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ale4655 [162]
3 years ago
9

An ideal gas is allowed to expand from 5.40 L to 35.1 L at constant temperature. By what factor does the volume increase?

Chemistry
1 answer:
horrorfan [7]3 years ago
6 0

Answer:

a) 6.5

b) pressure decreases

c)22 atm

Explanation:

Since the initial volume V1 is 5.40 L and the final volume V2 is 35.1 L, the ratio of V2:V1= 35.1/5.40= 6.5 hence the volume increases by a factor of 6.5.

When the volume increases, the pressure decreases accordingly in accordance with Boyle's law. Boyle's law states that the volume of a given mass of gas is inversely proportional to its pressure at constant temperature.

c) From Boyle's law

Initial volume V1= 5.40 L

Final volume V2= 35.1 L

Initial pressure P1= 143 ATM

Final pressure P2 = the unknown

P1V1= P2V2

P2= P1V1/V2

P2 = 143 × 5.40/ 35.1

P2= 22 atm

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Svetllana [295]

Answer:

Number of moles = 10.6 mol

Explanation:

Given data:

Molar mass of H = 1.008 g/mol

Molar mass of C = 12.01 g/mol

Molar mass of O = 16.00 g/mol

Mass of citric acid = 2.03 kg (2.03×1000 = 2030 g)

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Formula:

Number of moles = mass/molar mass

Now we will calculate the molar mass of citric acid:

C₆H₈O₇ = (12.01× 6) + (1.008×8) + (16.00×7)

C₆H₈O₇ = 72.06 + 8.064+112

C₆H₈O₇ = 192.124g/mol

Number of moles = 2030 g/ 192.124g/mol

Number of moles = 10.6 mol

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the reversible reaction N2(g) 3H2(g) <--> 2NH3(g) produces ammonia, which is a fertilizer. At equilibrium, a 1L flask cont
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