A reactant $\ce{X}$ is converted into products $\ce{Y}$ and $\ce{Z}$ according to the following first order parallel reactions:
$\ce{X->[k_1]Y}$
$\ce{X->[k_2]Z}$
$\ce{[X]}$ has decreased from $\pu{1.00 M}$ at $t = 0$ to $\pu{0.549 M}$ after $\pu{10 min}$. Calculate the rate constants $k_1$ and $k_2$, knowing that the yields of $\ce{Y}$ and $\ce{Z}$ obtained are $25.0$ and $\pu{75.0 mol\%}$, respectively.
So far, I have the ratio between $k_1$ and $k_2$ $=0.33$, which I found from the yield ratio but I'm unsure what to do with this ratio.
I also have derived the equation $[A] = [A]_0 \cdot e^{-(k_1+ k_2)t}$