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Lynna [10]
3 years ago
5

What is the effect of the following on the volume of 1 mol of an ideal gas? The temperature changes from 305 K to 32°C and the p

ressure changes from 2 atm to 101 kPa.
A. Volume increases by 200%
B. Volume decreases to 50% of its original value
C. Volume decreases by 100%
D. Volume increases by 100%
E. Volume does not change
Chemistry
1 answer:
ryzh [129]3 years ago
7 0

Answer:

The volume increases by 100%.

Explanation:

<u>Step 1:</u> Data given

Number of moles ideal gas = 1 mol

Initial temperature = 305 K

Final temperature = 32°C + 273.15 = 305.15 K

Initial pressure = 2 atm

final pressure = 101 kPa = 0.996792 atm

R = gasconstant = doesn't change

V1 = initial volume

V2= the final volume

<u>Step 2: </u>Calculate volume of original gas

P*V = n*R*T

(P*V)/ T = constante

(P1 * V1) / T1 = (P2 * V2)/ T2

In this situation we have:

(2atm * V1)/ 305  = (0.996792 *V2) / 305.15

0.006557*V1 = 0.003266*V2

V2 = 2*V1

We see that the final volume is twice the initial volume. So the volume gets doubled. The volume increases by 100%.

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First we need to calculate molar mass of <span>NaHCO3. Molar mass is mass of 1 mole of a substance. It is the sum of relative atomic masses, which are masses of atoms of the elements.

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