Constants Periodic Table A calorimeter is an insulated device in which a chemical reaction is contained. By measuring the temperature change, AT, we can calculate the heat released or absorbed during the reaction using the following equation: Part A q= specific heat x mass x AT A calorimeter contains 30.0 mL of water at 14.0 °C. When 1.70 g of X (a substance with a molar mass of 76.0 g/mol) is added, it dissolves via the reaction Or, if the calorimeter has a predetermined heat capacity, C, the equation becomes X(s) + H2O(1)-X(aq) q= Cx AT and the temperature of the solution increases to 30.0 °C At constant pressure, the enthalpy change for the Calculate the enthalpy change, AH for this reaction per mole of X. reaction, AH, is equal to the heat, qp; that is, H = qp Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g- C))., that density of water is 1.00g/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings. Express the change in enthalpy in kilojoules per mole to three significant figures. but it is usually expressed per mole of reactant and with a sign opposite to that of q for the surroundings. The total internal energy change, AE (sometimes referred to as AU), is the sum of heat, q, and work done, w: > View Available Hint(s) ? AE = q+ uw However, at constant volume (as with a bomb calorimeter) uw = 0 and so AE = qu ΔΗ- kJ/mol Submit P Pearson Privary Polo Permissions Contact Us stry.com/myct/itemView?assignmentProblemID=174388853 1 Pearson Education Inc All rights resenved Terms of Use Vi 1:07
Constants Periodic Table A calorimeter is an insulated device in which a chemical reaction is contained. By measuring the temperature change, AT, we can calculate the heat released or absorbed during the reaction using the following equation: Part A q= specific heat x mass x AT A calorimeter contains 30.0 mL of water at 14.0 °C. When 1.70 g of X (a substance with a molar mass of 76.0 g/mol) is added, it dissolves via the reaction Or, if the calorimeter has a predetermined heat capacity, C, the equation becomes X(s) + H2O(1)-X(aq) q= Cx AT and the temperature of the solution increases to 30.0 °C At constant pressure, the enthalpy change for the Calculate the enthalpy change, AH for this reaction per mole of X. reaction, AH, is equal to the heat, qp; that is, H = qp Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g- C))., that density of water is 1.00g/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings. Express the change in enthalpy in kilojoules per mole to three significant figures. but it is usually expressed per mole of reactant and with a sign opposite to that of q for the surroundings. The total internal energy change, AE (sometimes referred to as AU), is the sum of heat, q, and work done, w: > View Available Hint(s) ? AE = q+ uw However, at constant volume (as with a bomb calorimeter) uw = 0 and so AE = qu ΔΗ- kJ/mol Submit P Pearson Privary Polo Permissions Contact Us stry.com/myct/itemView?assignmentProblemID=174388853 1 Pearson Education Inc All rights resenved Terms of Use Vi 1:07
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter9: Energy And Chemistry
Section: Chapter Questions
Problem 9.101PAE
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Transcribed Image Text:Constants Periodic Table
A calorimeter is an insulated device in which a
chemical reaction is contained. By measuring the
temperature change, AT, we can calculate the
heat released or absorbed during the reaction using
the following equation:
Part A
q= specific heat x mass x AT
A calorimeter contains 30,0 mL of water at 14.0 °C. When 1.70 g of X (a substance with a molar mass of
76.0 g/mol) is added, it dissolves via the reaction
Or, if the calorimeter has a predetermined heat
capacity, C, the equation becomes
X(s) + H2O(1)→X(aq)
q = C x AT
and the temperature of the solution increases to 30.0 °C
At constant pressure, the enthalpy change for the
reaction, AH, is equal to the heat, qp, that is,
Calculate the enthalpy change, AH, for this reaction per mole of X.
Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g- C)), that density
of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings.
= qp
Express the change in enthalpy in kilojoules per mole to three significant figures.
but it is usually expressed per mole of reactant and
with a sign opposite to that of q for the
surroundings. The total internal energy change,
AE (sometimes referred to as AU), is the sum of
heat, q, and work done, uw:
> View Available Hint(s)
V A2O
AE= q+ w
However, at constant volume (as with a bomb
calorimeter) w = 0 and so AE = q.
ΔΗ
kJ/mol
Submit
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Transcribed Image Text:Constants | Periodic Table
calorimeter is an insulated device in which a
emical reaction is contained. By measuring the
mperature change, AT, we can calculate the
at released or absorbed during the reaction using
e following equation:
Part B
Consider the reaction
q= specific heat x mass x AT
C12 H22O11 (s) + 1202 (g)-12CO2 (g) + 11H20(1)
if the calorimeter has a predetermined heat
pacity, C, the equation becomes
in which 10.0 g of sucrose, C12 H22011, was burned in a bomb calorimeter with a heat capacity of 7.50
kJ/ C. The temperature increase inside the calorimeter was found to be 22.0 °C. Calculate the change in
internal energy, AE, for this reaction per mole of sucrose.
ECx AT
E constant pressure, the enthalpy change for the
action, AH, is equal to the heat, qp. that is,
Express the change in internal energy in kilojoules per mole to three significant figures.
> View Available Hint(s)
AH= 9p
ut it is usually expressed per mole of reactant and
ith a sign opposite to that of q for the
urroundings. The total internal energy change,
AE (sometimes referred to as AU), is the sum of
eat, q, and work done, w:
Πνα ΑΣφ
AE =
kJ/mol
AE = q+ w
Submit
However, at constant volume (as with a bomb
calorimeter) w=0 and so AE= qr-
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