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CHEM 103 Module 3 Exam Portage Learning Questions and Verified Answers,100% Guaranteed Pas, Exams of Nursing

University of PikevilleNursing

CHEM 103 Module 3 Exam Portage Learning Questions and Verified Answers,100% Guaranteed Pass This document contains all the verified questions and answers for Module 3 of CHEM 103 from Portage Learning. It covers fundamental topics such as chemical reactions, balancing equations, stoichiometry, limiting reactants, and percent yield. The content is designed to help students understand core concepts and succeed in their module exam with confidence.

Typology: Exams

2024/2025

Available from 05/23/2025

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Question 1
CHEM 103 Module 3 Exam Portage Learning
Questions and Verified Answers,100% Guaranteed Pass
CHEM 103
MODULE: 3 2025/2026
Click this link to access the
Periodic Table.
This may be helpful throughout the
exam.
A reaction between HCl and NaOH is being studied in a styrofoam coffee cup
with NO lid and the heat given off is measured by means of a thermometer
immersed in the reaction mixture. Enter the correct thermochemistry term to
describe the item listed.
1.
The type of thermochemical process
2.
The amount of heat released in the reaction of HCl with NaOH
1.
Heat given off =
Exothermic
process
2.
The amount of heat released =
Heat of reaction
Question 2
Click this link to access the
Periodic Table.
This may be helpful throughout the
exam.
1.
Show the calculation of the final temperature of the mixture when a
22.8 gram sample of water at 74.6
o
C is added to a 14.3 gram sample of water at
24.3
o
C in a coffee cup calorimeter.
pf3
pf4
pf5
pf8
pf9
pfa

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Question 1

CHEM 103 Module 3 Exam Portage Learning

Questions and Verified Answers,100% Guaranteed Pass

CHEM 103 MODULE: 3 202 5/ Click this link to access the Periodic Table. This may be helpful throughout the exam. A reaction between HCl and NaOH is being studied in a styrofoam coffee cup with NO lid and the heat given off is measured by means of a thermometer immersed in the reaction mixture. Enter the correct thermochemistry term to describe the item listed.

  1. The type of thermochemical process
  2. The amount of heat released in the reaction of HCl with NaOH
  3. Heat given off = Exothermic process 2. The amount of heat released = Heat of reaction

Question 2

Click this link to access the Periodic Table. This may be helpful throughout the exam.

  1. Show the calculation of the final temperature of the mixture when a 22.8 gram sample of water at 74.6oC is added to a 14.3 gram sample of water at 24.3oC in a coffee cup calorimeter.

c (water) = 4.184 J/g oC

  1. Show the calculation of the energy involved in freezing 54.3 grams of water at 0oC if the Heat of Fusion for water is 0.334 kJ/g
    • (mwarn H2O x cwarn H2O x ∆twarn H2O) = (mcool H2O x ccool H2O x ∆tcool H2O)

exam.

f 4 f f 2 Show the calculation of the heat of reaction (ΔHrxn) for the reaction: 3 C (graphite) + 4 H 2 (g) → C 3 H 8 (g) by using the following thermochemical data: C (graphite) kJ

  • O 2 (g)^ → CO 2 (g)^ ΔH = - 393. 2 H 2 (s) kJ
  • O 2 (g) → 2 H 2 O(l) ΔH = - 571. C 3 H 8 (g) (^) + 5 O 2 (g) (^) → 3 CO 2 (g) (^) + 4 H 2 O(l) (^) ΔH = - 2220.0 kJ Your Answer: 3 (C (graphite) + O 2 (g) → CO 2 (g) ΔH = - 393.51 kJ) 2 (2 H 2 (s) + O 2 (g) → 2 H 2 O(l) ΔH =
  • 571.66 kJ) 3 CO 2 (g) + 4 H 2 O(l) → C 3 H 8 (g) + 5 O 2 (g) ΔH = + 2220.0 kJ 3 C (graphite) + 4 H 2 (g) → C 3 H 8 (g) **ΔHrxn =
  • 103.85 kJ** ΔHrxn = 3(- 393.51) + 2(- 571.66) + 2220.0 = - 103.

Question 5

Click this link to access the Periodic Table. This may be helpful throughout the exam. Show the calculation of the heat of reaction (ΔHrxn) for the reaction: 2 CH 4 (g) + 3 O 2 (g) → 2 CO (g) + 4 H 2 O (l) by using the following ΔHf^0 data: ΔH 0 CH (g) = - 74.6 kJ/mole, ΔH 0 CO (g) = - 110.5 kJ/mole, ΔH 0 H O (l) = - 285. kJ/mole 2 CH 4 (g) + 3 O 2 (g) → 2 CO (g) + 4 H 2 O (l)

ΔHrxn = 2(+74.6) + 3(0) + 2(-110.5) + 4(-285.8) = - 1215.0 kJ/mole

Question 6

Click this link to access the Periodic Table. This may be helpful throughoutthe exam. Show the calculation of the new temperature of a gas sample has an original volume of 740 ml when collected at 710 mm and 35oC when the volume becomes 460 ml at 1.20 atm. P1V1/T1 = P2V2/T T2 = 1.2 x 460x308 / 0.934 x 740 = 245.98 kelvin = - 27.17oC (Pi x Vi ) / Ti = (Pf x Vf ) / Tf 740 ml/1000 = 0.740 liters = Vi 710 mm/760 = 0.934 atm = Pi 460 ml/1000 = 0.460 liters = Vf 1.20 atm = Pf 35 oC + 273 = 308 oK = Ti (0.934) x (0.740) / 308 = (1.20) x (0.460) / Tf Tf = 246 oK

Question 7

Click this link to access the Periodic Table. This may be helpful throughout the exam.

Show the calculation of the volume occupied by a gas sample containing 0. mole collected at 710 mm and 35oC. P x V = n x R x T

mixture of 7.60 g of N 2 and 8.40 g of O 2 at 25oC. nN2 = gN2 / (MWN2) = 7.60 g / 28.02 = 0.2712 mol nO2 = gO2 / (MWO2) = 8.40 g / 32.00 = 0.2625 mol

XN2 = 0.2712 / (0.2712 + 0.2625) = 0.

XO2 = 0.2625 / (0.2712 + 0.2625) = 0.

Question 10

Click this link to access the Periodic Table. This may be helpful throughout the exam. Show the calculation of the molecular weight of an unknown gas if the rate ofeffusion of carbon dioxide gas (CO 2 ) is 1.83 times faster than that of an^ unknown gas. (rN2 /runknown)^2 = MWunknown / MWCO (1.83/1)^2 = MWunknown / 44.01 MWunknown = (1.83)^2 x 44. = 147. calculation error; minus 2.