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3 years ago

6

Your blood contains many dissolved solids. What do you think could be done if you needed to remove the water from a sample of bl

ood in order to study the solids that remained?

1 answer:

s2008m [1.1K]3 years ago

8 0

Answer:

could the answer be boil the water away?

Explanation:

if the water gets boiled and evaporates, than you are left with the solids

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If a helium filled ballon has a volume of 3.4l at 25°c and 1.18atm., what is its volume at STP?

vladimir2022 [97]

Answer:

3.711 L

Explanation:

The formula you need to use is the following:

$\frac{V_{1}}{T_{1}} = \frac{V_{2}}{T_{2}}\\$

3.4L / 298 K = V2 / 273 K

V2 = 3.711 L

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3 years ago

MULTIPLE CHOICE

Flauer [41]

Answer:

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How many neutrons are found in a stable isotope of uranium-235?

bezimeni [28]

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3 years ago

What is the molarity of a solution made by adding 0.720 mole of NaOH to 2.40 liters of water

WITCHER [35]

Answer:

Molarity = 0.3 M

Explanation:

Given data:

Moles of NaOH = 0.720 mol

Volume of water = 2.40 L

Molarity = ?

Solution:

Molarity is used to describe the concentration of solution. It tells how many moles are dissolve in per litter of solution.

Formula:

Molarity = number of moles of solute / L of solution

Molarity = 0.720 mol / 2.40 L

Molarity = 0.3 mol/L

Molarity = 0.3 M

7 0

3 years ago

A 2.40 kg block of ice is heated with 5820 J of heat. The specific heat of water is 4.18 J•g^-1•C^-1. By how much will it’s temp

MrMuchimi

Answer: The temperature rise is $0.53^0C$

Explanation:

The quantity of heat required to raise the temperature of a substance by one degree Celsius is called the specific heat capacity.

$Q=m\times c\times \Delta T$

Q = Heat absorbed by ice = 5280 J

m = mass of ice = 2.40 kg = 2400 g (1kg=1000g)

c = heat capacity of water = $4.18J/g^0C$

Initial temperature = $T_i$

Final temperature = $T_f$

Change in temperature , $\Delta T=T_f-T_i=?$

Putting in the values, we get:

$5280J=2400g\times 4.18J/g^0C\times \Delta T$

$\Delta T=0.53^0C$

Thus the temperature rise is $0.53^0C$

0 0

3 years ago