Answer:
goes on to the circle
Explanation:
hm and the I have know what how much you have want
Answer:
See below.
Explanation:
1. The water here is the solvent, and the 'sugar and fruit specific chemicals' are considered the solute. That is as the solute is the component dissolved in the solvent.
2. The collision theory states that the greater the collisions, the greater the rate of reaction. When powdered sugar is placed in the water (solvent) it occupies more surface area, resulting in more collisions that speed up the rate of reaction, compared to a cube of sugar - that occupies less surface area. Therefore, the powdered sugar dissolved faster.
3. Molarity describes the number of moles of a substance per unit of volume. The standard unit of volume is liter, giving you the standard units (mol/l). Molality describes the number of moles per unit of mass, typically kilograms (mol/kg).
The concentration of a solution can be given in moles of solute dissolved per kilogram of solvent for molality, and moles of solute dissolved in liters of solvent for molarity. Molality is generally used for concentration.
Answer is <u>D</u> - homogeneous mixture has the same throughout a while a heterogeneous mixture is not a uniform throughout. Explanation: I hoped that helped.
Answer: a) 
b) 
Explanation:
a) If percentage are given then we are taking total mass is 100 grams.
So, the mass of each element is equal to the percentage given.
Mass of C = 15.8g
Mass of S= 84.2 g
Step 1 : convert given masses into moles.
Moles of C =
Moles of S=
Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.
For C = 
For S =
The ratio of C : S = 1:2
Hence the empirical formula is
b) Mass of C= 40 g
Mass of H= 6.7 g
Mass of O = 53.3 g
Step 1 : convert given masses into moles.
Moles of C =
Moles of H =
Moles of O =
Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.
For C = 
For H = 
For O =
The ratio of C : H: O= 1 :2: 1
Hence the empirical formula is
Answer:
i am sure its the last one
