To determine whether a shiny gold-colored rock is actually gold, a chemistry student decides to measure its heat capacity. She first weighs the rock and finds it has a mass of 3.2 g. She then finds that upon absorption of 56.4 J of heat, the temperature of the rock rises from 25 °C to 52 °C. Substance Elements Lead Gold Silver Copper Iron Specific heat capacity, Cs (J/(g. °C))* 0.128 0.128 0.235 0.385 0.449 0.903 Aluminum Compounds Ethanol Water Materials Glass (Pyrex) 0.75 Granite 0.79 Sand 0.84 * At 298 K. 2.42 4.18 Find the specific heat capacity of the substance composing the rock. Express the specific heat in joules per gram-Celsius to two significant figures. C₁ = Submit Part B ΠΙ ΑΣΦΑ Submit Request Answer Provide Feedback Determine whether the value is consistent with the rock being pure gold by referring to the table. ? O Yes, the value is consistent with the rock being pure gold. O No, the value is inconsistent with the rock being pure gold. J/g. °C Request Answer

When pure sulfuric acid is dissolved in water, heat is evolved. 10.65 g of pure sulfuric acid at 20.00 °C was added to a calorimeter containing 300 g of water at 20.00 °C. The temperature of the solution increased to 26.35 °C. If the specific heat of the mixture is 4.184 Jg1°C1, the density of water is 1 g/mL, and the heat capacity of the calorimeter is ignored, what is the heat evolved per mole of sulfuric acid? a. -83.2 kJ O b. -73.6 kJ O C. -76.0 kJ d. -80.8 kJ e. -78.4 kJ

In a calorimetric experiment, 6.24 g of lithium hydroxide, LIOH, was dissolved in water. The temperature of the calorimeter rose from 25.0°C to 36.7°C. What is AH for the solution process? LIOH(s) + Li* (aq) + OH (ag) The heat capacity of the calorimeter and its contents is 547 J/°C. ΔΗ- kl/mol

When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)

The table lists the specific heat capacities of select substances. Substance Specific heat capacity (J/g °C) lead 0.128 silver 0.235 copper 0.385 iron 0.449 aluminum 0.903 water 4.184 An unknown substance has a mass of 19.5 g.19.5 g. The temperature of the substance increases by 16.1 ∘C16.1⁢ ∘C when 73.8 J73.8 J of heat is added to the substance. What is the most likely identity of the substance?

A chemist carefully measures the amount of heat needed to raise the temperature of a 1.54 kg sample of C5H₁2S from 5.8 °C to 17.4 °C. The experiment shows that 3.51 × 104 J of heat are needed. What can the chemist report for the molar heat capacity of C5H₁2S? Be sure your answer has the correct number of significant digits. 12 - 1 – 1 K J. mol x10 X Ś 6 0 U

A chemist carefully measures the amount of heat needed to raise the temperature of a  1.10kg  sample of a pure substance from  −6.3°C  to  10.7°C . The experiment shows that  8.40kJ  of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits.

If 30.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The Δ H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g C) and that no heat is gained or lost by the container, what will be the final temperature of the solution?

A chemist carefully measures the amount of heat needed to raise the temperature of a 1.65kg sample of C9H10O2 from 25.9°C to 37.9°C. The experiment shows that 3.09 X 104J of heat are needed. What can the chemist report for the molar heat capacity of C9H10O2? Round your answer to 3 significant digits.   =   J * mol-1 * K-1

Calculate the energy required to heat 141.0mg of mercury from −1.1°C to 17.8°C . Assume the specific heat capacity of mercury under these conditions is 0.139J·g−1K−1 . Be sure your answer has the correct number of significant digits.