Answer: There are 3.2 moles of gas if you have a volume of 38.0 L under a pressure of 1430 mmHg at standard temperature.
Explanation:
Given: Volume = 38.0 L
Pressure = 1430 mm Hg (1 mm Hg = 0.00131579 atm) = 1.9 atm
Temperature = 273.15 K
Using ideal gas equation, the moles of gas will be calculated as follows.
where,
P = pressure
V = volume
n = no. of moles
R = gas constant = 0.0821 L atm/mol K
T =temperature
Substitute the values into above formula as follows.
Thus, we can conclude that there are 3.2 moles of gas if you have a volume of 38.0 L under a pressure of 1430 mmHg at standard temperature.
Answer:
Advanced Pharmaceutics Inc
Explanation:
Advanced Pharmaceutics Inc
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Answer:
Option-B (2-methylpropene)
Explanation:
The reaction scheme is attached below,
In first step the alkene acts a nucleophile and adds H⁺ across double bond yielding a stable tertiary carbocation.
In the second step the oxygen atom of methanol acts as nucleophile and attacks the positive charge carrying carbon atom resulting in the formation of t-butyl methyl ether.
B parts eroded by wind or water
Answer:
The final pressure is 173 kPa.
Explanation:
A mixture of gases at an initial pressure of P₁ = 101 kPa is compressed from an initial volume V₁ = 7.20 dm³ to a final volume V₂ = 4.21 dm³. If we suppose an ideal gas behavior and that temperature remains constant, we can apply Boyle's law to find out the final pressure P₂:
P₁ . V₁ = P₂ . V₂
