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3. Chemical Reactions
Stoichiometry
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Ammonium nitrate (NH4NO3), a common fertilizer, is 35.0% nitrogen by mass. How much ammonium nitrate contains 1.25 kg of nitrogen?
A
3.57 kg
B
437 g
C
15.6 kg
D
230 kg
Verified step by step guidance1
First, understand that the problem is asking for the mass of ammonium nitrate (NH4NO3) that contains a specific mass of nitrogen, given that ammonium nitrate is 35.0% nitrogen by mass.
To find the mass of ammonium nitrate, use the percentage composition formula: \( \text{mass of nitrogen} = \text{mass of ammonium nitrate} \times \frac{\text{percentage of nitrogen}}{100} \).
Rearrange the formula to solve for the mass of ammonium nitrate: \( \text{mass of ammonium nitrate} = \frac{\text{mass of nitrogen}}{\frac{\text{percentage of nitrogen}}{100}} \).
Substitute the given values into the equation: \( \text{mass of ammonium nitrate} = \frac{1.25 \text{ kg}}{0.35} \).
Calculate the result to find the mass of ammonium nitrate that contains 1.25 kg of nitrogen.
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