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2 years ago

Convert a pressure of 0.0248 mm Hg to the equivalent pressure in pascals (Pa). How did you get your answer ?

Chemistry

1 answer:

Rudik [331]2 years ago

5 0

Hope this helps :) remember your conversions and just practice it's fairly easy:)

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13.36

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use this formula for that:

moles = gram/molar mass

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2 years ago

C) Convert 649 kPa to atm.

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3 years ago

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Which statement is true about endothermic and exothermic reactions

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2 years ago

S2 + C ----> CS2How many grams of CS2 can be prepared by heating 11.0 moles of S2 with excess carbon in 5.20 L reaction vesse

pantera1 [17]

Answer : The mass of $CS_2$ prepared can be, 754.832 grams

Explanation : Given,

Initial moles of $S_2$ = 11.0 mole

Volume of solution = 5.2 L

Equilibrium constant $(K_c)$ = 9.40

First we have to calculate the concentration of $S_2$ .

$\text{Concentration of }S_2=\frac{\text{Moles of }S_2}{\text{Volume of solution}}=\frac{11.0mole}{5.20L}=2.115M$

The balanced equilibrium reaction will be,

$S_2(g)+C(s)\rightleftharpoons CS_2(g)$

Initial moles 2.115 0

At eqm. (2.115-x) x

The equilibrium expression for this reaction will be,

$K_c=\frac{[CS_2]}{[S_2]}$

Now put all the given values in this expression, we get:

$9.40=\frac{(x)}{(2.115-x)}$

$x=1.91M$

The concentration of $CS_2$ = x = 1.91 M

Now we have to calculate the moles moles of $CS_2$ .

Formula used : $Concentration=\frac{Moles}{Volume}$

$\text{Concentration of }CS_2=\frac{\text{Moles of }CS_2}{\text{Volume of solution}}$

$1.91M=\frac{\text{Moles of }CS_2}{5.20L}$

$\text{Moles of }CS_2=9.932mole$

Now we have to calculate the mass of $CS_2$ .

$\text{Mass of }CS_2=\text{Moles of }CS_2\times \text{Molar mass of }CS_2$

$\text{Mass of }CS_2=9.932mole\times 76g/mole=754.832g$

Therefore, the mass of $CS_2$ prepared can be, 754.832 grams

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2 years ago