객관식
Given the balanced equation N2(g) + 3 H2(g) → 2 NH3(g), what is the rate of reaction with respect to [NH3] if the rate of disappearance of H2 is 0.6 mol/L·s?
1026
views
3. Chemical Reactions
Stoichiometry
객관식
How many grams of Li3N can be formed from 1.75 moles of Li based on the following balanced chemical equation of the reaction? Assume an excess of nitrogen. 6 Li(s) + N2(g) → 2 Li3N(s)
A
20.3 grams
B
58.3 grams
C
29.2 grams
D
116.6 grams
검증된 단계별 안내1
Identify the balanced chemical equation: 6 Li(s) + N2(g) → 2 Li3N(s). This equation tells us that 6 moles of lithium react with 1 mole of nitrogen gas to produce 2 moles of lithium nitride.
Determine the mole ratio between lithium and lithium nitride from the balanced equation. The ratio is 6 moles of Li to 2 moles of Li3N, which simplifies to 3 moles of Li to 1 mole of Li3N.
Calculate the moles of Li3N that can be formed from 1.75 moles of Li using the mole ratio. Use the formula: \( \text{moles of Li3N} = \frac{1.75 \text{ moles Li}}{3} \).
Convert the moles of Li3N to grams. First, calculate the molar mass of Li3N by adding the atomic masses of 3 lithium atoms and 1 nitrogen atom. Use the formula: \( \text{grams of Li3N} = \text{moles of Li3N} \times \text{molar mass of Li3N} \).
Perform the multiplication to find the mass of Li3N that can be formed. This will give you the final answer in grams.
관련 영상
관련 실천
