Physics Lab: Calorimetry and Specific Heat

What is the primary purpose of a calorimeter?

In calorimetry, what is the relationship between the heat lost by a hotter object and the heat gained by a cooler object in an isolated system?

Which of the following is the correct formula to calculate the heat (Q) absorbed or released by a substance?

What does the 's' stand for in the equation $Q = s \cdot m \cdot \Delta T$?

If a calorimeter isn't perfectly insulated and some heat is lost to the surroundings, how would it affect the calculation of the specific heat of a substance?

In the calorimetry experiment, what is the significance of using a weighed amount of a substance?

Why is it important to gently swirl the calorimeter during the experiment?

What does the change in temperature ($\Delta$T) represent in calorimetry calculations?

What is the approximate specific heat of pure water?

Why is it important to avoid dropping the hot substance directly into the calorimeter's beaker or thermometer?

In calorimetry, what is meant by 'thermal equilibrium'?

What is the definition of 'specific heat'?

During the calorimetry experiment involving metal and water, which of the following assumptions is made?

In the context of food calorimetry, what does a higher calorie content indicate?

In food calorimetry, what is being directly measured?

What unit is used to quantify the amount of heat measured in food calorimetry?

Why is distilled water preferred over tap water in calorimetry experiments?

Why is it important to measure the initial temperature of the water in the calorimeter and the hot metal before mixing them?

If the final temperature of the water in a calorimeter is higher than expected, what could be a potential reason?

Consider a scenario where you're using a calorimeter to determine the specific heat of an unknown metal. You notice that the temperature of the water increases rapidly at first, then the rate of increase slows down significantly. What does this observation suggest?

When using the formula $Q = m imes c imes \Delta T$, what condition must be met for Q to be considered negative?

Why are two styrofoam cups used in the calorimeter?

In the food calorimetry experiment, if the cashew nut doesn't completely burn, how would this affect the results?

If 50.0g of a metal at 85°C is placed in 100.0g of water at 22°C, and the final temperature of the water and metal is 25°C, calculate the heat lost by the metal, given that the specific heat of water is 4.184 J/g°C. (Assume no heat loss to the surroundings.)

If 1500 J of energy is added to 100 g of Aluminum, what is the temperature increase if the specific heat of Aluminum is 0.900 J/g°C?

Consider a calorimetry experiment where a 75.0 g metal sample at 90.0°C is placed into 125.0 g of water at 21.0°C. The final temperature of the water and metal is 24.6°C. What is the specific heat of the metal?

What is the purpose of determining the percent yield in the context of a calorimetry experiment?

Why is the calorimeter insulated?

Why is it important to gently swirl the calorimeter during the procedure?

What would be the effect of significantly increasing the volume of water used in the calorimeter?

When determining the calories in food, what is the role of the water that is suspended above the burning food item?

Why must the bulb of the thermometer be submerged in the water during the entire calorimetry process?

What is the crucial reason that each team must keep track of their metal sample? (Imagine, another team has the exact same metal, and your team accidentally swaps! What happens?)

In the equation Qmetal = (ΔTm)(mm)(sm) = Qwater = (∆Tw)(mw)(sw), what do the subscripts 'm' and 'w' refer to?

If you are not using absolute values of (\Delta T), what change needs to be made to the equation Qmetal = Q water?

If 1 calorie is equivalent to 4.184 joules, how many calories are there in 1 joule?

What is 'specific heat capacity' a measure of?

How does specific heat generally compare between water and other substances?

In calorimetry, what does the 'Q' represent in the equation $Q = s \cdot m \cdot \Delta T$?

When a substance cools, how does the value of Q in the equation $Q = s \cdot m \cdot \Delta T$ change?

In calorimetry, which of the following is assumed to be true during the heat transfer process?

What happens to the thermal energy of two objects that are at different temperatures when they come into contact?

What does the equation $Q_{metal} = (\Delta T_m)(m_m)(s_m) = Q_{water} = (\Delta T_w)(m_w)(s_w)$ express?

If the absolute value of (\Delta T) is not used in the equation Qmetal = Q water, what adjustment must be made?

Based on the materials list, what piece of equipment is used to transfer the heated metal into the calorimeter?

During the calorimetry procedure, why should the hot plate only have '2 - 2.5' of water in it?

Why is it important to know which metal sample belongs to your team during the calorimetry experiment?

During the calorimetry procedure, how long should the substance be soaking in the boiling water?

In the context of the experiment, what should you do with the water and the substance after using it in the calorimeter?

When calculating the heat gained by the water in the calorimeter, which equation should you use?

In Part B of the experiment, what is being measured when burning food items?

What unit is typically used to quantify the energy released when burning food items in calorimetry?

What releases more energy when burned: one gram of protein or one gram of fat?

In food calorimetry, the amount of energy contained in a food item is approximated by measuring the heat absorbed by what?

In the food calorimetry experiment, what piece of equipment measures the distilled water?

In the food calorimetry experiment, what is the next step once the cashew catches fire?

Why is it important to measure the initial temperature of the water in the food calorimetry experiment?

Which of the following laboratory equipment are utilized during the food calorimetry experiment?

In a calorimetry experiment, 55.0g of a metal at 93°C is placed into 100.0g of water at 25°C. The final temperature of the water and metal is 29°C. What is the change in temperature of the metal?

In a calorimetry experiment, 55.0g of a metal at 93°C is placed into 100.0g of water at 25°C. The final temperature of the water and metal is 29°C. The specific heat capacity of water is 4.18 J/g°C. How much heat was gained by the water?

In a calorimetry experiment, 55.0g of a metal at 93°C is placed into 100.0g of water at 25°C. The final temperature of the water and metal is 29°C. The specific heat capacity of water is 4.18 J/g°C. The values have been plugged in for H = m x (sh) x (\Delta T) to find the specific heat of the metal, but the value is now negative! What must be done to the absolute value of the answer, to adhere to the rules taught in the passage?

84.0g of a metal are heated to 99°C in a hot water bath, and then placed in a coffee cup calorimeter containing 60.0g of water at 32°C. The final temperature in the calorimeter is 42°C. What is the change in temperature of the water?

84.0g of a metal are heated to 99°C in a hot water bath, and then placed in a coffee cup calorimeter containing 60.0g of water at 32°C. The final temperature in the calorimeter is 42°C. How much heat was gained by the water?

84.0g of a metal are heated to 99°C in a hot water bath, and then placed in a coffee cup calorimeter containing 60.0g of water at 32°C. The final temperature in the calorimeter is 42°C. How much heat was lost by the metal?

84.0g of a metal are heated to 99°C in a hot water bath, and then placed in a coffee cup calorimeter containing 60.0g of water at 32°C. The final temperature in the calorimeter is 42°C. What is the specific heat of the metal?

A 50.0g metal sample is heated to 95.0°C and placed into 100.0g of water at 22.0°C. If the final temperature of the water and metal is 25.5°C, and the specific heat of water is 4.184 J/g°C, how much heat did the water gain?

A 50.0g metal sample is heated to 95.0°C and placed into 100.0g of water at 22.0°C. If the final temperature of the water and metal is 25.5°C, and the specific heat of water is 4.184 J/g°C, the heat gained by the water is 1464.4 J. What is the specific heat of the metal?

A 75.0 g metal sample at 89.0°C is placed into 125.0 g of water at 21.0°C. The final temperature of the water and metal is 24.6°C. Assuming no heat loss to the surroundings and given the specific heat of water is 4.184 J/g°C, determine the amount of heat gained by the water.

A 75.0 g metal sample at 89.0°C is placed into 125.0 g of water at 21.0°C. The final temperature of the water and metal is 24.6°C. Assuming no heat loss to the surroundings and given the specific heat of water is 4.184 J/g°C, the amount of heat gained by the water is 1880.4 J. What is the specific heat of the metal?

A student performs a calorimetry experiment to determine the specific heat of an unknown metal. They find that the experimental specific heat is somewhat lower than the literature value for the metal they believe they used. Assuming they performed the experiment carefully, what could explain this discrepancy?

A student is performing a calorimetry experiment to determine the specific heat of a metal. They use a setup with a metal container instead of styrofoam cups. How would this affect their results, and why?

A student wants to improve the insulation of their calorimeter setup. Which of the following changes would be MOST effective at reducing heat loss to the surroundings?

During a calorimetry experiment, a student observes that the temperature of the water in the calorimeter rises very slowly after adding the heated metal. What could this indicate?

A student performs a calorimetry experiment to determine the specific heat of a metal and forgets to account for the heat absorbed by the calorimeter itself. How will this error affect the calculated specific heat of the metal?

A student is using a bomb calorimeter to measure the energy content of a new snack food. After combusting the food sample inside the calorimeter, they find that the temperature of the water surrounding the bomb increases by only a very small amount, close to the resolution limit of their thermometer. However, upon inspecting the bomb itself, they note that the food sample has completely combusted (burned to ash). What is the most likely source of experimental error?

What is the definition of specific heat capacity, according to the provided text?

In calorimetry, what does the symbol 'Q' represent in the equation $Q = s \cdot m \cdot \Delta T$?

Why should the bulb of the thermometer be submerged in the water when taking measurements during calorimetry experiment?

What is the purpose of using a hot plate and beaker with boiling water in the calorimetry experiment?

What is the key assumption made when calculating heat transfer in a calorimeter?

What happens to the 'Q' value in the equation $Q = s \cdot m \cdot \Delta T$ when a substance is cooled?

In the calorimetry procedure, after heating the metal sample, what is the next step?

In calorimetry experiments, distilled water is preferred over tap water. What is the primary reason for this preference?

What is the likely consequence of using significantly more water than recommended in the hot water can?

What is the purpose of using two nested styrofoam cups in the calorimeter setup?

In calorimetry, why is it important to frequently but gently swirl the calorimeter during the experiment?

Why is it important to avoid dropping the heated metal directly into the calorimeter or thermometer?

If a team accidentally uses another team's metal sample during the calorimetry experiment, what is the most significant consequence?

In the food calorimetry experiment, what does the water suspended above the burning food item measure?

According to the provided text, which type of food releases far more Calories when burned: fat or protein?

During the calorimetry experiment, before combining the metal and the water, you measure the mass of the styrofoam cups and the water. Why do you do this?

In a calorimetry experiment, what is the final step before repeating with a second sample?

What key piece of lab equipment must be used to pick up the metal so that the student does not burn themselves?

What does thermal equilibrium refer to?

If a cashew nut in a food calorimetry experiment does not completely burn, how will this affect the determination of its calorie content?

What is the relationship betwen Joules and Calories?

According to the provided text, what should you do with the water and the metal after using it in the calorimetry experiment?

A student finds the experimental specific heat of a metal to be higher than its literature value. What error could account for this discrepancy?

During a calorimetry experiment, a student observes that it takes a very long time for the water in the calorimeter to reach thermal equilibrium after adding the heated metal. What could this indicate about the experimental setup?

A student measures the energy content of a food item using a bomb calorimeter. However, the temperature of the water and the calorimeter increases only slightly, close to the limit of the resolution of their thermometer. However, the food has completely combusted. What is the most likely reason for this?

In a closed calorimetry experiment, a 50.0 g metal sample at 80.0C is placed into 100.0 g of water at 22.0C. The final temperature of the water and metal is 25.6C. The specific heat capacity of water is 4.184 J/gC. How much energy did the water gain?

In a closed calorimetry experiment, a 50.0 g metal sample at 80.0C is placed into 100.0 g of water at 22.0C. The final temperature of the water and metal is 25.6C. The specific heat capacity of water is 4.184 J/gC. The water gained 1506 Joules. Find the specific heat of the metal.

In a calorimetry experiment, 75.0g of a metal at 100C is placed into 100.0g of water at 22C. The final temperature of the water and metal is 30C. The specific heat capacity of water is 4.18 J/gC. What is the mass of the water?

81.0g of a metal are heated to 97C in a hot water bath, and then placed in a coffee cup calorimeter containing 66.0g of water at 32C. The final temperature in the calorimeter is 44C. The specific heat capacity of water is 4.18 J/gC. How much heat did the water gain?

81.0g of a metal are heated to 97C in a hot water bath, and then placed in a coffee cup calorimeter containing 66.0g of water at 32C. The final temperature in the calorimeter is 44C. The change in temperature of the water is 12C, and the heat gained by the metal is 3306.24 J. What is the specific heat of the metal?

What is the purpose of repeating the calorimetry procedure with a second sample?

What piece of equipment is used measure 100ml of distilled water?

What should you measure using the analytical balance?

What is the next step once the cashew immediately catches fire?

A student heats a metal sample in boiling water before dropping it into a calorimeter, but forgets to record the temperature of the boiling water. How will this affect their calculations?

A student is using a coffee cup calorimeter to measure the heat of reaction of a chemical process. To improve the accuracy of the experiment, what is the most important modification they should make to the setup?

What is likely to happen as the water reaches thermal equilibrium with the metal?

Why is the mass of samples important?

When measuring the calories in food, what must immediately happen once the cashew catches fire?

Why must the thermometer bulb be fully submerged?

Which equation presented in the provided document should used when calculating heat gained by water?