Question

Oxygen and chlorine gas are mixed in a container with partial pressures of 52 kPa and 60 kPa, respectively. What is the total pressure inside the container?

Answer 1

Answer:$P_T=112kPa$

Explanation:

Hello,

In this case case, the Dalton's law is useful to compute the total pressure in terms of the partial pressure of the present gases:

$P_T=P_{O_2}+P_{Cl_2}=52kPa+60kPa\\\\P_T=112kPa$

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Answer 2

Answer:

The total pressure inside the container is 112 kPa

Explanation:

The partial pressure of a gas is the pressure it exerts on a mixture of gases. The total pressure of the mixture is the sum of the partial pressures that each contained gas.  That is, in cases where gas mixtures are involved, the total pressure of the gas is related to the partial pressures, that is, the pressures of the individual gaseous components of the mixture.

Dalton established that the total pressure of a mixture of gases is equal to the sum of the pressures that each gas would exert if it were only in the container. This is called Dalton's Law and is expressed mathematically as:

PT=P1 + P2 + P3 + P4 +...+ Pn

where 1, 2, 3, 4, ..., n are the gases present in the mixture.

In this case:

Ptotal=Poxygen + Pchlorine

Being:

• Poxygen= 52 kPa
• Pchlorine= 60 kPa

Replacing:

Ptotal= 52 kPa+ 60 kPa

Ptotal= 112 kPa

The total pressure inside the container is 112 kPa