A vessel contains 1.6 g of dioxygen at STP (273.15K, 1 atm pressure). The gas is now transferred to another vessel at constant temperature, where pressure becomes half of the original pressure. Calculate

(i) volume of the new vessel.

(ii) number of molecules of dioxygen.

Answers (1)

P_{1}=1 \; atm

T_{1}=273\; K

We will be calculating V1 now,

We know that 32 g of oxygen occupies 22.4 L of volume at STP+

Hence, 1.6 g Of O2 will occupy,

1.6\; g\; of\; Oxygen\times \frac{22.4\; L}{32\; g\; of\; oxygen}=1.12\; L

Hence\; V_{1}=1.12\; L

We know that, p_{2}=p_{1}/2=\frac{1}{2}=0.5 \; atm

Now we must calculate V_{2}

As per Boyle's law, P_{1}V_{1}=P_{2}V_{2}

Therefore, V_{2}=\frac{P_{1}V_{1}}{2}

\frac{1\; atm\times 1.12\; L}{2}=0.5\; atm\times v_{2}

Therefore, V_{2}=2.24L

(iii) Number of molecules of O2 that are present in the vessel,

= 6.023\times 10^{23}\times \frac{1.6}{32}=3.011\times 10^{22}

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