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Phoenix [80]
3 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]3 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%

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Answer:

The 12L helium tank pressurized to 160 atm will fill <em>636 </em>3-liter balloons

Explanation:

It is possible to answer this question using Boyle's law:

P_1V_1=P_2V_2

Where P₁ is the pressure of the tank (160atm), V₁ is the volume of the tank (12L), P₂ is the pressure of the balloons (1atm, atmospheric pressure) And V₂ is the volume this gas will occupy at 1 atm, thus:

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As the tank will never be empty, the volume of the gas able to fill balloons is the total volume minus 12L, thus the volume of helium able to fill balloons is:

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7 0
3 years ago
Sometimes a nuclide is referenced by the name of the element followed by the:
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Answer:

electric charge

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A nuclide is represented by the name of the element, preceded by the mass number (A) as a superscript on the left and the atomic number (Z) as subscript.

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Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor: 4 NH3 + 5 O2 → 4 NO + 6 H2O When 40.0 g NH3 and 50.0 g
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Answer:

18.75 g of NH3.

Explanation:

The balanced equation for the reaction is given below:

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Next, we shall determine the masses of NH3 and O2 that reacted from the balanced equation.

This can be obtained as follow:

Molar mass of NH3 = 14 + (3x1) = 17 g/mol

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Mass of O2 from the balanced equation = 5 x 32 = 160 g

From the balanced equation above,

68 g if NH3 reacted with 160 g of O2.

Next, we shall determine the excess reactant. This can be obtained as follow:

From the balanced equation above,

68 g if NH3 reacted with 160 g of O2.

Therefore, 40 g of NH3 will react with = (40 × 160)/68 = 94.12 g of O2.

From the calculations made above, we can see that it will take a higher amount of O2 i.e 94.12g than what was given i.e 50g to react completely with 40 g of NH3.

Therefore, O2 is the limiting reactant and NH3 is the excess reactant.

Next we shall determine the mass of excess reactant that reacted. This can be obtained as follow:

From the balanced equation above,

68 g if NH3 reacted with 160 g of O2.

Therefore, Xg of NH3 will react with 50 g of O2 i.e

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Therefore, 21.25 g of NH3 (excess reactant) were consumed in the reaction.

Finally, we shall determine mass of the remaining excess reactant as follow:

Mass of excess reactant = 40 g

Mass of excess reactant that reacted = 21.25 g

Mass of excess reactant remainig =?

Mass of excess reactant remainig = (Mass of excess reactant) – (Mass of excess reactant that reacted)

Mass of excess reactant remainig

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Therefore, the mass of excess reactant remaining is 18.75 g of NH3.

8 0
3 years ago
A gas at 127०C and 10.0 L expands to 20.0 L. What is the new temperature in Celcius? (HINT: You need to convert to Kelvins solve
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Answer:

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Based on Charles's law, the volume of a gas is directly proportional to absolute temperature. The formrula is:

V₁ / T₁ = V₂ / T₂

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Using the values of the problem:

V₁ = 10.0L

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Thus, replacing in the formula:

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3 years ago
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P2 = 1066.56 kPa.

The new pressure of the gas is 1066.56 kPa

5 0
3 years ago
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