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siniylev [52]
2 years ago
12

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

Chemistry
1 answer:
bearhunter [10]2 years ago
8 0

n = 0.100 moles

At STP (standard temperature pressure), where gas is collected, the temperature is 0°C and the pressure is 1 atm.

\\$\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

#SPJ4

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Write the net ionic equ.
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a) AgNO3 + KI → AgI + KNO3

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Explanation:

a) AgNO3 + KI → Ag+ + NO3- + K+ + I-

Ag+ + NO3- + K+ + I-  → AgI + KNO3

AgNO3 + KI → AgI + KNO3

b) Ba(OH)2 + 2HNO3 → Ba^2+ + 2OH- + 2H+ + 2NO3-

Ba^2+ + 2OH- + 2H+ + 2NO3- → Ba(NO3)2 + 2H2O

Ba(OH)2 + 2HNO3 → Ba(NO3)2 + 2H2O

c) 2Na3PO4  + 3Ni(NO3)2 → 6Na+ + 2PO4^3- + 3Ni^2+ + 6NO3-

6Na+ + 2PO4^3- + 3Ni^2+ + 6NO3- →  Ni3(PO4)2 + 6NaNO3

2Na3PO4  + 3Ni(NO3)2  → Ni3(PO4)2 + 6NaNO3

d) 2Al(OH)3 + 3H2SO4 → 2Al^3+ + 6OH- + 6H+ + 3SO4^2-

2Al^3+ + 3OH- + 3H+ + 3SO4^2- → Al2(SO4)3 + 6H2O

2Al(OH)3 + 3H2SO4 → Al2(SO4)3 + 6H2O

7 0
3 years ago
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Answer:

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Explanation:

In writing the cell notation for an electrochemical cell, the anode is written on the left hand side while the cathode is written on the right hand side. The two half cells are separated by two thick lines which represents the salt bridge.

For the cell discussed in the question; the Mn(s)/Mn^2+(aq) is the anode while the Co^2+(aq)/Co(s) half cell is the cathode.

Hence I can write; Mn(s)/Mn^2+(aq)//Co^2+(aq)/Co(s)

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