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2 years ago

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If you collect 1.75 L of hydrogen gas during a lab experiment when the room temperature is 23oC and the barometric pressure is 1

05 kPa how many moles of hydrogen will you have

1 answer:

ziro4ka [17]2 years ago

8 0

Answer:

$n=0.0747mol$

Explanation:

Hello,

In this case, since we can consider hydrogen gas as an ideal gas, we check the volume-pressure-temperature-mole relationship by using the ideal gas equation:

$PV=nRT$

Whereas we are asked to compute the moles given the temperature in Kelvins, thr pressure in atm and volume in L as shown below:

$n=\frac{105kPa*\frac{0.009869atm}{1kPa}*1.75L}{0.082\frac{atm*L}{mol*K}*(23+273.15)K} \\\\n=0.0747mol$

Best regards.

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Air containing 0.04% carbon dioxide is pumped into a room whose volume is 6000 ft3. The air is pumped in at a rate of 2000 ft3/m

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Here is the full question:

Air containing 0.04% carbon dioxide is pumped into a room whose volume is 6000 ft3. The air is pumped in at a rate of 2000 ft3/min, and the circulated air is then pumped out at the same rate. If there is an initial concentration of 0.2% carbon dioxide, determine the subsequent amount in the room at any time.

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$R_{in}$ = 0.8

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$12 =2.4 + Ce^{-\frac{1}{3}}(0)$

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$A(t) = 2.4 +9.6e^{-\frac{t}{3}}$

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∴ the concentration at 10 minutes is ;

= $\frac{2.74}{6000}*100$ %

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