Use the value of the activation energy (Ea=1.50×102kJ/mol) and the given rate constant of the reaction at either of the two temperatures to predict the rate constant at 551 K.

The rate constant

K= 0.967m-1s-1

Explanation: To calculate the rate constant, we will use the Arrhenius equation.

lnK = (- Ea/R) (1/T) + lnZ(1)

K is the rate constant

Ea is the activation energy

R is the gas constant

T is the temperature in Kelvin

Z is the constant related to the geometry needed, but in this question Z is equal to zero.

Therefore fro data given, we have

Ea = 1.50 × 102kj/mol = 153kj/mol

R = 8.314j/mol-k

T = 551k

Z= 0

Therefore using the equation

lnK = -153÷ (8.314 × 551) = -153 × 4581.014

lnK = - 0.033398719

Taking the ln inverse of K

K = e^ (-0.033398819) = 0.96715286

K= 0.967m-1s-1

This is the rate constant

answer: the rate of diffusion increases with increase in temperature.

increase in temperature, increases the molecular/particles speed (kinetic energy. diffusion means movement of particles through the material.

generally, the heavier the particle the more it interacts with the environment and more the temperature matters. so higher temperature results in higher diffusion.

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"