1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
Phoenix [80]
4 years ago
13

A blood sample with a known glucose concentration of 102.0 mg/dL is used to test a new at home glucose monitor. The device is us

ed to measure the glucose concentration in the blood sample five times. The measured glucose concentrations are 96.3 , 97.2 , 104.8 , 111.5 , and 110.5 mg/dL. Calculate the absolute error and relative error for each measurement made by the glucose monitor. A. 96.3 mg/dL absolute error = mg/dL relative error = B. 97.2 mg/dL absolute error = mg/dL relative error = C. 104.8 mg/dL absolute error = mg/dL relative error = D. 111.5 mg/dL absolute error = mg/dL relative error = E. 110.5 mg/dL
Chemistry
1 answer:
Zinaida [17]4 years ago
4 0

Answer:

A. 96.3 mg/dL

Absolute error: 5.7 mg/dL

Relative error: 5.6%

B. 97.2 mg/dL

Absolute error: 4.8 mg/dL

Relative error: 4.7%

C. 104.8 mg/dL

Absolute error: 2.8 mg/dL

Relative error: 2.7%

D. 111.5 mg/dL

Absolute error: 9.5 mg/dL

Relative error: 9.3%

E. 110.5 mg/dL

Absolute error: 8.5 mg/dL

Relative error: 8.3%

Explanation:

The formula for the absolute error is:

Absolute error = |Actual Value - Measured Value|

The formula for the relative error is:

Relative error = |Absolute error/Actual value|

In your exercise, we have that

Actual Value = 102.0 mg/dL

A. 96.3 mg/dL:

E_{ABS} = |102.0 - 96.3| = 5.7mg/dL

E_{R} = \frac{5.7}{102} = 0.056 = 5.6%

B. 97.2 mg/dL

E_{ABS} = |102.0 - 97.2| = 4.8mg/dL

E_{R} = \frac{4.8}{102} = 0.047 = 4.7%

C. 104.8 mg/dL

E_{ABS} = |102.0 - 104.8| = 2.8mg/dL

E_{R} = \frac{2.8}{102} = 0.027 = 2.7%

D. 111.5 mg/dL

E_{ABS} = |102.0 - 111.5| = 9.5mg/dL

E_{R} = \frac{9.5}{102} = 0.093 = 9.3%

E. 110.5 mg/dL

E_{ABS} = |102.0 - 111.5| = 8.5mg/dL

E_{R} = \frac{8.5}{102} = 0.083 = 8.3%

You might be interested in
What type of soils are more likely to transmit contaminants
Sindrei [870]

Answer:

Chemicals can attach more easily to soils with a higher content of clay and organic matter. In addition, sandy soils generally do not contain a large amount of soil organisms compared with other soil types.

Explanation:

4 0
3 years ago
Read 2 more answers
What amounts to use in sulfur foods?​
coldgirl [10]

Answer:

Allium vegetables. Even if you haven't heard the term “allium” before, you're probably a lot more familiar with these vegetables than you think!

Explanation:

3 0
4 years ago
Read 2 more answers
How do the functions of the two groups of peripheral nerves differ?
gizmo_the_mogwai [7]

Answer:

One moves the arm one moves the legs???

Explanation:

8 0
3 years ago
Read 2 more answers
EXTRA POINTSSS 1. A solution at 25 degrees Celsius is 1.0 × 10–5 M H3O+. What is the concentration of OH– in this solution?
AlekseyPX

Answer:

Concentration of OH⁻:

1.0 × 10⁻⁹ M.

Explanation:

The following equilibrium goes on in aqueous solutions:

\text{H}_2\text{O}\;(l)\rightleftharpoons \text{H}^{+}\;(aq) + \text{OH}^{-}\;(aq).

The equilibrium constant for this reaction is called the self-ionization constant of water:

K_w = [\text{H}^{+}]\cdot[\text{OH}^{-}].

Note that water isn't part of this constant.

The value of K_w at 25 °C is 10^{-14}. How to memorize this value?

  • The pH of pure water at 25 °C is 7.
  • [\text{H}^{+}] = 10^{-\text{pH}} = 10^{-7}\;\text{mol}\cdot\text{dm}^{-3}
  • However, [\text{OH}^{-}] = [\text{H}^{+}]=10^{-7}\;\text{mol}\cdot\text{dm}^{-3} for pure water.
  • As a result, K_w = [\text{H}^{+}] \cdot[\text{OH}^{-}] = (10^{-7})^{2} = 10^{-14} at 25 °C.

Back to this question. [\text{H}^{+}] is given. 25 °C implies that K_w = 10^{-14}. As a result,

\displaystyle [\text{OH}^{-}] = \frac{K_w}{[\text{H}^{+}]} = \frac{10^{-14}}{1.0\times 10^{-5}} = 10^{-9} \;\text{mol}\cdot\text{dm}^{-3}.

8 0
3 years ago
How much heat (in kj) is released when 3.600 mol naoh(s) is dissolved in water? (the molar heat of solution of naoh is â445.1 kj
Fantom [35]
<span>-1602 kj

Sauce:me

Your welcome
</span>
8 0
3 years ago
Read 2 more answers
Other questions:
  • Can ocean currents be caused by differences in water temperature
    15·1 answer
  • Równania reakcji chemicznej
    13·1 answer
  • Magnesium has 2 valence electrons, and oxygen has 6 valence electrons. Which type of bonding is likely to occur between a magnes
    8·2 answers
  • Which is true about an invading species?
    9·2 answers
  • If two animals can reproduce and produce fertile offspring, then they are members of the same ________________.
    5·2 answers
  • Which of the following statements are true regarding the effect of flame temperature on atomic absorbance and atomic emission sp
    12·1 answer
  • Ammonia, NH3, is used as a refrigerant. At its boiling point of –33 oC, the standard enthalpy of vaporization of ammonia is 23.3
    12·1 answer
  • Question: Looking at the above visual of "Atmospheres of the Solar System" What are two patterns
    11·2 answers
  • 3. How are the protons held in the
    9·1 answer
  • 1.-Una solución de 1600 ml contiene 9,5 gramos de agua oxigenada H2O2 Calcular el porcentaje peso volumen del soluto.
    5·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!