Calorimetry - Page 5
Questions
- How much heat is needed to raise the temperature of 5.58 kilograms of iron from 20.0°C to 1000.0°C?
- How will the temperature of a calorimeter solution change for an exothermic reaction?
- What minimum mass of ice is needed so that a glass of water at #25^@ "C"# is cooled down to #0^@ "C"# before the ice completely melts?
- Why is bomb calorimetry important?
- If 980 kJ of energy are added to 6.2 L of water at 291 K, what wil the final temperature of the water be?
- How is calorimetry used in the industry?
- To what temperature will a 50.0 g piece of glass raise if it absorbs 5275 joules of heat and its specific heat capacity is 0.50 J/g°C, if the initial temperature of the glass is 20.0°C?
- The temperature of 50.0 g of water was raised to 50.0°C by the addition of 1.0 kJ of heat energy. What was the initial temperature of the water?
- What is an equation that you can use to find the number of Calories in any number of grams of trail mix?
- Why do we often write the water product as a gas in complete combustion reactions?
- A sample of substance X that has a mass of 326.0 g releases 4325.8 cal when it freezes at its freezing point. If substance X has a molar mass of 58.45 g/mol, what is the molar heat of fusion for substance X?
- If you combine 250.0 mL of water at 25°C and 120.0 mL of water at 95°C, what is the final temperature of the mixture?
- In calorimetry, we often define #q_(sys) = 0#. What assumptions about the calorimeter make this possible?
- Why does water take so long to heat up or cool down?
- An ancient copper coin was found to absorb 545.8 J of heat when the temperature increases 31.4 C°. The specific heat of copper is 0.387 J/g°C. What is the mass of the copper coin?
- How many calories are required to raise the temperature of a 35.0 g sample of iron from 25°C to 35°C? Iron has a specific heat of 0.108 cal/g°C?
- Mass spectroscopy is an analytical technique which involves ? a. production of gaseous ions from a sample b. separation of the gaseous ions c. measurement of the relative abundance of the gaseous ions d. all of the above
- A piece of gold initially at a temperature of 25.1 °C absorbs 675 J of heat, raising its temperature to 57.4 °C. Assuming the specific heat of gold is 0.126 J/(g°C), what is the mass of the sample?
- What information do you get from a differential scanning calorimetry plot?
- If a #25.00g# piece of copper (#C_s = (0.385J)/(g*°C)#) at #115.0°C# is added to #50.00g# of water (#C_s = (4.184J)/(g*°C)#) at #25.00°C#, what is the final temperature once the object and water thermally equilibrate?