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3 years ago

Please help me dont just use me for points

Chemistry

1 answer:

JulijaS [17]3 years ago

4 0

Answer:

It's B

Explanation:

A is going to evaporate more quickly causing it to push through the tube to beaker B.

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Which element of weather is caused by a difference in air pressure between two air masses?

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Wind results due to difference in air pressure of air masses. Due to difference in pressure of two air masses, low pressure zone is created by lifting of one the air mass above the other as the movement of air takes place from higher pressure area to lower pressure area. This causes different wind speed in different areas. The direction of wind depends on its origin for example, a northerly wind always moves from north to south direction.

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3 years ago

Read 2 more answers

Balance the following equation:

Firdavs [7]

Answer: a) $2K_2CrO_4+3Na_2SO_3+10HCl\rightarrow 4KCl+3Na_2SO_4+2CrCl_3+5H_2O$

b) 1 mole of $SO_2$ is produced.

Explanation:

According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

The skeletal equation is:

$K_2CrO_4+Na_2SO_3+HCl\rightarrow KCl+Na_2SO_4+CrCl_3 +H_2O$

The balanced equation will be:

$2K_2CrO_4+3Na_2SO_3+10HCl\rightarrow 4KCl+3Na_2SO_4+2CrCl_3+5H_2O$

Thus the coefficients are 2, 3 , 10 , 4 , 3 , 2 and 5.

b) Oxidation: $2I-^-\rightarrow I_2+2e-^-$

Reduction: $SO_4^{2-}+2e^-+4H^+\rightarrow SO_2+2H_2O$

Net reaction: $2I-^-+SO_4^{2-}+4H^+\rightarrow I_2+SO_2+2H_2O$

When 1 mole of $I_2$ is produced, 1 mole of $SO_2$ is produced.

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4 years ago

By what factor does the rate change in each of the following cases (assuming constant temperature)? (a) A reaction is first orde

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Answer:

a) 2

b) 1/4

c) 9

Explanation:

a) for a first order reaction in reactant A

r initial = k*[A initial]

then if the concentration is doubled [A final ]= 2*[A initial] , then

r final = k*[A final ] = 2* k*[A initial] = 2*r initial

then the velocity changes by a factor of 2

b) for a second order reaction in reactant B

r initial = k*[B initial]²

then if the concentration is halved: [B final ]= [B initial]/2 , then

r final = k*[B final ]² = k*( [B initial]/2 )² =k* [B initial]² /4 = r initial /4

then the velocity changes by a factor of 1/4

c) for a second order reaction in reactant C

r initial = k*[C initial]²

then if the concentration is tripled : [C final ]= 3* [C initial] , then

r final = k*[C final ]² = k*( 3*[C initial] )² =k* [C initial]² *9 = 9 * r initial

then the velocity changes by a factor of 9

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