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scoundrel [369]
3 years ago
9

What would you expect to observe when you add flour to a glass of water?

Chemistry
2 answers:
Shtirlitz [24]3 years ago
6 0
It would look cloudy at the bottom or float up top srry if wrong
algol [13]3 years ago
4 0

Answer:

hmmm

Explanation:

hmmmmmmmmmmmmmmmmmmmmmmmmmmmmmmmmmmmmm

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Ostrovityanka [42]
I would say the answer is C
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What happens when an electron jumps energy from energy level 3 energy level 6 in an atom
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Explanation:

high energy to Low energy

=the electron gains energy (K.E)

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A teardrop-shaped hill that points the direction a glacier has flowed is a:
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The answer is A Drumlin

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3 years ago
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If the density of an object is 5 g/cm3 and it takes up 7 cm3 of space, calculate the mass?
statuscvo [17]

Answer:

<h2>The answer is option A</h2>

Explanation:

The mass of a substance when given the density and volume can be found by using the formula

<h3>mass = Density × volume</h3>

From the question

volume of object = 7 cm³

density = 5 g/cm³

The mass of the object is

mass = 5 × 7

We have the final answer as

<h2>35 g</h2>

Hope this helps you

8 0
3 years ago
The theoretical yield of Cl2 from certain starting amounts of MnO2 and HCl was calculated as 60.25 g and 65.02 g, respectively.
user100 [1]

Answer:

c    43.38 g

Explanation:

The reaction  between MnO2 and HCl can be represented by the following balanced equation:

MnO2 + HCl ---> Cl2 + MnCl2 + H2O

From the balanced equation, the theoretically required molar ratio of MnO2 to HCl is 1:1, therefore the yields would have been expected to be equal.  

For the fact that HCl  gives a higher yield (65.02g) than MnO2 (60.25g) according to the problem statement, HCl should be in excess,  while the limiting reagent should be MnO2 .  

Thus, the theoretical yield of Cl2 will be  60.25 g.

By definition, the percentage yield is given by

% Yield = (Actual Yield) / (Theoretical Yield),  

This can be simplified to

Actual Yield = % Yield * Theoretical Yield

Plugging in the given values we have

Actual Yield = 72% *  60.25 = 43.38 g

5 0
3 years ago
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