| 1.dThe true mass m can be calculated from the observed mass, m’.d1-adM= m'Where:d, is the density of air (0.001 2 g/mL at 1 bar and 25°C)dwis the density of the calibration weights (8.0 g/mL)d, is the density of the object being weighed.Wd..1-dowhere do = 0.001782 g/mL at 25°C for CO2%3Dapparent mass =true mass%3D (Correction) You mixed 2.450g CaC2O4 with 0.750g KMNO4 in excess aqueous acid. What apparent mass and true mass of CO2 will the resulting reaction yield?note of the following information:• Use the mass of CO2 you calculate above as the apparent mass. No need to convert the masses of CaC204 and KMNO4 into true masses first.• The unbalanced chemical equation of the redox reaction is as follows:C2042- + MnO4" + H* → CO2 + Mn²+ + H2OThe pertinent formula masses are as follows:ReagentFormula Mass (g/mol)CaC204128.097KMNO4158.03CO244.0095• The formula for the true mass is as follows:

Given reaction of CaC2O4 with KMnO4: C2O42- + MnO4- + H+ → CO2 + Mn2+ + H2O

The true mass m can be calculated from the observed mass, m'. d. 1- d, m = m' d a Where: da is the density of air (0.001 2 g/mL at 1 bar and 25°C) dwis the density of the calibration weights (8.0 g/mL) d, is the density of the object being weighed. W a 1- do where do = 0.001782 g/mL at 25°C for CO2 apparent mass = --- 8 true mass = ---

The true mass m can be calculated from the observed mass, m'. d. 1- d, m = m' d a Where: da is the density of air (0.001 2 g/mL at 1 bar and 25°C) dwis the density of the calibration weights (8.0 g/mL) d, is the density of the object being weighed. W a 1- do where do = 0.001782 g/mL at 25°C for CO2 apparent mass = --- 8 true mass = ---

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...

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Question

| 1.d
The true mass m can be calculated from the observed mass, m’.
d
1-
a
d
M= m'
Where:
d, is the density of air (0.001 2 g/mL at 1 bar and 25°C)
dwis the density of the calibration weights (8.0 g/mL)
d, is the density of the object being weighed.
W
d.
.
1-
do
where do = 0.001782 g/mL at 25°C for CO2
%3D
apparent mass =
true mass
%3D

(Correction) You mixed 2.450g CaC2O4 with 0.750g KMNO4 in excess aqueous acid. What apparent mass and true mass of CO2 will the resulting reaction yield?
note of the following information:
• Use the mass of CO2 you calculate above as the apparent mass. No need to convert the masses of CaC204 and KMNO4 into true masses first.
• The unbalanced chemical equation of the redox reaction is as follows:
C2042- + MnO4" + H* → CO2 + Mn²+ + H2O
The pertinent formula masses are as follows:
Reagent
Formula Mass (g/mol)
CaC204
128.097
KMNO4
158.03
CO2
44.0095
• The formula for the true mass is as follows:

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