Answer:
if it cannot be made to fit the new findings
Its very hard to answer all of these questions
Th actual yield of the reaction is 24.86 g
We'll begin by calculating the theoretical yield of the reaction.
2Na + Cl₂ → 2NaCl
Molar mass of Na = 23 g/mol
Mass of Na from the balanced equation = 2 × 23 = 46 g
Molar mass of NaCl = 23 + 35.5 = 58.5 g/mol
Mass of NaCl from the balanced = 2 × 58.5 = 117 g
From the balanced equation above,
46 g of Na reacted to produce 117 g of NaCl.
Therefore,
11.5 g of Na will react to produce = (11.5 × 117) / 46 = 29.25 g of NaCl.
Thus, the theoretical yield of NaCl is 29.25 g.
Finally, we shall determine the actual yield of NaCl.
- Theoretical yield = 29.25 g
Actual yield = Percent yield × Theoretical yield
Actual yield = 85% × 29.25
Actual yield = 0.85 × 29.25 g
Actual yield = 24.86 g
Learn more about stoichiometry: brainly.com/question/25899385
Answer:
9.8 L
Explanation:
The reaction that takes place is:
- 4H₂(g) + CS₂(g) → CH₄(g)+ 2H₂S(g)
At STP, 1 mol of any gas occupies 22.4 L.
We <u>calculate how many moles are there in 2.5 L of CH₄ at STP</u>:
- 2.5 L ÷ 22.4 L/mol = 0.11 mol CH₄
Then we <u>convert CH₄ moles into H₂ moles</u>, using the<em> stoichiometric coefficients of the reaction</em>:
- 0.11 mol CH₄ *
= 0.44 mol H₂
Finally we <u>calculate the volume that 0.44 moles of H₂ would occupy at STP</u>:
- 0.44 mol * 22.4 L/mol = 9.8 L
