The balanced chemical reaction is written as:
<span>Zn + 2AgNO3 = Zn(NO3)2 + 2Ag
To determine the grams of silver metal that is being produced, it is important to first determine which is the limiting reactant and the excess reactant from the given initial amounts. We do as follows:
4.35 g Zn ( 1 mol / 65.38 g ) ( 2 mol AgNO3 / 1 mol Zn ) = 0.1331 mol AgNO3 needed
35.8 g AgNO3 ( 1 mol / 169.87 g ) ( 1 mol Zn / 2 mol AgNO3 ) = 0.1054 mol Zn needed
Therefore, the limiting reactant would be the zinc metal since it would be consumed completely in the reaction. The excess amount of AgNO3 would be:
0.2107 mol AgNO3 - 0.1331 mol AgNO3 = 0.0776 mol AgNO3 left ( 169.87 g / 1 mol ) = 13.19 g AgNO3 left
0.0665 mol Zn ( 2 mol Ag / 1 mol Zn) ( 107.9 g / 1 mol) = 14.3581 g Ag produced</span>
Answer:
The volume is 2238,6 L
Explanation:
We use the formula PV=nRT. The conditions STP are: 1 atm of pressure and 273K of temperature:
PV=nRT ---> V=(nRT)/P
V= 100 mol x 0,082 l atm/K mol x 273K/ 1 atm
<em>V=2238, 6L</em>
Explanation:
( a )
The decomposition reaction of KClO₃ to form diatomic oxygen gas is the following way -
2 KClO₃ ( s ) -------> 2 KCl ( s ) + 3O₂ ( g )
( b )
The reaction of solid metal of Aluminum with Iodine in the following way -
2 Al ( s ) + 3 I₂ ( s ) ------> Al₂I₆ ( s )
( c )
The reaction of sodium chloride with aqueous sulfuric acid is as follow -
2 NaCl ( s ) + H₂SO₄ ( aq ) ------> 2 HCl ( g ) + Na₂SO₄ ( aq )
( d )
The reaction of phosphoric acid with potassium hydroxide , in the following way -
H₃PO₄ ( aq ) + KOH ( aq ) ------> KH₂PO₄ ( aq ) + H₂O ( l )
Answer:
it looks like deoxyribose...im not sure tho
Explanatio
