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Brums [2.3K]
3 years ago
15

Indicate which of the following are exact numbers. (Select all that apply.) 1.the number of microseconds in a week 2.the number

of inches in a mile 3.the mass of a paper clip 4.the number of pages in a book 5.the surface area of a dime 6.the number of ounces in a pound
Chemistry
1 answer:
iVinArrow [24]3 years ago
5 0

Exact numbers need not be measured. They can be counted. Conversion factors and countable units come under exact numbers. Measured quantities are measured using a device.

1) Number of microseconds in a week -Exact as it need not be measured. It can be estimated using the conversion factors between microseconds, seconds, minutes, hours, days and week.

2) Number of inches in a mile - Exact number as it is an established conversion factor.

3) The mass of a paper clip - Measured number as it has to measured using a weighing balance.

4) The number of pages in a book - Exact number as it is not measured. It can be counted.

5) Surface area of the dime-Measured number as it has to be measured.

6) The number of ounces in a pound-Exact number as it is a constant value.

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What is extrapolation?
bixtya [17]

Answer:

A. Predicting data that fall beyond a known data point

Explanation:

Extrapolating is unreliable because you are predicting data outside of the data range - anything could happen for the data to stop following the trend or pattern

8 0
3 years ago
What is the density of an unknown object that<br> has a volume of 4cm. and a mass of 10g.
Dmitry [639]
The density would be 2.5g/cm^3
5 0
3 years ago
If you need to measure the volume of liquid in a bottle of eyedrops, what unit would be the most practical?
nexus9112 [7]
The most practical would be milliliters
4 0
3 years ago
Read 2 more answers
Various members of a class of compounds, alkenes, react with hydrogen to produce a corresponding alkane. Termed hydrogenation, t
Vitek1552 [10]

<u>Answer:</u> The mass of decane produced is 1.743\times 10^2g

<u>Explanation:</u>

To calculate the number of moles, we use the equation:  

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}       ......(1)

Mass of hydrogen gas = 2.45 g

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1:, we get:

\text{Moles of }H_2=\frac{2.45g}{2g/mol}=1.225mol

The chemical equation for the hydrogenation of decene follows:

C_{10}H_{20}(l)+H_2(g)\rightarrow C_{10}H_{22}(s)

As, decene is present in excess. So, it is considered as an excess reagent.

Thus, hydrogen gas is a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of hydrogen gas produces 1 mole of decane.

So, 1.225 moles of hydrogen gas will produce = \frac{1}{1}\times 1.225=1.225mol of decane

Now, calculating the mass of decane by using equation 1, we get:

Moles of decane = 1.225 mol

Molar mass of decane = 142.30 g/mol

Putting values in equation 1, we get:

1.225mol=\frac{\text{Mass of decane}}{142.30g/mol}\\\\\text{Mass of carbon dioxide}=(1.225mol\times 142.30g/mol)=174.3g=1.743\times 10^2g

Hence, the mass of decane produced is 1.743\times 10^2g

5 0
3 years ago
At 25.0°c, a solution has a concentration of 3.179 m and a density of 1.260 g/ml. the density of the solution at 50.0°c is 1.249
oksano4ka [1.4K]

Answer: -

3.151 M

Explanation: -

Let the volume of the solution be 1000 mL.

At 25.0 °C, Density = 1.260 g/ mL

Mass of the solution = Density x volume

= 1.260 g / mL x 1000 mL

= 1260 g

At 25.0 °C, the molarity = 3.179 M

Number of moles present per 1000 mL = 3.179 mol

Strength of the solution in g / mol

= 1260 g / 3.179 mol = 396.35 g / mol (at 25.0 °C)

Now at 50.0 °C

The density is 1.249 g/ mL

Mass of the solution = density x volume = 1.249 g / mL x 1000 mL

= 1249 g.

Number of moles present in 1249 g = Mass of the solution / Strength in g /mol

= \frac{1249 g}{396.35 g/mol}

= 3.151 moles.

So 3.151 moles is present in 1000 mL at 50.0 °C

Molarity at 50.0 °C = 3.151 M

7 0
3 years ago
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