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Hatshy [7]
2 years ago
11

What is the pressure of 1.27 L of a gas at 288°C, if the gas had a volume of 875 ml at

Chemistry
1 answer:
lyudmila [28]2 years ago
3 0

The pressure of 1.27 L of a gas at 288°C, if the gas had a volume of 875 ml at 145 kPa and 176°C is 1.195 atm.

<h3>What is ideal gas equation?</h3>

Ideal gas equation of any gas will be represented as:
PV = nRT, where

P = pressure

V = volume

n = moles

R = universal gas constant

T = temperature

First we calculate the moles of gas, when the volume of gas 875 ml at

145 kPa and 176°C as:

n = (1.431atm)(0.875L) / (0.082L.atm/K.mol)(449.15K)

n = 1.252 / 36.83 = 0.033 moles

Now we measure the pressure of 0.033 moles of gas of 1.27 L of a gas at 288°C as:

P = (0.033mol)(0.082L.atm/K.mol)(561K) / (1.27L) = 1.195 atm

Hence required pressure of gas is 1.195 atm.

To know more about ideal gas equation, visit the below link:
brainly.com/question/555495

#SPJ1

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Answer:

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Explanation:

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2 cytoplasmic NADH formed in glycolysis         Each yields 2 ATP   +4

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2 FADH2 formed in the citric acid cycle         Each yields 2 ATP         +4

6 NADH formed in the citric acid cycle             Each yields 3 ATP         +18

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2 cytoplasmic FADH2 formed in glycolysis          Each yields 2 ATP            +4

2 FADH2 formed in the oxidation of pyruvate   Each yields 3 ATP    +4

2 FADH2 formed in the citric acid cycle            Each yields 2 ATP    +4

6 FADH2 formed in the citric acid cycle                  Each yields 2 ATP   +12

2 ATP from glycolysis                                                                                    

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2 ATP from citric acid cycle                                                                            +2

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C6H12O6 + 6 CO2 + 28ADP + 28 Pi ⇒6 CO2 + 6 H2O + 28 ATP

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