Solving for mass of a solute given ppm and volume?

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To find the mass of oxygen in a solution with 23 ppm and a volume of 242.0066 mL, the formula for ppm can be applied: ppm = (grams of solute / grams of solution) * 1,000,000. The challenge arises from the lack of information about the density of the solution, which is necessary to convert volume to mass. Without knowing the density, it's impossible to determine the mass of the solution and subsequently the mass of the solute. Clarification on the solution's density or additional context is needed to solve the problem accurately. Accurate calculations require both the ppm value and the mass of the solution.
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The question is: A solution contains 23ppm of dissolved O2 in 242.0066 mL of solution. What is the mass of the oxygen.

Formula: ppm=(grams of solute/grams of solution)*1,000,000

I tried plugging stuff in but it wasn't working out what so ever.

I just don't know how to do these when given so little information. Thanks in advance if you can help.
 
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The solution is NOT water.
 
Formula calls for the mass of the solution. You are give volume. You either have enough information to do the conversion, or not - hard to say not knowing the context.
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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