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alexandr1967 [171]
3 years ago
5

A sample of hydrogen occupies a volume of 351 mL at a temperature of 20 degrees Celsius. What is the new volume if the temperatu

re increases to 38 degrees Celsius? (Do not forget to convert to Kelvin!)
Chemistry
1 answer:
xeze [42]3 years ago
6 0
Volume of Hydrogen V1 = 351mL 
Temperature T1 = 20 = 20 + 273 = 293 K 
Temperature T2 = 38 = 38 + 273 = 311 K 
We have V1 x T2 = V2 x T1 
So V2 = (V1 x T2) / T1 = (351 x 311) / 293 = 372.56 
Volume at 38 C = 373 ml
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Answer: 190 g of magnesium chloride can be produced by reacting 2 moles of chlorine gas with excess magnesium bromide.

Explanation:

The balanced chemical reaction is;

Cl_2+MgBr_2\rightarrow MgCl_2+Br_2

Cl_2 is the limiting reagent as it limits the formation of product and MgBr_2 is the excess reagent.

According to stoichiometry :

1 mole of Cl_2 produces = 1 mole of MgCl_2

Thus 2 moles of Cl_2 will produce=\frac{1}{1}\times 2=2moles  of MgCl_2

 Mass of MgCl_2=moles\times {\text {Molar mass}}=2moles\times 95g/mol=190g

Thus 190 g of magnesium chloride can be produced by reacting 2 moles of chlorine gas with excess magnesium bromide

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If 20.0 mL of glacial acetic acid (pure HC2H3O2HC2H3O2) is diluted to 1.70 L with water, what is the pH of the resulting solutio
Andreas93 [3]

Answer:

The answer to your question is pH = 0.686

Explanation:

Data

Acetic acid = 20 ml

Final volume = 1.7 L

pH = ?

density = 1.05 g/ml

Process

1.- Calculate the mass of acetic acid

density = mass / volume

mass = density x volume

mass = 1.05 x 20

mass = 21 g

2.- Calculate the moles of acetic acid (CH₃COOH)

Molar mass = (12 x 2) + (16 x 2) + (4 x 1)

                   = 24 + 32 + 4

                   = 60 g

                 60 g of acetic acid ---------------- 1 mol

                 21 g of acetic acid ----------------- x

                 x = (21 x 1) / 60

                 x = 0.35 moles

3.- Calculate the concentration

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