1. How much heat must be added to a 38-g sample of aluminum to increase itstemperature by 250.0°C? The specific heat capacity for aluminum is 0.902 J/g °C.62. A solid substance has a mass of 250 grams. It is cooled by 25.00°C and loses4.937 kJ of heat. What is the specific heat capacity of the substance?3. A 10.0 g sample of pure acetic acid, CH3CO2H, is completely burned. The heatreleased warms 2.0 L of water from 22.3°C to 39.6°C.a) Assuming that no heat was lost to the calorimeter, what is the molar enthalpychange of the complete combustion of acetic acid? Express your answer inkJ/mol.b) Will the bonds in the products be longer or shorter than the bonds in thereactants?7

Dear student since you have posted multiple questions, As per BARTLEBY QnA guidelines we are allowed…

Answered: 1. How much heat must be added to a…

1. How much heat must be added to a 38-g sample of aluminum to increase its temperature by 250.0°C? The specific heat capacity for aluminum is 0.902 J/g °C.

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

A 93.82 g bar of iron was heated to 98.4 °C and then dropped into 38.1 mL of water at 15.3 °C. The temperature of the water increased to a maximum of 32.7 °C. Calculate the specific heat capacity of iron. Assume that the density of water is 1.00 g/mL. heat capacity (J/g°C)
The specific heat of a substance is the amount of heat required to raise the temperature of one gram of the substance by one degree Celsius. The relationship between the amount of heat gained or released by a substance and the change in temperature of the substance is given by the equation ?=??Δ?q=m⁢s⁢Δ⁢T where ?q is the heat gained or released, ?m is the mass of the substance, ?s is the specific heat of the substance, and Δ?Δ⁢T is the change in temperature. 1. Rearrange the equation to solve for ?. 2. When a substance with a specific heat of 0.635 J/g⋅∘C0.635 J/g⋅∘C is heated from 25.2 ∘C25.2⁢ ∘C to 71.4 ∘C,71.4⁢ ∘C, it absorbs 422 J422 J of heat. Calculate the mass of the substance.
A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with 22.4 mL of 6.45 M hydrochloric acid. The temperature of the mixture rises 17.2 ° C. The density of the resulting solution is 1.00 g mL and has a specific heat capacity of 4.184 J g · ° C . The heat capacity of the calorimeter is 16.97 J ° C . Part 1: (a) Identify the limiting reagent for the reaction. Part 2: (b) Calculate the heat of reaction (in J). qrxn = × 10 JEnter your answer in scientific notation. Part 3 out of 3 (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization = ____ kj/mol
The temperature of an object increases by 44.1 °C when it absorbs 3761 J of heat. The mass of the object is 355 g. Calculate the heat capacity of the object.
22.9 mL of an unknown acid was neutralized by mixing it with 50.3 mL of NaOH in an aqueous solution. The final temperature of the solution was 35.2 °C. The initial temperature of the acid and base was 22.0 °C. Assuming that the density of the solution is 1.00 g/mL and the specific heat is 4.184 J/g°C, what is the heat of neutralization reaction?
A chemist dissolved an 10.8-g sample of KOH in 100.0 grams of water in a coffee cup calorimeter. When she did so, the water temperature increased by 23.9°C. Based on this, how much heat energy was required to dissolve the sample of KOH? Assume the specific heat of the solution is 4.184 J/g - °C. %3D =Db Calculate the heat of solution for KOH in kJ/mol. kJ/mol heat of solution =
For the highly exothermic reaction H2(g) + 1/2 O2(g) → H2O(g) qrx =DHrx = -242 kJ, What quantity of heat (kJ) is exchanged when 17.9 moles of hydrogen and 1.13 moles of oxygen are combusted?
4. The specific heat of water is quite high at 4.184 J/gC. Explain how life on this planet would be different if the specific heat of water were that of lead at 0.128 J/gC.
A sample of copper was heated to 120o C and then plunged into an insulated vessel containing 200.g of water at 25.00o C. The final temperature of the mixture was 26.50o C. Assuming no heat was lost to the surroundings, calculate the mass of the copper sample. The specific heat of copper is 0.385 J/go C and the specific heat of water is 4.184 J/go C.
A 837837 g copper pan is removed from the stove at a temperature of 150 °C. It is then stacked on top of a 787787 g aluminum sheet at room temperature, 25 °C. The specific heat capacity for copper is 0.387 Jg·KJg·K and that for aluminum is 0.904 Jg·KJg·K. Assume no heat is gained or lost to the surroundings. What is the final temperature (?fTf) of the two objects after thermal equilibrium is reached?
A sample of copper with a specific heat of 0.385 J goC is heated from 45.6 oC to 80.7 oC. What is the mass of the copper sample if this process required 816.24 J of energy?
If 1495 J of heat is needed to raise the temperature of a 327 g sample of a metal from 55.0°C to 66.0°C, what is the specific heat capacity of the metal?