Please EXPLAIN and solve EACH/ALL part(s) in Question #6!

DOUBLE CHECK YOUR WORK AND ANSWER(S).

PLEASE NEATLY SHOW ALL WORK, EXPLANATIONS, & CALCULATIONS STEP-BY-STEP USING PEN AND PAPER! I AM NEW TO CHEMISTRY! I AM A COMPLETE NEWBIE!

6A. Write out the first-order integrated rate equation as an equation for a straight line (with the general form y=mx+b ). 6B. As our first-order reaction (Figure 2) proceeds, does the reaction rate change as [A] changes? Type your answer here. 6C. The decomposition of N2O5 in CCl4 is a first-order reaction. If 2.56mg of N2O5 is present initially and 2.50mg is present after 4.26 minutes at 55C, what is the value of the rate constant? Hint: Because the first-order integrated rate equation depends on the ratio of the final versus initial concentration, we can simply use a mole ratio or mass ratio in place of a ratio of concentrations. Figure 2. Plot of natural logarithm of concentration versus time for a first-order Insert your work image here. reaction