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 16.1 g. The temperature of the substance increases by 18.7 °C when 70.8 J of heat is added to the substance. What is the most likely identity of the substance? copper silver iron lead aluminum water

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 16.1 g. The temperature of the substance increases by 18.7 °C when 70.8 J of heat is added to the substance. What is the most likely identity of the substance? copper silver iron lead aluminum water

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

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)
Food contains three main categories of compounds: carbohydrate, protein, and fat. Arctic explorers often eat a high-fat diet because fats have a high food value. The average food values for carbohydrate, protein, and fat are 4 Cal/g, 4 Cal/g, and 9 Cal/g, respectively. Consider a typical fat to have the chemical formula C18H36O2, glucose (C6H12O6) to be a representative carbohydrate, and the amino acid alanine (C3H6NO2) a building block of proteins. Express the food values given above in kJ/mol.
Which of the following reactions is exothermic? C2H4(g) + O2(g) → 2C(s) + 2H2O(g) AH = 469.2 kJ O N204(g) + 57.6 kJ → 2NO2(g) C2H4(g) + 302(g) → 2CO2(g) + 2H2O(g) > AH = 1322.9 kJ PCI3(g) + Cl2(g)→ PCI5(g) + 92.5 kJ
When 3.8 g A are reacted with 8.5 g D, according to the balanced chemical equation below, 33 kJ of energy are released. Please calculate the enthalpy for this reaction when 3 moles of G are produced. 2A + 3D = 2Z + 3G given molar masses: A = 141.8 g/mole D = 63.996 g/ mole Z = 4.032 g/ mole G = 56.028 g/ mole
A 4.81 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. If 3.12 × 10³ J of heat was gained by the solution, what is the total heat for the dissolution reaction of the 4.81 g of salt? How many moles of the unknown salt were used in the reaction ? _______ J?
1. A thermometer placed in a solution undergoing a chemical reaction indicates an increase in temperature as the reaction proceeds. Is this reaction endothermic or exothermic? Describe if heat energy is lost or gained from the reaction (the system) to the surroundings. What is the sign of the enthalpy change (AH) of this reaction? 2. A student performs a reaction and determines the enthalpy change (AH) to be 31.4 kJ. Will the temperature of the surrounding solution increase or decrease as a result of this chemical process? 3. If you hold 3 grams of ice in your hand at room temperature, your hand will become cold. a) Is the reaction H,O(s) – H,O(1) endothermic or exothermic? b) In which direction does heat flow?
Determine the most likely identity of the unknown metal sample. Mass of empty beaker = 50.45 g Mass of beaker and water = 81.26 g Mass of water 30.81 g (represents a calculation rather than a direct measurement) Initial water temperature = 25.5 C Mass of metal = 54.02 g Initial metal temperature = 102.5 C Final water and metal mixture temperature = 36.0 C The specific heat capacity of water is 4184 J/kg C
When a 6.50 g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature of the water rises from 21.6 to 37.8oC. Was the chemical reaction (dissolving the solid) endothermic or exothermic? How do you know? Write a balanced chemical equation for this process. Determine how many joules of heat (q) were involved in changing the temperature of the water. If the heat that changed the temperature of the water was a result of the chemical reaction, determine the ΔH of the chemical reaction in kJ/mol of sodium hydroxide.
Silane, SiH4, burns according to the reaction, SiH4 + 2O2 → SiO2 + 2H2O, with ΔH° = –1429 kJ. How much energy in kJ is released if 18.01 g of silane is burned? Atomic Mass: Si: 28.086 g/mol H: 1.008 g/mol O: 15.999 g/mol Round your answer to 2 decimal places. Silane, SiH4, burns according to the reaction, SiH4 + 2O2 → SiO2 + 2H2O, with ΔH° = –1429 kJ. How much energy in kJ is released if 18.01 g of silane is burned? Atomic Mass: Si: 28.086 g/mol H: 1.008 g/mol O: 15.999 g/mol Round your answer to 2 decimal places.
A piece of metal with a specific heat of 1.153 J/gºC is heated to 124.6ºC and then placed in 120.382 g of water which is at a temperature of 2.1 ºC. After a minute, the temperature of the water has stopped changing and is now 45.5ºC. Assuming that there are no heat losses to the container or surroundings, what is the mass of the piece of metal in grams? Assume that water has a specific heat of 4.184 J/gºC. Enter your answer with at least 3 sig figs.