A4.00 l flexible container holds a sample of hydrogen gas at 7 atm if the pressure increases to 6 atm and the temperature remains constant what will the volume be. a. 4.67l b. 3.42l c. 0.22l d. 5.26l will mark as

Boyles law states that at constant temperature the pressure of gases are inversely proportional to volume of gases.

PV = k

where P - pressure , V - volume and k - constant

P1V1 = P2V2

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

substituting the values in the equation

7 atm x 4.00 L = 6 atm x V

V = 4.67 L

new volume is A. 4.67 L

i think it is true since you can test the answer and can use observations to complete it.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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