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2 years ago

PLEASE HURRY AND SHOW WORK

Chemistry

1 answer:

IgorC [24]2 years ago

3 0

Answer:

The answer to your question is P = 1.64 atm

Explanation:

Data

Volume = 2.5 x 10⁷ L

Temperature = 22°C

Pressure = ?

Moles = 1.7 x 10⁶

R = 0.082 atm L/ mol°K

Process

1.- Convert temperature to °K

Temperature = 22 + 273

= 295°K

2.- Use the Ideal gas law to solve this problem

PV = nRT

- Solve for P

P = nRT / V

- Substitution

P = (1.7 x 10⁶)(0.082)(295) / 2.5 x 10⁷

- Simplification

P = 41123000 / 2.5 x 10⁷

- Result

P = 1.64 atm

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2 years ago

In a titration, 4.7 g of an acid (HX) requires 32.6 mL of 0.54 M NaOH(aq) for complete reaction. What is the molar mass of the a

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Mass of an acid (HX) = 4.7 g

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First we have to calculate the moles of NaOH.

$\text{Moles of }NaOH=\text{Molarity of }NaOH\times \text{Volume of solution}=0.54mole/L\times 0.0326L=0.017604mole$

Now we have to calculate the moles of an acid.

In the titration, the moles of an acid will be equal to the moles of NaOH.

Moles of an acid = Moles of NaOH = 0.017604 mole

Now we have to calculate the molar mass of and acid.

$\text{Moles of an acid}=\frac{\text{Mass of an acid}}{\text{Molar mass of an acid}}$

Now put all the given values in this formula, we get:

$0.017604mole=\frac{4.7g}{\text{Molar mass of an acid}}$

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