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pantera1 [17]
2 years ago
7

Which compounds were classified as organic compounds according to the early chemists

Chemistry
1 answer:
Temka [501]2 years ago
4 0

Answer:

hope it's help you ok have a good day

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What explanation accounts for the observation that the mass of the products in reaction #1 (open system) were not equal?
Anna007 [38]

Answer:

The law of conservation of mass states that matter can not be created or destroyed in a chemical reaction.

Explanation:

5 0
2 years ago
Consider two equal-volume flasks of gas at the same temperature and pressure. One gas, oxygen, has a molecular mass of 32. The o
san4es73 [151]

Answer: The ratio of the number of oxygen molecules to the number of nitrogen molecules in these flasks is 1: 1

Explanation:

According to avogadro's law, equal volumes of all gases at same temperature and pressure have equal number of moles.

According to avogadro's law, 1 mole of every substance contains avogadro's number 6.023\times 10^{23} of particles.

Thus as oxygen and nitrogen are at same temperature and pressure and are in equal volume flasks , they have same number of moles and thus have same number of molecules.

The ratio of the number of oxygen molecules to the number of nitrogen molecules in these flasks is 1: 1

3 0
2 years ago
How many milliliters of a 0.211 M HI solution are needed to reduce 24.0 mL of a 0.354 M KMnO4 solution according to the followin
Novay_Z [31]

Answer:

The answer to your question is 242 ml

Explanation:

Data

HI 0.211 M   Volume = x

KMnO₄ 0.354 M   Volume = 24 ml

Balanced Chemical reaction

     12HI + 2KMnO₄ + 2H₂SO₄ → 6I₂ + Mn₂SO₄ + K₂SO₄ + 8H₂O

Process

1.- Calculate the moles of KMnO₄  0.354 M in 24 ml

Molarity = moles / volume (L)

moles = Molarity x volume (L)

moles = 0.354 x 0.024

moles = 0.0085

2.- From the balanced chemical reaction we know that HI and KMnO₄ react in the proportion 12 to 2. Then,

              12 moles of HI --------------- 2 moles of KMnO₄

                x                     --------------- 0.0085 moles of KMnO₄

             x = (0.0085 x 12)/2

             x = 0.051 moles of HI

3.- Calculate the milliliters of HI 0.211 M

Molarity = moles/volume

Volume = moles/molarity

Volume = 0.051/0.211

Volume = 0.242 L or Volume = 242 ml

8 0
3 years ago
A gas at STP occupies 22.4 L if the temperature is changed to 260 K and the pressures changed it to 0.50 ATM what will the new v
asambeis [7]

Answer:

The new volume will be 42, 7 L.

Explanation:

We use the gas formula, which results from the combination of the Boyle, Charles and Gay-Lussac laws. According to which at a constant mass, temperature, pressure and volume vary, keeping constant PV / T. The conditions STP are: 1 atm of pressure and 273 K of temperature.

P1xV1/T1 =P2xV2/T2

1 atmx 22,4 L/273K = 0,5atmx V2/260K

V2=((1 atmx 22,4 L/273K )x 260K)/0,5 atm= 42, 67L

3 0
3 years ago
A sample of helium gas has a pressure of 1.20 atm at 22°c. at what celsius temperature will the helium reach a pressure of 2.00
sukhopar [10]
Gay-Lussac's law gives the relationship between pressure and temperature of a gas.
it states that for a fixed amount of gas of constant volume pressure is directly proportional to temperature. 
P/T = k
where P - pressure, T - temperature and k - constant 
\frac{P1}{T1} =  \frac{P2}{T2}
where parameters for the first instance are on the left side and parameters for the second instance are on the right side of the equation.
temperature should be in the kelvin scale,
T1 = 22 °C + 273 = 295 K
substituting the values in the equation 
\frac{1.20atm}{295 K}  =  \frac{2.00 atm}{T}
T = 492 K
new temperature - 492 - 273 = 219 °C
5 0
3 years ago
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