is the change in temperature.
A 48.26g sample of aluminum at 100.0C is dropped into 34.47g of water at 25.0C What is the final temperature?
To find the final temperature, you can use the principle of conservation of energy, Q lost = Q gained. The heat lost by the aluminum will be equal to the heat gained by the water. Use this formula: (mass of aluminum) x (specific heat capacity of aluminum) x (change in temperature) = (mass of water) x (specific heat capacity of water) x (change in temperature). You can then solve for the final temperature.
What is the final temperature of a 3.0kg bar of gold at 99 degrees Celsius dropped into 0.22kg of water at 25 degrees celsius?
To find the final temperature, we can use the principle of conservation of energy: heat lost by gold = heat gained by water. We can use the formula m * c * ∆T to calculate the heat exchanged. By setting the two heat exchanges equal to each other and solving for the final temperature, we can find that the final temperature is 25.9 degrees Celsius.
When 45g of an alloy at 25 are dropped into 100.0g of water the alloy absorbs 956 j of heat. If the final temperature of the alloy is 37 what is its specific heat?
1.77
Does sand or water have a higher final temperature?
water
What is the final temperature when a 3.0 kg gold bar at 99C is dropped into 0.22 kg od water at 25C?
To find the final temperature, we can use the principle of conservation of energy. We set the heat lost by the gold equal to the heat gained by the water: m_gold * c_gold * (Tf - Ti) = m_water * c_water * (Tf - Ti), where m is mass, c is specific heat capacity, T is temperature, and the subscripts i and f denote initial and final values, respectively. Solving for Tf gives the final temperature of the system.
How will heat flow if an ice cube is dropped in boiling water?
Heat will flow from the boiling water to the ice cube, causing the cube to melt and the water temperature to decrease. The final temperature of the system will depend on the masses and initial temperatures of the ice cube and boiling water.
If water vapours condensate on metal will it increase metal temperature?
yes
