A container has a volume of #1 L# and holds #16 mol# of gas. If the container is expanded such that its new volume is #27 L#, how many moles of gas must be injected into the container to maintain a constant temperature and pressure?

Answer 1

#n_(added) = 416 mol#

Using the Ideal Gas Law:

#PV_1 = n_1rT# [1]

and

#PV_2 = n_2rT# [2]

Dividing [2] by [1]

#V_2/V_1 = n_2/n_1#
#n_2 = (27 L)/(1 L)(16 mol)#
#n_2 = 432 mol#

Subtract 16 to find the amount that you must add:

#n_(added) = 416 mol#
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Answer 2

Using the ideal gas law ( PV = nRT ), where ( P ) is pressure, ( V ) is volume, ( n ) is the number of moles of gas, ( R ) is the gas constant, and ( T ) is temperature, we can find that the number of moles of gas needed to maintain constant temperature and pressure when the volume increases to 27 L is approximately 1.5 mol.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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