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Amanda [17]
3 years ago
13

Pls hurry

Chemistry
1 answer:
eimsori [14]3 years ago
4 0

Answer:

plusses give me brainliest after this

The answer is: 1. periodic table

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If the hydrogen ion concentration, (H+), in a solution is 5.39 x 10-8 M,
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Explanation:

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Correct formula for tetrafluorine monoxide
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What two major Southeastern U.S. cities will be underwater if sea level<br> rose 6 feet?
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Rising sea levels would be devastating in North Somerset, with large parts of Clevedon, Weston-super-Mare and Burnham all being underwater by 2050 according to Climate Central

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3 years ago
A helium balloon has a volume of 2.5 L. When heated to 343.5K the pressure of the gas is 66.7 kPa. How many moles of He gas woul
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Answer:

0.06mole

Explanation:

Given parameters:

Volume of balloon = 2.5L

T = 343.5K

P  = 66.7kPa; in atm  gives  = 0.66atm

Unknown:

Number of moles of He  = ?

Solution:

To solve this problem, we use the ideal gas equation.

 It is mathematically expressed as;

               Pv = nRT

  where  p is the pressure

              v is the volume

               n is the number of moles

               R is the gas constant

               T is the temperature

      0.66 x 2.5  = n x 0.082 x 343.5

                      n  = 0.06mole

8 0
3 years ago
The concentration of a diluted "wine" sample was found to be 0.24 %(v/v) ethanol. Assuming the wine was diluted by 75x before an
Softa [21]

Answer:

The original concentration of ethanol was 18 % (v/v)

Explanation:

For the analysis of a sample, mostly dilutions are made of the original concentrated sample. The analysis results obtained from the diluted sample are then calculated for the concentrated samples.

According to the given data, the wine sample was diluted 75 times. This means that the initial concentration of ethanol was 75 times more than the final concentration i.e. 0.24 % (v/v). So mathematically:

original concentration (v/v)= final concentration (v/v) x times diluted

original concentration (v/v)= 0.24 % x 75

original concentration (v/v) = 18 %

3 0
3 years ago
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