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vodomira [7]
3 years ago
5

In preparation for a demonstration, your professor brings a 1.50−L bottle of sulfur dioxide into the lecture hall before class t

o allow the gas to reach room temperature. If the pressure gauge reads 988 psi and the lecture hall is 25°C, how many moles of sulfur dioxide are in the bottle? In order to solve this problem, you will first need to calculate the pressure of the gas. Hint: The gauge reads zero when 14.7 psi of gas remains.
Chemistry
1 answer:
solmaris [256]3 years ago
4 0

Answer:

4.81 moles

Explanation:

The total pressure of the gas = Pressure at which gauge reads zero + pressure read by it.

Pressure at which gauge reads zero = 14.7 psi

Pressure read by the gauge = 988 psi

Total pressure = 14.7 + 988 psi = 1002.7 psi

Also, P (psi) = P (atm) / 14.696

Pressure = 1002.7 / 14.696  = 68.2297 atm

Temperature = 25 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T = (25 + 273.15) K = 298.15 K  

Volume = 1.50 L

Using ideal gas equation as:

PV=nRT

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

68.2297 atm × 1.5 L = n × 0.0821 L.atm/K.mol × 298.15 K  

⇒n = 4.81 moles

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</span>where here now it has two lonely valence electrons, one on the s and the other on the p, so that it can do a total of two bonds.</span><span>That's why bromine and sodium can form </span>

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A sample 0.100 moles of a gas is collected at at stp. what is the volume of the gas in liters? group of answer choices 2.44 l
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n = 0.100 moles

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\\$\therefore$ Temperature $(T)=0^{\circ} \mathrm{C}=0^{\circ}+273

                              =273K

          Pressure $(P)=1$ atm.

The ideal gas equation indicates that

\begin{aligned}& P V=n R T \Rightarrow V=\frac{n R T}{P} \\\therefore & R=\text { gas constant }=0.0821 \mathrm{~L} \cdot \mathrm{cetm} / \mathrm{mo} / \cdot K\end{aligned}

 \begin{aligned}&V=\frac{0.100 \mathrm{~mol} \cdot \times 0.0821 \mathrm{~L} \cdot \mathrm{atm} / \mathrm{mol} . \mathrm{K} \times 273 \mathrm{~K}}{1 \mathrm{~atm}} \\&V=\frac{2.24 L}{1}\end{aligned}\\

V=2.24L

Group of answer choices 2.44L .The volume occupied by  mole of a given gas at a given temperature and pressure is expressed as the gas's molar volume.

The most typical illustration is the molar volume of a gas at STP, which is equal to 2.44L for 1 mole of any ideal gas at a temperature of 273.15 Kand a pressure of 1 atm.

Hence, the volume of the gas is 2.24L.

<h3 /><h3>What is the STP?</h3>

A unit is stated to have a temperature of absolute zero (273 Kelvins) and an atmospheric pressure of one atmosphere, or 1 atm, at standard temperature and pressure. Additionally, at STP, a mole of any gas takes up 22.414 L of space. Keep in mind that this idea only applies to gases.

For experimental measurements to be established under standard conditions that allow for comparisons between various sets of data, standard temperature and pressure must be met.

To learn more about STP, Visit:

brainly.com/question/1626157

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