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charle [14.2K]
3 years ago
11

If two gases with pressures of 2 atm and 3 atm are mixed at a constant temperature, what will the total pressure be?

Chemistry
2 answers:
slamgirl [31]3 years ago
8 0
If two gases with pressures of 2 atm and 3 atm are mixed at constant temperature, the total pressure will be the sum of the two pressures. Therefore the answer is D. 2 atm + 3 atm or 5 atm will be the total pressure of the gas mixture. 
kotegsom [21]3 years ago
6 0

Answer:

D. 2 atm + 3 atm

Explanation:

Given:

Pressure Gas 1 = 2 atm

Pressure Gas 2 = 3 atm

Explanation:

As per Dalton's Law in a mixture of gases, the total pressure is the sum of the partial pressures of the individual gases.

Ptotal = P1 + P2 + P3 + ...

where P1, P2,P3 are the partial pressures

Therefore for the given gas mixture, the total pressure would be:

Ptotal = 2 atm + 3 atm = 5 atm

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How many moles are in 12 liters of Cl2?
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Answer:

\boxed {\boxed {\sf 0.54 \ mol \ Cl_2}}

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A mole is any quantity of a substance that contains 6.02 × 10²³ particles. At standard temperature and pressure, or STP, 1 mole of as is equal to 22.4 liters. This is true for any gas, regardless of the specific kind.

Although it is not specified, we can assume this gas is at STP. Let's set up a ratio using this information: 22.4 L/mol

\frac {22.4 \ L \ Cl_2}{1 \ mol \ Cl_2}

Multiply by the given number of liters: 12

12 \ L \ Cl_2 *\frac {22.4 \ L \ Cl_2}{1 \ mol \ Cl_2}

Flip the ratio so the liters of chlorine cancel.

12 \ L \ Cl_2 * \frac {1 \ mol \ Cl_2}{22.4 \ L \ Cl_2}

12  * \frac {1 \ mol \ Cl_2}{22.4 }

\frac {12}{22.4 }  \ mol \ Cl_2

0.53571428571 \ mol \ Cl_2

The original measurement of liters has 2 significant figures, so our answer must have the same.

For the number we found, that is the hundredth place.

  • 0.53<u>5</u>71428571

The 5 in the thousandth place tells us to round the 3 up to a 4.

0.54 \ mol \ Cl_2

12 liters of chlorine gas at STP is approximately <u>0.54 moles of chlorine gas.</u>

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