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hodyreva [135]
3 years ago
14

A cylinder with a moveable piston contains 0.552 mol of gas and has a volume of 259 mL . Part A What will its volume be if an ad

ditional 0.232 mol of gas is added to the cylinder? (Assume constant temperature and pressure.) View Available Hint(s)
Chemistry
1 answer:
Naddik [55]3 years ago
7 0

Answer:

The new volume will be 367mL

Explanation:

Using PV = nRT

V1 = 259mL = 0.000259L

n1 = 0.552moles

At constant temperature and pressure, the value is

P * 0.000259 = 0.552 * RT ------equation 1

= 0.552 / 0.000259

= 2131.274

V2 = ?

n2 = 0.552 + 0.232

n2 = 0.784mole

Using ideal gas equation,

PV = nRT

P * V2 = 0.784 * RT ---------- equation 2

Combining equations 1 and 2 we have;

V2 = 0.784 / 2131.274

V2 = 0.000367L

V2 = 367mL

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In general, if a reaction is spontaneous, the reactants possess more free energy than the products.  

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Which of the following is a unit of length? O A. A liter O B. A kilogram C. A meter O D. A degree​
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The density of an aqueous solution of nitric acid is 1.64 g/mL and the concentration is 1.85 M. What is the concentration of thi
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Answer:

Mass % of the solution = 7.1067 %

Explanation:

Given :

Molarity of nitric acid solution = 1.85 M

Density of the solution = 1.64 g/mL

<u>Molarity of a solution is defined as the number of moles of solute present in 1 liter of the solution.</u>

Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}

Lets, consider the volume of the solution = 1 L

Thus,

Moles of nitric acid present in the solution:

Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}

Moles of Nitric acid=Molarity \times {Volume\ of\ the\ solution}

So,

Moles of Nitric acid  = 1.85 moles

Molar mass of nitric acid = 63 g/mol

The mass of Nitric acid can be find out by using mole formula as:

moles=\frac{Mass\ taken}{Molar\ mass}

Thus,  

Mass\ of\ Nitric\ acid=Moles \times Molar mass}

Mass\ of\ Nitric\ acid=1.85 g \times 63 g/mol}

<u>Mass of Nitric acid = 116.55 g</u>

Also,

Density=\frac{Mass}{Volume}

Given : Density = 1.64 g/mL

Also, 1 L = 10³ mL

Volume of the solution is 1000 mL

So, mass of the solution:

Mass\ of\ the\ solution=Density \times {Volume\ of\ the\ solution}

Mass\ of\ the\ solution=1.64 g/mL \times {1000 mL}

<u>Mass of the solution  = 1640 g</u>

Mass % is defined as the mass of solute in 100 g of the solution. The formula for the calculation of mass % is shown below:

Mass \% =\frac{Mass\ of\ the\ solute}{Mass\ of\ the\ solution} \times {100}

So,

Mass \%=\frac{116.55}{1640} \times {100}

<u>Mass % = 7.1067 %</u>

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