The answer is (2). To calculate the density, you need to divide the mass with volume. When doing division, the significant figures of result is the minimal of the numbers using before. So the answer is 2.
Explanation:
Since this is an equilibrium problem, we apply le chatelier principle. This principle states that whenever a system at equilibrium is disturbed due to change in several factors, it would move in a way to annul such change.
C2H4(g) + Cl2 ⇔ 2C2H4Cl2(g)
When the concentration of C2H4 is increased, there is more reactant sin the system. In order to annul this change, the equilibrium position will shift to the right favoring product formation.
When the concentration of C2H4Cl2 is increased, there is more product in the system. To annul this change, the equilibrium position will shift to the left, favoring reactant formation.
Answer:
(1) The sample should not be large, because a large sample would produce a higher and broader mp range.
(2) The rate of heating does not matter.
Explanation:
(1) The sample should not be large, because a large sample would produce a higher and broader mp range, because varying temperature range across the body will lead to inaccurate determination of melting point.
(2) In principle, the melting temperature is INDEPENDENT (not dependent) on the heating rate. so in other words, altering the heating rate does not affect the measure of melting point.
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The partial pressure of oxygen, P(O₂) is 198.83 mmHg.
<h3>What is partial pressure of a gas?</h3>
The partial pressure of a gas is the pressure gas will exert in a mixture of gases which do not react chemically together.
The sum of partial pressure of gases at atmospheric pressure = 760 mmHg
P(N₂) + P(H₂O) + P(CO₂) + P(O₂) + P(other) = 760 mmHg
P(N₂) = 0.72 atm = 547.2 mmHg
P(H₂O) = 7.7 torr = 7.7 mmHg
P(CO₂) = 0.37 mmHg
P(other) = 0.97 kPa = 5.9 mmHg
P(O₂) = 760 - (547.2 + 7.7 + 0.37 + 5.9) = 198.83 mmHg
Therefore, the partial pressure of oxygen, P(O₂) is 198.83 mmHg.
Learn more partial pressure at: brainly.com/question/14119417
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