Answer:
c
Explanation:
there are billions of cells in living things. We are made out of millions of cells
Answer:
1. The actual amount of product that is produced from a given amount of reactant or reactants. → actual yield
2. A law which states that in ordinary chemical reactions, the sum of the masses of the reactants always equals the sum of the masses of the products. → Conservation of Mass
3. The reactant that is not used up in a reaction that goes to completion
→ excess reactant
4. The reactant that limits how much product is produced in a reaction that goes to completion. It is used up in the reaction. → limiting reactant
5. The ratio of the actual yield to theoretical yield multiplied times 100.
→ percent yield
6. The maximum calculated amount of product produced from a given reactant in a reaction that goes to completion. → theoretical yield
7. The study of the quantitative relationships between reactants and products in a chemical reaction. → stoichiometry
Explanation:
1. The actual amount of product that is produced from a given amount of reactant or reactants. → actual yield
- The actual yield is the actual amount of product that is produced in a chemical reaction and it can be determined experimentally.
2. A law which states that in ordinary chemical reactions, the sum of the masses of the reactants always equals the sum of the masses of the products. → Conservation of Mass
- The law of conservation of mass states that mass in an isolated closed system is neither created nor destroyed by chemical reactions or physical transformations. According to the law of conservation of mass, the mass of the products in a chemical reaction must equal the mass of the reactants.
3. The reactant that is not used up in a reaction that goes to completion
→ excess reactant
- In any chemical reaction between two or more reactants, the excess reactant is the substance that is leftover when the chemical reaction is ended. The amount of product formed is not limited by this reagent.
4. The reactant that limits how much product is produced in a reaction that goes to completion. It is used up in the reaction. → limiting reactant
- In any chemical reaction between two or more reactants, the limiting reactant is the substance that is consumed completely when the chemical reaction is ended. The amount of product formed is limited by this reagent, since the reaction cannot continue without it.
5. The ratio of the actual yield to theoretical yield multiplied times 100.
→ percent yield
- percent yield = (actual yield / theoretical yield) *100
6. The maximum calculated amount of product produced from a given
reactant in a reaction that goes to completion.
→ theoretical yield
- theoretical yield is defined as the amount of the obtained desired product.
7. The study of the quantitative relationships between reactants and products in a chemical reaction.
→ Stoichiometry
- Stoichiometry is a branch of chemistry that deals with relationships between reactants and/or products in a reaction to determine desired quantitative data.
It will be extracted only 1/3 of NaCl less in 10 mL of water than in 30 mL of water.
If it is known that solubility of NaCl is 360 g/L, let's find out how many NaCl is in 30 mL of water:
360 g : 1 L = x g : 30 mL
Since 1 L = 1,000 mL, then:
360 g : 1,000 mL = <span>x g : 30 mL
Now, crossing the products:
x </span>· 1,000 mL = 360 g · 30 mL
x · 1,000 mL = 10,800 g mL
x = 10,800 g ÷ 1,000
x = 10.8 g
So, from 30 mL mixture, 10.8 g of NaCl could be extracted.
Let's calculate the same for 10 mL water instead of 30 mL.
360 g : 1 L = x g : 10 mL
Since 1 L = 1,000 mL, then:
360 g : 1,000 mL = <span>x g : 10 mL
Now, crossing the products:
x </span>· 1,000 mL = 360 g · 10 mL
x · 1,000 mL = 3,600 g mL
x = 3,600 g ÷ 1,000
<span>x = 3.6 g
</span>
<span>So, from 10 mL mixture, 3.6 g of NaCl could be extracted.
</span>
Now, let's compare:
If from 30 mL mixture, 10.8 g of NaCl could be extracted and <span>from 10 mL mixture, 3.6 g of NaCl could be extracted, the ratio is:
</span>3.6/10.8 = 1/3
Therefore, i<span>t will be extracted only 1/3 of NaCl less in 10 mL of water than in 30 mL of water. </span>
<span>C7H8
First, determine the number of relative moles of each element we have and the molar masses of the products.
atomic mass of carbon = 12.0107
atomic mass of hydrogen = 1.00794
atomic mass of oxygen = 15.999
Molar mass of CO2 = 12.0107 + 2 * 15.999 = 44.0087
Molar mass of H2O = 2 * 1.00794 + 15.999 = 18.01488
We have 5.27 mg of CO2, so
5.27 / 44.0087 = 0.119749 milli moles of CO2
And we have 1.23 mg of H2O, so
1.23 / 18.01488 = 0.068277 milli moles of H2O
Since there's 1 carbon atom per CO2 molecule, we have
0.119749 milli moles of carbon.
Since there's 2 hydrogen atoms per H2O molecules, we have
2 * 0.068277 = 0.136554 milli moles of hydrogen atoms.
Now we need to find a simple integer ratio that's close to
0.119749 / 0.136554 = 0.876937
Looking at all fractions n/m where n ranges from 1 to 10 and m ranges from 1 to 10, I find a closest match at 7/8 = 0.875 with an error of only 0.001937, the next closest match has an error over 6 times larger. So let's go with the 7/8 ratio.
The numerator in the ratio was for carbon atoms, and the denominator was for hydrogen. So the empirical formula for toluene is C7H8.</span>
