An unknown compound, B, has the molecular formula C7H12. On catalytic hydrogenation 1 mol of B absorbs 2 mol of hydrogen and yie

The new pressure of the gas is calculated to be 40.7 kPa. Using the principle that P1 • V1 = P2 • V2, we can set 98.8 kPa (P1) multiplied by 21.7 mL (V1) equal to P2 (unknown pressure) multiplied by 52.7 mL (V2). To isolate P2, we rearrange the equation to P2 = (98.8 kPa • 21.7 mL) / 52.7 mL, resulting in P2 equal to 40.7 kPa.

Response: The rate constant at 525 K is,

Rationale:

Based on the Arrhenius equation,

or,

where,

= rate constant when =

= rate constant when =?

= activation energy for the process =

R = gas constant = 8.314 J/mole.K

= initial temperature = 701 K

= final temperature = 525 K

Substituting the provided values into this formula yields:

Thus, the rate constant at 525 K is,

The reaction that exhibits the lowest K value is: A + B → 2 C; E°cell = -0.030 V. This can be rationalized by noting that the standard electrode potential of the cell is directly proportional to the reaction's equilibrium constant. A higher potential results in a larger K value, whereas a lower potential yields a smaller K value.

The question is incomplete,the complete question:

Determine the molality of a 10.0% (by weight) solution of hydrochloric acid in water:

a) 0.274 m

b) 2.74 m

c) 3.05 m

d) 4.33 m

e) the solution's density is necessary for calculations

Answer:

The molality for a 10.0% (by weight) hydrochloric acid solution is 3.05 mol/kg.

Explanation:

The solution is a 10.0% (by weight) hydrochloric acid mix.

This means there are 10 grams of HCl in 100 grams of the solution.

Amount of HCl = 10 g

Total mass of solution = 100 g

Total mass of solution = Mass of solute + Mass of solvent

Mass of solvent (water) = 100 g - 10 g = 90 g

Calculate moles of HCl =

Mass of water converted to kilograms = 0.090 kg

Molality =

<strongTherefore, the molality of a 10.0% (by weight) hydrochloric acid solution is 3.05 mol/kg.