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Natasha_Volkova [10]
3 years ago
12

The pressure of a gas at the triple point of water is 1.20 atm. Part A If its volume remains unchanged, what will its pressure b

e at the temperature at which CO2CO2 solidifies?
Chemistry
1 answer:
kondaur [170]3 years ago
7 0

The pressure P2 at the temperature which CO2 gets solidifies is 0.857 atm.

<u>Explanation:</u>

The relation between temperature T and the pressure P is that it is proportional to each other.

                                      T ∝ P

As the temperature decreases, the pressure also decreases which is given by

                             T1 / T2 = P1 / P2

At the triple point of water, the temperature equals 273 K.

Consider T1 = 273 K,  P1 = 1.20 atm

The temperature T2 of the CO2 solidifies equals 195 K

                            (273 / 195) = (1.20 / P2)

                              P2 = (195 x 1.20) / 273

                             P2 = 0.857 atm.

The pressure P2 at the temperature which CO2 gets solidifies is 0.857 atm.

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Answer:

Approximately 53.3\; \rm g.

Explanation:

Lookup Avogadro's Number: N_{\rm A} = 6.02\times 10^{23}\; \rm mol^{-1} (three significant figures.)

Lookup the relative atomic mass of \rm H, \rm S, and \rm O on a modern periodic table:

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(For example, the relative atomic mass of \rm H is 1.008 means that the mass of one mole of \rm H\! atoms would be approximately 1.008\! grams on average.)

The question counted the number of \rm H_2SO_4 molecules without using any unit. Avogadro's Number N_{\rm A} helps convert the unit of that count to moles.

Each mole of \rm H_2SO_4 molecules includes exactly (1\; {\rm mol} \times N_\text{A}) \approx 6.02\times 10^{23} of these \rm H_2SO_4 \! molecules.

3.27 \times 10^{23} \rm H_2SO_4 molecules would correspond to \displaystyle n = \frac{N}{N_{\rm A}} \approx \frac{3.27 \times 10^{23}}{6.02 \times 10^{23}\; \rm mol^{-1}} \approx 0.541389\; \rm mol of such molecules.

(Keep more significant figures than required during intermediary steps.)

The formula mass of \rm H_2SO_4 gives the mass of each mole of \rm H_2SO_4\! molecules. The value of the formula mass could be calculated using the relative atomic mass of each element:

\begin{aligned}& M({\rm H_2SO_4}) \\ &= (2 \times 1.008 + 32.06 + 4 \times 15.999)\; \rm g \cdot mol^{-1} \\ &= 98.702\; \rm g \cdot mol^{-1}\end{aligned}.

Calculate the mass of approximately 0.541389\; \rm mol of \rm H_2SO_4:

\begin{aligned}m &= n \cdot M \\ &\approx 0.541389\; \rm mol \times 98.702\; \rm g \cdot mol^{-1}\\ &\approx 53.3\; \rm g\end{aligned}.

(Rounded to three significant figures.)

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