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Virty [35]
3 years ago
7

What is the correct way to write 0.0000250 m in scientific notation?

Chemistry
2 answers:
yulyashka [42]3 years ago
7 0
Scientific notation is: n * 10^a, where n is a number between 1 and 10 ( but not 10 itself ) and a is an integer.
We move decimal place to the left to create a new number from 1 to 10.
Answer:
0.0000250 m = 2.5 * 10^(-5) m.
Ivenika [448]3 years ago
3 0

Answer: The correct way to write 0.0000250 m in scientific notation is 0.0000250 m=2.50\times 10^{-5} m

Explanation

The scientific notation is way to represent a very large or very small  number in a convenient way.

For numbers without decimal:

It is written by shifting the decimal point to the left until single digit before decimal point is reached and multiplying with number '10' raised to the power equal to number of times decimal point shifted towards left.

For example:  Number '2345 ' is written in scientific notation as 2.345\times 10^{3}.

For numbers with decimal:

It is written by shifting the decimal point to the right until single digit before decimal point is reached and multiplying with number '10' raised to the power equal to number of times decimal point shifted towards right with negative sign.For example:  Number '0.003045 ' is written in scientific notation as 3.045\times 10^{-3}.

So, the correct way to write 0.0000250 m in scientific notation:

0.0000250 m=2.50\times 10^{-5} m

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In a titration of 0.5 M HCl and an unknown concentration NaOH, 25.0 ml of NaOH was required to completely neutralize 25.0 ml of
baherus [9]
When an acid is neutralized by a base, that means moles of H+ = moles of OH-

moles of H+ = 0.5 M * 0.025 L HCl = 0.0125 moles H+

moles of OH- should be equal to 0.0125 moles, so
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3 years ago
PLEASE HELP ASAP WILL GIVE BRAINLIEST
kirill115 [55]

The amount of heat required to convert H₂O to steam is :  382.62 kJ

<u>Given data :</u>

Mass of liquid water  ( m ) = 150 g

Temperature of liquid water = 43.5°C

Temperature of steam = 130°C

<h3 /><h3>Determine the amount of heat required </h3>

The amount of heat required = ∑ q1 + q2 + q3 ----- ( 1 )

where ;

q1 = heat required to change Temperature of water from 43.5°C to 100°C .  q2 = heat required to change liquid water at 100°C to steam at 100°C

q3 = heat required to change temperature of steam at 100°C to 130°C

  • For q1

M* S_{water}*ΔT

= 150 * 4.18 * ( 100 - 43.5 )

= 35425.5 J

  • For q2

moles * ΔHvap

= (150 / 18 )* 40.67 * 1000

=  338916.67 J

  • For q3

M * S_{steam} * ΔT

= 150 * 1.84 * ( 130 -100 )

= 8280 J

Back to equation ( 1 )

Amount of heat required = 35425.5  + 338916.67 + 8280 = 382622.17 J

                                                                                               ≈ 382.62 kJ

Hence we can conclude that The amount of heat required to convert H₂O to steam is :  382.62 kJ.

Learn more about Specific heat of water : brainly.com/question/16559442

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