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lions [1.4K]
2 years ago
11

The forensic technician at a crime scene has just prepared a luminol stock solution by adding 13.0 g of luminol into a total vol

ume of 75.0 mL of H2O. What is the molarity of the stock solution of luminol?
Chemistry
1 answer:
Andrews [41]2 years ago
3 0

Answer:

0.978 M

Explanation:

Given data

  • Mass of luminol (solute): 13.0 g
  • Volume of the solution = volume of water: 75.0 mL = 0.0750 L

We can find the molarity of the stock solution of luminol using the following expression.

M = mass of solute / molar mass of solute × liters of solution

M = 13.0 g / 177.16 g/mol × 0.0750 L

M = 0.978 M

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What would be the pressure of 1.0g of O2 contained in a 4.00L container at 293 K?
Natalka [10]

Answer: The pressure will be equal to 0.19 atm.

Explanation:

The Ideal Gas Equation states the relationship among the pressure, temperature, volume, and number of moles of a gas.

The equation is:

PV=nRT

where P = pressure in <em>atm</em>

           V = volume in <em>L</em>

           n = numbers of moles of gas in <em>mol</em>

           R = universal gas constant = 0.08206 \frac{L-atm}{mol - K}

           T = temperature in <em>K</em>

Based on the problem,

mass of O2 = 1.0 g

V = 4.00 L

T = 293 K

mol of O2  = ?

P = ?

We need to calculate the moles of O2 before we can use the Ideal Gas Equation. To solve the number of moles, we use the equation:

no. of moles = \frac{given\ mass\ (in\ grams) }{molar\ mass\ (in\ \frac{grams}{mole}) }

The molar mass of O2 is 32 g/mol, therefore,

no. of moles = \frac{1.0g}{32\frac{g}{mol} }

no. of moles of O2 = 0.03125 mol.

Now we substitute the values into the Ideal Gas equation:

P(4.00L) = (0.03125 mol)(0.08206\frac{L-atm}{mol-K} )(293K)

Solving for P, we will get

P=\frac{(0.03125mol)(0.08206\frac{L-atm}{mol-K})(293K) }{4.00L} \\\\P= 0.1878 atm.

In correct significant figures, P is equal to 0.19 atm.

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3 years ago
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