The percent yield of this reaction is calculated as follows
Mg3N2 + 3H2O =2NH3 + 3Mgo
calculate the theoretical yield,
moles=mass/molar mass
moles Mg3N2= 3.82 g/100g/mol= 0.0382 moles(limiting regent)
moles of H2o= 7.73g/18g/mol = 0.429 moles ( in excess_)
by use of mole ratio between Mg3N2 to MgO which is 1:3 the moles of MgO = 0.0382 x3 = 0.1146 moles
mass =moles x molar mass
the theoretical mass is therefore = 0.1146mole x 40 g/mol = 4.58 grams
The % yield = actual mass/theoretical mass x1000
= 3.60/4.584 x100= 78.5%
Equation is as follow,
<span> SnCl</span>₂ <span> + PbCl</span>₄<span> </span>→ <span>SnCl</span>₄ <span> + PbCl</span>₂
Oxidation State of Sn on left hand side in SnCl₂ is +2, while that in SnCl₄ on right hand side is +4. Means Sn has lost two electrons. Hence, it is oxidized and has worked as a reducing agent (has reduced Pb from Pb⁺⁴ to Pb⁺²).
Oxidation State of Pb on left hand side in PbCl₄ is +4, while that in PbCl₂ on right hand side is +2. Means Pb has gained two electrons. Hence, it is reduced and has worked as an oxidizing agent (has oxidized Sn from Sn⁺² to Sn⁺⁴).
Four grams of calcium must be combined with phosphorus to form one mole of the compound Ca3P2
I think the answer is A but I’m not completely sure
Answer:
Sn(s) + MgBr2(aq) --> SnBr2(aq) + Mg(s)
Explanation:
<em>Decide whether a chemical reaction happens in either of the following situations. </em>
- A reaction happens. The type of this reaction is the single replacement reaction.
<em>If a reaction does happen, write the chemical equation for it.</em>
Sn(s) + MgBr2(aq) --> SnBr2(aq) + Mg(s)