Finding rate of reaction from a concentration vs. time graph
Let the reactant be $S$ and the product be $P$.  Let $p$ be the dimenionless product concentration, $\frac{P}{S_0}$.  First order kinetics:


$$\frac{P}{S_0} = p = 1- e^{-k t}$$


Slope of first-order kinetics:


$$\frac{dp}{dt} = k e ^{-kt}$$


Slopes and angles.  One confusing thing about this problem is the definition of $\theta$ is different than what you usually see in math class.  It's the angle with respect to the $y$ axis, not the $x$ axis.  As you note, if the $y$ angle is 30 degrees, then the $x$ angle is 60 degrees, meaning the slope is $\tan~60^{\circ} = \sqrt{3}$.  
Units problem.  However there is a big units problem in this question.  The slope is $\sqrt{3}$ what?  Gigamolar per nanosecond?  Zeptomolar per eon?  The angle of the tangent curve will change depending on the units used to plot the data.  If you use nanoseconds as the time unit, the angle of the tangent curve will be very flat, but conversely if eons is the time unit, the the angle will be very sharp.  The question does not explicitly say what units are used in the plot.  And the expression for the derivative of a first-order reaction shows that the slope should have units of concentration per time, but $\sqrt{3}$ is dimensionless.  So there is not really enough information to solve the problem.
Dicey assumptions about units.  Let's assume that the time unit is minutes.  Let's further assume that the $y$ axis plots a dimensionless concentration, i.e., $p$. Then the derivative (slope) is $-k e^{-k t}$ and apparently has a value of $\sqrt{3}~\mathbf{{min}^{-1}}$.


The question is asking for the rate, so you are done.  But there are a lot of weird assumptions in this problem.