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gavmur [86]
3 years ago
8

Which statement about the gas laws is correct?

Chemistry
1 answer:
Elena-2011 [213]3 years ago
4 0

Answer:

Gay-Lussac's law states that pressure and temperature are directly proportional

Explanation:

Gay-Lussac's law states that pressure and temperature are directly proportional. This always occurs if the volume keeps in constant.

n and V are not directly proportional, they are the same.

At Charles Gay Lussac's law

V1 = V2

n1 = n2

T1 < T2

P1 < P2

P1 / T1 = P2 / T2

If the pressure is contant:

V1 / T1 = V2 /T2

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Carbon 14 because it has an approximate half life of 5000 years. 
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A compound contains only nitrogen and oxygen and has a formula mass of 44.02. What is the formula of the compound
ch4aika [34]
N₂O

N = 14.01 amu
O ≈ 16 amu

14.01 × 2 = 28.02 ; 2 Nitrogen

44.02 - 28.02 = 16 ; 1 Oxygen

Check

28.02 + 16 ≈ 44.02amu
8 0
3 years ago
A flask containing 9.65 mL of liquid has a mass of 164.5g. The empty flask has a mass of 155.9 g. Calculate the density of the l
zlopas [31]

155.9

Explanation:

A flask containing 9.65 mL of liquid has a mass of 164.5g. The empty flask has a mass of 155.9

5 0
2 years ago
Is na2S an ionic compound,covalent compound,or acid
liq [111]

Na2S

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3 0
3 years ago
A student mixes a 10.0 mL sample of 1.0 M NaOH with a 10.0 mL sample of 1.0 M HCl in a polystyrene container. The temperature of
ElenaW [278]

Answer:

The experimental value of ΔH is -50 kJ/mol

Explanation:

<u>Step 1: </u>Data given

Volume of 1.0 M NaOH = 10.0 mL = 0.01 L

Volume of 1.0 M HCl = 10.0 mL = 0.01 L

Temperature before mixing = 20 °C

Final temperature = 26 °C

Specific heat of solution = 4.2 J/g°C

Density = 1g/mL

<u>Step 2: </u>Calculate q

q = m*c*ΔT

⇒ with m = the mass

  ⇒ 20.0 mL * 1g/mL = 20 grams

⇒  c = specific heat of solution = 4.2 J/g°C

⇒ ΔT = T2 -T1 = 26 -20 = 6 °C

q = 20g * 4.2 J/g°C * 6°C

q = 504 J

ΔHrxn = -q  ( because it's an exothermic reaction)

ΔHrxn = -504 J

<u>Step 3:</u> Calculate number of moles

Moles = Molarity * volume

Moles = 1M *0.01 L = 0.01 moles

<u>Step 4:</u> Calculate the experimental value of ΔH

ΔHrxn = -504 / 0.01 mol = -50400 J/mol = -50.4 kJ/mol

The experimental value of ΔH is -50 kJ/mol

6 0
3 years ago
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