The answer is h the reaction produces a lot of thermal energy
Answer:
63.02 g.
Explanation:
- Na reacts with Cl₂ according to the balanced equation:
<em>2Na + Cl₂ → 2NaCl,</em>
It is clear that 2 mole of Na react with 1 mole of Cl₂ to produce 2 moles of NaCl.
- Firstly, we need to calculate the no. of moles of Na and Cl₂:
no. of moles of Na = (mass/atomic mass) = (19.0 g/22.9897 g/mol) = 0.826 g.
no. of moles of Cl₂ = (mass/atomic mass) = (34.0 g/70.906 g/mol) = 0.48 g.
- From the stichiometry, Na reacts with Cl₂ with a molar ratio (2:1).
<em>So, 0.826 mol of Na "the limiting reactant" reacts completely with 0.413 mol of Cl₂ "left over reactant".</em>
The no. of moles of Cl₂ remained after the reaction = 0.48 mol - 0.413 mol = 0.067 mol.
∴ The mass of Cl₂ remained after the reaction = (no. of moles of Cl₂ remained after the reaction)(molar mass of Cl₂) = (0.067 mol)(70.906 g/mol) = 4.75 g.
- To get the no. of grams of produced NaCl:
<u><em>using cross multiplication:</em></u>
2 mol of Na produce → 2 mol of NaCl, from the stichiometry.
∴ 0.826 mol of Na produce → 0.826 mol of NaCl.
∴ The mass of NaCl produced after the reaction = (no. of moles of NaCl)(molar mass of NaCl) = (0.826 mol)(58.44 g/mol) = 48.27 g.
∴ The total weight of the glass vial containing the final product = the weight of the glass vial + the weight of the remaining Cl₂ + the weight of the produced NaCl = 10.0 g + 4.75 g + 48.27 g = 63.02 g.
Answer:
Explanation:
For part C, this should be what the graph looks like.
The reactants should have higher energy that the products so that it can release energy. Recall the reaction is N2 + 3H2 => 2NH3 + energy, making it exothermic. Apparently, you are supposed to adjust the energy diagram on the simulation so that 20% of the reactants become the products.
The answer is “H2O2” .....
Answer:
50 mol CH₄
Explanation:
The question is incomplete so I looked it up online.
<em>How many moles CH₄, are needed to produce 50 moles of CO₂?</em>
Step 1: Write the balanced equation for the complete combustion of methane
CH₄ + 2 O₂ ⇒ CO₂ + 2 H₂O
Step 2: Establish the appropriate molar ratio
According to the balanced equation, the molar ratio of CH₄ to CO₂ is 1:1.
Step 3: Calculate the number of moles of CH₄ needed to produce 50 moles of CO₂
We will use the previously established molar ratio.
50 mol CO₂ × 1 mol CH₄/1 mol CO₂ = 50 mol CH₄
