The air is so dry that when it hits a snowpack, the frozen water evaporates, going directly from the ice to vapor and bypassing the liquid phase entirely. This is called sublimation, and it's a common way for snow to disappear in the arid West."
Answer:Correct
Explanation:According to the balanced chemical reaction, 2 mol FeBr3 are consumed for every 3 mol Na2S consumed.
Answer:
• 1.62432 moles of nitrogen
• Tire Pressure: 2.74 * 10⁵ Pa
• The tires will burst
• Pressure: 244 kPa
Explanation:
• We can determine the number of moles of nitrogen using the formula pV = nRT, where p = pressure, V = volume, n = number of moles, R = gas constant, and T = absolute temperature.
Now remember we have our initial pressure in kilopascals so let's convert to pascals (249 pascals). The volume is given in liters, so let's convert into m². And the initial temperature is given in Celsius ⇒ our absolute temperature in Kelvins.
![\mathrm{p\:}=\mathrm{249 kPa\:} = \mathrm{2.49 * 10^5\:},\\\mathrm{15.6L\:} =\mathrm{0.0156m^2\:},\\\mathrm{R\:}=\mathrm{8.314J/mol*K\:},\\\mathrm{T\:}=\mathrm{21C\:} + \mathrm{273\:}=\mathrm{294K\:}](https://tex.z-dn.net/?f=%5Cmathrm%7Bp%5C%3A%7D%3D%5Cmathrm%7B249%20kPa%5C%3A%7D%20%3D%20%5Cmathrm%7B2.49%20%2A%2010%5E5%5C%3A%7D%2C%5C%5C%5Cmathrm%7B15.6L%5C%3A%7D%20%3D%5Cmathrm%7B0.0156m%5E2%5C%3A%7D%2C%5C%5C%5Cmathrm%7BR%5C%3A%7D%3D%5Cmathrm%7B8.314J%2Fmol%2AK%5C%3A%7D%2C%5C%5C%5Cmathrm%7BT%5C%3A%7D%3D%5Cmathrm%7B21C%5C%3A%7D%20%2B%20%5Cmathrm%7B273%5C%3A%7D%3D%5Cmathrm%7B294K%5C%3A%7D)
Respectively the moles of nitrogen in each tire should be:
![\mathrm{n\:}=\mathrm{pV/RT\:}=\mathrm{(2.49*10^5)(0.0156)/(8.314)(294)\:}=\frac{\left(2.49\cdot \:10^5\right)\left(0.0156\right)}{\left(8.134\right)\left(294\right)}=\frac{3884.4}{2391.396}\\](https://tex.z-dn.net/?f=%5Cmathrm%7Bn%5C%3A%7D%3D%5Cmathrm%7BpV%2FRT%5C%3A%7D%3D%5Cmathrm%7B%282.49%2A10%5E5%29%280.0156%29%2F%288.314%29%28294%29%5C%3A%7D%3D%5Cfrac%7B%5Cleft%282.49%5Ccdot%20%5C%3A10%5E5%5Cright%29%5Cleft%280.0156%5Cright%29%7D%7B%5Cleft%288.134%5Cright%29%5Cleft%28294%5Cright%29%7D%3D%5Cfrac%7B3884.4%7D%7B2391.396%7D%5C%5C)
![= 1.62432\dots \mathrm{moles\:}\mathrm{of\:}\mathrm{nitrogen\:}](https://tex.z-dn.net/?f=%3D%201.62432%5Cdots%20%5Cmathrm%7Bmoles%5C%3A%7D%5Cmathrm%7Bof%5C%3A%7D%5Cmathrm%7Bnitrogen%5C%3A%7D)
• We can solve this part similarly. All our values will be the same, besides the temperature, as we have to consider both the initial and final temperature here.
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![\mathrm{p_2\:}=\mathrm{(2.49*10^5)(324)/(294)\:} }=\frac{\left(2.49\cdot \:10^5\right)\left(324\right)}{294}=\frac{40338000}{147}=274408.16326\dots](https://tex.z-dn.net/?f=%5Cmathrm%7Bp_2%5C%3A%7D%3D%5Cmathrm%7B%282.49%2A10%5E5%29%28324%29%2F%28294%29%5C%3A%7D%20%7D%3D%5Cfrac%7B%5Cleft%282.49%5Ccdot%20%5C%3A10%5E5%5Cright%29%5Cleft%28324%5Cright%29%7D%7B294%7D%3D%5Cfrac%7B40338000%7D%7B147%7D%3D274408.16326%5Cdots)
![=2.74408.16326*10^5\dots\mathrm{Pa}](https://tex.z-dn.net/?f=%3D2.74408.16326%2A10%5E5%5Cdots%5Cmathrm%7BPa%7D)
• The text mentions that the tires will burst when the internal pressure reaches 269kP. From part #2 we know that the final pressure will be, in kilopascals, 274kP. As 274 > 269, the tires will burst in Death Valley.
• We would want the final temperature = breaking pressure. Therefore,
![\mathrm{p_2\:}=\mathrm{(269)(294)/(324)\:} }=\frac{79086}{324}=\frac{13181}{54}=244.09259\dots\mathrm{kPa\:} }](https://tex.z-dn.net/?f=%5Cmathrm%7Bp_2%5C%3A%7D%3D%5Cmathrm%7B%28269%29%28294%29%2F%28324%29%5C%3A%7D%20%7D%3D%5Cfrac%7B79086%7D%7B324%7D%3D%5Cfrac%7B13181%7D%7B54%7D%3D244.09259%5Cdots%5Cmathrm%7BkPa%5C%3A%7D%20%7D)
Answer:
False
Explanation:
The Avogadro's number is not used to determine the number of subatomic particles in an atom.
Subatomic particles of an atom are the protons, neutrons and electrons.
The protons are the positively charged particles in an atom
Neutrons do not carry any charges
Electrons carry negative charges.
The number of protons, neutrons and electrons in an atom are experimentally determine using spectrometric techniques.
Answer:
The reaction will proceed to the left to attain equilibrium.
Explanation:
The question is missing but I guess it must be about <em>how the reaction will proceed to attain equilibrium.</em>
First, we have to calculate the partial pressures using the ideal gas equation.
![pP_{4}=\frac{2.50mol\times (0.08206atm.L/mol.K)\times 673K}{25.0L} =5.52atm](https://tex.z-dn.net/?f=pP_%7B4%7D%3D%5Cfrac%7B2.50mol%5Ctimes%20%280.08206atm.L%2Fmol.K%29%5Ctimes%20673K%7D%7B25.0L%7D%20%3D5.52atm)
![pP_{2}=\frac{1.50mol\times (0.08206atm.L/mol.K)\times 673K}{25.0L}=3.31atm](https://tex.z-dn.net/?f=pP_%7B2%7D%3D%5Cfrac%7B1.50mol%5Ctimes%20%280.08206atm.L%2Fmol.K%29%5Ctimes%20673K%7D%7B25.0L%7D%3D3.31atm)
Now, we have to calculate the reaction quotient (Qp).
![Qp=\frac{pP_{2}^{2}}{pP_{4}} =\frac{3.31^{2} }{5.52} =1.98](https://tex.z-dn.net/?f=Qp%3D%5Cfrac%7BpP_%7B2%7D%5E%7B2%7D%7D%7BpP_%7B4%7D%7D%20%3D%5Cfrac%7B3.31%5E%7B2%7D%20%7D%7B5.52%7D%20%3D1.98)
Since Qp > Kp, the reaction will proceed to the left to attain equilibrium.