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3 years ago

Here is a pic of me I'm ugly i dont have all my pics of me anymore lost it all

Chemistry

2 answers:

Hunter-Best [27]3 years ago

6 0

ur hair is pretty tho

Elden [556K]3 years ago

3 0

Answer:

u looking so beautiful

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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

Zinaida [17]

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

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

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

4 0

3 years ago

1 what do you understand by the term isotopes 2 why do I should talk of an element process identical chemical properties 3 name

Bad White [126]

Answer:

Isotopes of an element have same number of protons but different number of neutrons. Which means isotopes of an element have same atomic number but different mass number.

The chemical property of an element is determined by the number of electrons. And as all the isotopes have same number of electrons, they have same chemical properties.

Thus as isotopes of an element have same atomic number , they have same number of electrons and protons. As they have different mass number, the number of neutrons will be different. Hydrogen has three isotopes , $^1_1\textrm{H}$ , $^2_1\textrm{H}$ and $^3_1\textrm{H}$ . Thus $^1_1\textrm{H}$ has no neutron.

5 0

3 years ago

What is the pH of 1.00 L of a buffer that is 0.110 M nitrous acid (HNO2) and 0.200 M NaNO2? (pKa of HNO2 = 3.40)

Andrei [34K]

Answer:

pH = 3.65

Explanation:

given data

pKa of HNO2 = 3.40

nitrous acid (HNO2) = 0.110 M

NaNO2 = 0.200 M

to find out

What is the pH

solution

we get here ph for acidic buffer that is express as

pH = pKa + log(salt÷acid) ........................1

put here value and we get

pH = 3.40 + log(0.200÷0.110)

pH = 3.65

4 0

3 years ago

The atomic mass of hydrogen-1 is 1.008 and the atomic mass of helium-4 is 4.003. Find the difference in grams between 4 moles of

CaHeK987 [17]

4 moles of hydrogen = 4 * 1.008 = 4.032 grams

1 mole of helium = 4.003 grams

Difference is 4.032 - 4.003

= 0.029 g

7 0

3 years ago

Read 2 more answers

Combustion analysis of 0.300 g of an unknown compound containing carbon, hydrogen, and oxygen produced 0.5213 g of co2 and 0.283

Lyrx [107]

First, we have to get how many grams of C & H & O in the compound:
- the mass of C on CO2 = mass of CO2*molar mass of C /molar mass of CO2
= 0.5213 * 12 / 44 = 0.142 g
- the mass of H atom on H2O = mass of H2O*molar mass of H / molar mass of H2O
=0.2835 * 2 / 18 = 0.0315 g
- the mass of O = the total mass - the mass of C atom - the mass of H atom
= 0.3 - 0.142 - 0.0315 = 0.1265 g
Convert the mass to mole by divided by molar mass
C(0.142/12) H(0.0315/2) O(0.1265/16)
C(0.0118) H(0.01575) O(0.0079) by dividing by the smallest value 0.0079
C1.504 H3.99 O1 by rounding to the nearst fraction
C3/2 H4/1 )1/1 multiply by 2
∴ the emprical formula C3H8O2

6 0

3 years ago