Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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How many litres of C6H14(I), measured at 20 C, must be burned to provide enough heat to warm 25.3 m3 of water from 16.1 to 39.4 C. assuming that all the heat of combustion is transferred to the water, which has a specific heat of 4.18 J a1 C1? Recall that 1 mL 103 L Express your answer to four significant figures and include the appropriate units
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- A chemist carefully measures the amount of heat needed to raise the temperature of a 1.54kg sample of C4H8O from 2.1°C to 19.3°C. The experiment shows that 4.33 x 10^4J of heat are needed. What can the chemist report for the molar heat capacity ofC4H8O? Round your answer to 3 significant digits.arrow_forwardA student is asked to identify an unknown piece of metal. The metal has a mass of 12.34 g. It is placed in a boiling water bath and brought up to 99.98 oC. A coffee-cup calorimeter is set up with 103.25 mL of water (density = 1.00 g/mL and specific heat = 4.184 J/g.oC) at a room temperature of 21.30 oC. The metal is removed from the boiling water and placed in the calorimeter. A final temperature is recorded as 22.32 oC. Find the specific heatcapacity of the unknown metal. (Assume there is no heat loss)arrow_forwardWhen 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)arrow_forward
- A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 4.70 kg of water at 38.7 °C. During the reaction 55.6 kJ of heat flows out of the flask and into the bath. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is -1 4.18 J∙g¯¹·K¯¹. Be sure your answer has the correct number of significant digits. 心。 °℃ x10 Sarrow_forwardIf 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?arrow_forwardExpress the quantity in the unit indicated and designate whether this heat is gained or lost by the substance a. The quantity of heat in calories when 162.5 grams of water undergoes a temperature decrease from 45.84 C to 40.00 C. b. The quantity of heat in Kilojoules when 43.5 Kg of chloroform ,CHCl3 has its temperature changed from 16.8 C to 22.3 C ( sp ht of CHCl3 = 0.971 KJ/kg- C)arrow_forward
- A chemist carefully measures the amount of heat needed to raise the temperature of a 0.46 kg sample of a pure substance from 36.2 °C to 51.6 °C. The experiment shows that 33. kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits.arrow_forwardIn the laboratory a student finds that it takes 145 Joules to increase the temperature of 14.7 grams of solid silicon from 23.0 to 38.0 degrees Celsius. The specific heat of silicon calculated from her data is J/g°C.arrow_forward
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