Answer:
a. V = 1000 mL
b. Denisty = 0.022 g/mL
Explanation:
a.
First we need to convert the volume of the Osmium into mL. For that purpose we are given the conversion unit as:
1 mL = 0.1 cL
Hence, the given volume of Osmium will be:
V = Volume of Osmium = 100 cL = (100 cL)(1 mL/0.1 cL) = 1000 mL
<u>V = 1000 mL</u>
b.
The density of Osmium is given by the following formula:
Density = mass/Volume
Denisty = 22 g/1000 mL
<u>Denisty = 0.022 g/mL</u>
A: Trial 1, because the average rate of the reaction is lower.
The rate of reaction is the speed with which reactants are converted into products. It is also the rate at which reactants disappear and products appear. The higher the rate of reaction, the greater the amount of product formed in a reaction.
If we look at the graph, we will realize that trial 1 produces a lesser amount of product than trial 2. This implies that the average rate of the reaction in trial 1 is lower than in trial 2.
Lower average rate of reaction implies lower concentration of the reactants since the rate of reaction depends on the concentration of reactants.
Hence trial 1 has a lower concentration of reactants because the average rate of the reaction is lower.
Molecular weight of (NH4)2 CO3 = 96 gm. 96 gm (NH4)2CO3 = 1 mol of (NH4)2CO3 = 2 moles of NH4.
Therefore 1.3 gm of (NH4)2CO3 = 1.3x2/ 96 = 0.027 moles.
Answer:
Percentage yield = 75.03%
Explanation:
Actual yield = 6.13
Theoretical yield = 8.17g
Percentage yield = ?
Percentage yield of compound in a reaction is the percentage ratio of actual yield to theoretical yield of that compound
Percentage yield = (actual yield / theoretical yield) * 100
Percentage yield = (6.13/8.17) * 100
Percentage yield = 0.7503 * 100
Percentage yield = 75.03%
Percentage yield of water in the reaction is 75.03%
