If the rate constant of a reaction is 0.010 L/mols at 30 °C, calculate the rate constant at 100 °C assuming the rate doubles for each 10 °C rise in temperature. It says that the answer is 1.3 L/mols, but I don't understand why.

1.3L/mols

Explanation:

At 30°C the rate constant is 0.010L/mols

As the rate doubles for each 10° rise in temperature:

At 40°:

0.010L/mols*2 = 0.020L/mols

At 50°C:

0.020L/mols*2 = 0.040L/mols

At 60°C:

0.040L/mols*2 = 0.080L/mols

At 70°C:

0.080L/mols*2 = 0.160L/mols

At 80°C:

0.160L/mols*2 = 0.320L/mols

At 90°C:

0.320L/mols*2 = 0.640L/mols

And at 100°C:

0.640L/mols*2 =

1.280L/mols ≅

hey there!

boiling point is the temperature at which the vapor pressure of the liquid equals atmospheric pressure. the vapor pressure of solvent molecules is decreased when a solute is added, so a higher temperature is required to increase the number of solvent molecules in the gas phase above the liquid.

at the freezing point, the vapor pressures of the solid and liquid are equal; a lower temperature is needed to reduce the number of solvent particles above the liquid.

hope this you

tobey