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3 years ago

If we had 79.3 grams of Xe, would we expect a volume that is

Chemistry

1 answer:

Shtirlitz [24]3 years ago

6 0

Answer:

13.44 liters of Xe

Explanation:

First, change grams to moles by dividing the mass given (79.3) by the mass of one mole of Xe (131.3) to get .6 moles.

Now you turn moles to liters (aka volume) by multiplying the number of moles of Xe (.6) by 22.4 to get 13.44 liters of Xe

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3 years ago

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lbvjy [14]

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3 years ago

A gas used to extinguish fires is composed of 75 % CO2 and 25 % N2. It is stored in a 5 m3 tank at 300 kPa and 25 °C. What is th

tatyana61 [14]

Answer : The partial pressure of the $CO_2$ in the tank in psia is, 32.6 psia.

Explanation :

As we are given 75 % $CO_2$ and 25 % $N_2$ in terms of volume.

First we have to calculate the moles of $CO_2$ and $N_2$ .

$\text{Moles of }CO_2=\frac{\text{Volume of }CO_2}{\text{Volume at STP}}=\frac{75}{22.4}=3.35mole$

$\text{Moles of }N_2=\frac{\text{Volume of }N_2}{\text{Volume at STP}}=\frac{25}{22.4}=1.12mole$

Now we have to calculate the mole fraction of $CO_2$ .

$\text{Mole fraction of }CO_2=\frac{\text{Moles of }CO_2}{\text{Moles of }CO_2+\text{Moles of }N_2}$

$\text{Mole fraction of }CO_2=\frac{3.35}{3.35+1.12}=0.75$

Now we have to calculate the partial pressure of the $CO_2$ gas.

$\text{Partial pressure of }CO_2=\text{Mole fraction of }CO_2\times \text{Total pressure of gas}$

$\text{Partial pressure of }CO_2=0.75mole\times 300Kpa=225Kpa=225Kpa\times \frac{0.145\text{ psia}}{1Kpa}=32.625\text{ psia}$

conversion used : (1 Kpa = 0.145 psia)

Therefore, the partial pressure of the $CO_2$ in the tank in psia is, 32.6 psia.

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2 years ago

PLEASE HELP 20 points

777dan777 [17]

n = 1.5atm (15L) / .0821 (280k) = .98 mol NaCl

NaCl = 22.99g Na + 35.45g Cl = 58.44g NaCl

58.44g NaCl x .98 mol NaCl = 57.27g NaCl

Explanation:

hope you get it right :)

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2 years ago