Given below are two statements : one is labelled as Assertion (A) and the other is labelled as Reason (R) :Assertion (A) : NH3 gas is more easily liquefiable than CO2 gas.Reason (R) : NH3 gas has higher critical temperature than that of CO2 gas.Both (A) and (R) are true and (R) is the correct explanation of (A)Both (A) and (R) are true and (R) is not the correct explanation of (A)(A) is true but (R) is falseBoth (A) and (R) is false
Question
Given below are two statements : one is labelled as Assertion (A) and the other is labelled as Reason (R) :Assertion (A) : NH3 gas is more easily liquefiable than CO2 gas.Reason (R) : NH3 gas has higher critical temperature than that of CO2 gas.Both (A) and (R) are true and (R) is the correct explanation of (A)Both (A) and (R) are true and (R) is not the correct explanation of (A)(A) is true but (R) is falseBoth (A) and (R) is false
Solution
The correct answer is: Both (A) and (R) are true and (R) is not the correct explanation of (A).
Explanation: Assertion (A) is true because NH3 (Ammonia) is more easily liquefiable than CO2 (Carbon Dioxide). This is due to the fact that Ammonia molecules are polar and can form hydrogen bonds, which makes them stick together more easily and thus easier to liquefy.
Reason (R) is also true because the critical temperature of NH3 is indeed higher than that of CO2. The critical temperature of a gas is the temperature above which it cannot be liquefied, no matter how much pressure is applied. For NH3, this temperature is -33.34°C, while for CO2 it is -56.6°C.
However, (R) is not the correct explanation of (A). The reason NH3 is more easily liquefiable than CO2 is not because it has a higher critical temperature, but because of its ability to form hydrogen bonds due to its polarity.
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