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How many $\mathrm{mL}$ of solution will result when $15.0~\mathrm{g}$ of $\ce{H2SO4}$ is dissolved to make a $0.200~\mathrm{M}$ solution?

Here's what I have so far:

First, I converted $15~\mathrm{g}$ of $\ce{H2SO4}$ to moles using a conversion factor. I calculated that it would be $0.15~\mathrm{mol}$. Second, I just plugged in the numbers.

\begin{aligned} 0.200~\mathrm{M} &= 0.15~\mathrm{mol} / (x)\\ (0.15)(0.200) &= x\\ 0.03~\mathrm{L} &= x\\ 0.03~\mathrm{L} &= 30~\mathrm{mL}\end{aligned} Is this wrong?

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$$ (0.15)(0.200)= x $$

should be $(0.15) / (0.200)= x$

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\begin{aligned} (15/98) &= 0.200\cdot x\\ \text{Moles} &= \text{molarity}\times\text{volume}\\ x &=0.765~\mathrm{L}=765~\mathrm{mL}\\ \end{aligned}

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