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ankoles [38]
2 years ago
14

at atmoshperic pressure, a balloon contains 2.00L of nitrogen of gas. How would the volume change if the Kelvin temperature were

only 75 percent of its original value
Chemistry
1 answer:
Nataly [62]2 years ago
5 0

<u>Answer:</u> The percent change in volume will be 25 %

<u>Explanation:</u>

To calculate the final temperature of the system, we use the equation given by Charles' Law. This law states that volume of the gas is directly proportional to the temperature of the gas at constant pressure.

Mathematically,

\frac{V_1}{T_1}=\frac{V_2}{T_2}

where,

V_1\text{ and }T_1 are the initial volume and temperature of the gas.

V_2\text{ and }T_2 are the final volume and temperature of the gas.

We are given:

V_1=2L\\T_1=T_1\\V_2=?\\T_2=75\% \text{ of }T_1=0.75\times T_1

Putting values in above equation, we get:

\frac{2L}{T_1}=\frac{V_2}{0.75\times T_1}\\\\V_2=\frac{2\times 0.75\times T_1}{T_1}=1.5L

Percent change of volume = \frac{\text{Change in volume}}{\text{Initial volume}}\times 100

Percent change of volume = \frac{(2-1.5)}{2}\times 100=25\%

Hence, the percent change in volume will be 25 %

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The reaction between phosphoric acid and ammonia that produces ammonium phosphate can be written as follows:
3NH3 + H3PO4 ..................> (NH4)3PO4

From the periodic table:
molar mass of nitrogen = 14 grams
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based on this:
molar mass of 3NH3 = 3 (14 + 3(1)) = 51 grams
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molar mass of  (NH4)3PO4 = 3 (14 + 4(1)) + 30.9 + 4(16) = 54 + 30.9 + 64
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Therefore, 97.9 grams of phosphoric acid is required to produced 148.9 grams of ammonium phosphate.
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