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What type of reaction is 2NH3+H2SO4 right arrow (NH4)SO4

3 answers

The reaction you provided:

\[ 2 \text{NH}_3 + \text{H}_2\text{SO}_4 \rightarrow (\text{NH}_4)_2\text{SO}_4 \]

is a type of acid-base neutralization reaction. In this reaction, ammonia (NH₃), which acts as a base, reacts with sulfuric acid (H₂SO₄), serving as an acid, to form ammonium sulfate ((NH₄)₂SO₄).

In essence, NH₃ accepts protons (H⁺ ions) from H₂SO₄, leading to the formation of the ammonium ion (NH₄⁺), resulting in the salt ammonium sulfate.

2.7g of a gaseous hydrcarbon, which contains 11.1% of hydrogen occupies a volume of 1.12dm3 at s.t.p. what is the percentage composition of carbon in the compound

To find the percentage composition of carbon in the gaseous hydrocarbon, we can follow these steps:

  1. Determine the moles of the gas using the ideal gas law: At standard temperature and pressure (s.t.p), 1 mole of gas occupies 22.4 dm³.

  2. Find the number of moles of the gaseous hydrocarbon: \[ \text{Moles of gas} = \frac{\text{Volume}}{\text{Molar volume at s.t.p}} = \frac{1.12 , \text{dm}^3}{22.4 , \text{dm}^3/\text{mol}} \approx 0.05 , \text{mol} \]

  3. Determine the mass of hydrogen in the compound:

    • Given that the compound is 11.1% hydrogen by mass: \[ \text{Mass of hydrogen} = 0.111 \times 2.7 , \text{g} \approx 0.2997 , \text{g} \]

  4. Calculate the number of moles of hydrogen:

    • The molar mass of hydrogen (H) is approximately 1 g/mol: \[ \text{Moles of H} = \frac{0.2997 , \text{g}}{1 , \text{g/mol}} \approx 0.2997 , \text{mol} \]

  5. Calculate the number of moles of carbon in the compound:

    • The total mass of the hydrocarbon is 2.7 g, so the mass of carbon (C) can be found by subtracting the mass of hydrogen: \[ \text{Mass of carbon} = \text{Total mass} - \text{Mass of hydrogen} = 2.7 , \text{g} - 0.2997 , \text{g} \approx 2.4003 , \text{g} \]

  6. Calculate the number of moles of carbon:

    • The molar mass of carbon is approximately 12 g/mol: \[ \text{Moles of C} = \frac{2.4003 , \text{g}}{12 , \text{g/mol}} \approx 0.2000 , \text{mol} \]

  7. Calculate the percentage composition of carbon: \[ \text{Percentage of C} = \left( \frac{\text{Mass of carbon}}{\text{Total mass}} \right) \times 100 = \left( \frac{2.4003 , \text{g}}{2.7 , \text{g}} \right) \times 100 \approx 88.89% \]

Thus, the percentage composition of carbon in the compound is approximately 88.89%.