The solvent is the part of the solution that

If you have 2.4L of SO2 gas (at STP) how many moles of sulfur dioxide do you have?

Andru [333]

Answer:

0.107 mole of SO2.

Explanation:

1 mole of a gas occupy 22.4 L at standard temperature and pressure (STP).

With the above information, we can simply calculate the number of mole of SO2 that will occupy 2.4 L at STP.

This can be obtained as follow:

22.4 L contains 1 mole of SO2.

Therefore, 2.4 L will contain = 2.4/22.4 = 0.107 mole of SO2.

Therefore, 0.107 mole of SO2 is present in 2.4 L at STP.

4 0

4 years ago

Based off of the plum pudding model, what should've happened in the gold foil experimet

stepan [7]

Based on that, alpha-particle get attracted and many of the particles were not gone away without deflection

3 0

3 years ago

Is baking cookies a chemical or physical change

Natalija [7]

Answer: Its a chemical change because the materials are mix to make the dough

I hope that I help you.

6 0

3 years ago

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The equilibrium constant Kp for the reaction I2(g) + Br2(g) ⇀↽ 2 IBr(g) + 11.7 kJ is 280 at 150◦C. Suppose that a quantity of IB

mixas84 [53]

Answer:

$\large \boxed{\text{0.0120 atm }}$

Explanation:

The balanced equation is

I₂(g) + Br₂(g) ⇌ 2IBr(g)

Data:

Kp = 280

p(IBr) = 0.200 atm

1. Set up an ICE table.

Let p = the initial pressure of IBr. Then

$\begin{array}{ccccccc}\rm \text{I}_{2}& + & \text{Br}_{2} & \, \rightleftharpoons \, & \text{2IBr} & & \\0 & & 0 & & p & & \\+x & & +x & & -2x & &\\x & & x} & & 280 & & \\\end{array}$

2. Calculate p(I₂)

$\begin{array}{rcl}K_{\text{p}}&=&\dfrac{p_{\text{IBr}}^{2}} {p_{\text{I}_2}^{2}}\\\\280&=&{\dfrac{0.200^{2}}{x^{2}}&&\\\\280x^{2} & = &0.0400\\x^{2} & = &\dfrac{0.0400}{280 }\\\\& = & 1.429 \times 10^{-4}\\x & = & \textbf{0.0120 atm}\\\end{array}\\\text{The partial pressure of iodine is $\large \boxed{\textbf{0.0120 atm }}$}$ }

Check:

$\begin{array}{rcl}{\dfrac{0.200^{2}}{0.0120^{2}}}&=&280\\\\280& =& 280\\\end{array}$

8 0

3 years ago

What would be the change in pressure in a sealed 10.0 l vessel due to the formation of n2 gas when the ammonium nitrite in 2.40

larisa86 [58]

The change in pressure in a sealed 10.0L vessel is 5.28 atm

calculation

The pressure is calculated using the ideal gas equation

That is P=n RT

where;

P (pressure)= ?

v( volume) = 10.0 L

n( number of moles) which is calculated as below

write the equation for decomposition of NH₄NO₂

NH₄NO₂ → N₂ +2H₂O

Find the moles of NH₄NO₂

moles = molarity x volume in liters

= 2.40 l x 0.900 M =2.16 moles

Use the mole ratio to determine the moles of N₂

that is from equation above NH₄NO₂:N₂ is 1:1 therefore the moles of N₂ is also =2.16 moles

R(gas constant) =0.0821 l.atm/mol.K

T(temperature) = 25° c into kelvin = 25 +273 =298 K

make p the subject of the formula by diving both side by V

P = nRT/V

p ={ (2.16 moles x 0.0821 L.atm/mol.K x 298 K) /10.0 L} = 5.28 atm.

3 0

3 years ago

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