03:20Thermal Equilibrium, Temperature and Temperature Scales | A-level Physics | AQA, OCR, EdexcelSnapRevise462views
Multiple ChoiceIf 53.2 g Al at 120.0 ºC is placed in 110.0 g H2O at 90 ºC within an insulated container that absorbs a negligible amount of heat, what is the final temperature of the aluminum? The specific heat capacities of water and aluminum are 4.184 J/g ∙ ºC and 0.897 J/g ∙ ºC, respectively.1713views2rank4comments
Open QuestionSuppose a 50.0 g block of silver (specific heat = 0.2350 J/g∙°C) at 100°C is placed in contact with a 50.0 g block of iron (specific heat = 0.4494 J/g∙°C) at 0°C, and the two blocks are insulated from the rest of the universe. the final temperature of the two blocks291views
Open QuestionA 2.74-g sample of a substance suspected of being pure gold is warmed to 72.1 °C and submerged into 15.2 g of water initially at 24.7 °C. The final temperature of the mixture is 26.3 °C. What is the heat capacity of the unknown substance? Could the substance be pure gold?
Open QuestionA copper cube with an edge measuring 1.55 cm and an aluminum cube with an edge measuring 1.62 cm are both heated to 55.0 °C and submerged in 100.0 mL of water at 22.2 °C. What is the final temperature of the water when equilibrium is reached? (Assume a density of 0.998 g/mL for water.)
Open QuestionA pure gold ring and a pure silver ring have a total mass of 14.9 g. The two rings are heated to 62.0 °C and dropped into 15.0 mL of water at 23.5 °C. When equilibrium is reached, the temperature of the water is 25.0 °C. What is the mass of each ring? (Assume a density of 0.998 g/mL for water.)
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