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∙ 6y agoT = 28.9°C + 1.7°C/hr × 3 hr - 0.5°C/hr × 4 hr
= 28.9°C + 5.1°C - 2 °C
= 32°C
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∙ 6y agoYou need the heat capacities for these substances in order to answer this question. If you have those, it's simple algebra.
If the temperature was -25°C and rose 19°C, it would reach a temperature of -6°C. If it then fell 8°C, the final temperature would be -14°C.
Use the ideal gas equation to solve this. PV= nRT. You will have to convert your pressure to atmosphere to use the constant R = 0.0821 L*ATM/mol*K. You know your initial pressure, volume, and temperature. Moles can be neglected (n) because they will stay the same. You also know your final pressure and final volume, so you can solve for final temperature.
This is the formula for finding calories: calories= (Tf-Ti)mass Or, in words, you subtract the final temperature (the temperature of the fused waters) by its initial temperature (the hot/ cold water's original temperature). You then multiply this answer by the mass of the water before you mix them together. Your hot and cold water should both have the same mass, but not the same temperature.
42.3 C
The relation is:[K] = [oC] + 273,15
To find the final temperature of each substance, you need to calculate the specific heat capacity of each substance. Once you have the specific heat capacity, you can use the formula Q = mcΔT to find the final temperature. Substituting the given values into the formula will give you the final temperature of each substance.
Using the specific heat capacity of aluminum (0.897 J/g°C), you can calculate the change in temperature using the formula Q = mcΔT, where Q is the heat absorbed (725J), m is the mass of aluminum block (55g), c is the specific heat capacity, and ΔT is the change in temperature. Rearranging the formula to solve for ΔT and substituting the values, you can then find the final temperature by adding the change in temperature to the initial temperature (27.5°C). Calculate and the final temperature of the aluminum block will be the sum of the initial temperature and the change in temperature.
To find the final volume of the balloon, you would need to use the ideal gas law equation. V2 = V1 * (T2 / T1), where V1 is the initial volume, T1 is the initial temperature, T2 is the final temperature (in Kelvin), and V2 is the final volume. Convert temperatures to Kelvin (25C = 298K, 50C = 323K) and then calculate the final volume.
Sample B had the lowest final temperature.
The final temperature of the ice block can be calculated using the formula: Q = mcΔT, where Q is the heat removed, m is the mass of the ice block, c is the specific heat capacity of ice, and ΔT is the change in temperature. Given the data, you can find the final temperature of the ice block.
To find the final temperature, we can use the principle of conservation of energy, assuming no heat is lost to the surroundings. The heat lost by the coffee equals the heat gained by the milk. Using the equation: mcΔT = mcΔT, where m is mass, c is specific heat capacity, and ΔT is the temperature change, you can calculate the final temperature.
The final temperature is 59.9°C.
The final temperature of the coffee in the thermos after the ice cubes melt can be calculated using the principle of conservation of energy. The heat lost by the coffee as it cools down will be equal to the heat gained by the ice cubes as they melt. By applying this principle along with the specific heat capacities of water and ice, you can determine the final temperature of the coffee.
You need the heat capacities for these substances in order to answer this question. If you have those, it's simple algebra.
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.
To calculate the final temperature of the water, we need additional information such as the initial temperature of the second substance and their specific heat capacities. Without this information, we cannot provide an accurate answer.