Answer:
Atoms are composed of extremely small particles that are too small to be seen with an optical microscope.
Size at the atomic level is measured on the nanoscale.
Atoms are made of three subatomic particles - protons, neutrons, and electrons.
Protons:
- positively charge
- located in the nucleus
Neutrons:
- no charge (neutraly charge)
- located in the nucleus
Electrons:
- negatively charged
- located around the nucleus
Atomic number (Z) = the number of protons in the nucleus of an atom.
(i apologize, i don't understand the last part...)
Answer:
option b is the answer of given statementtwo atoms of potassium react with one molecule of chlorine to produce two molecules of potassium chloride
Answer:
80mL
Explanation:
Step 1:
Data obtained from the question.
Initial Volume (V1) = 40mL
Initial temperature (T1) = –123°C
Final temperature (T2) = 27°C
Final volume (V2) =..?
Step 2:
Conversion of celsius temperature to Kelvin temperature.
T(K) = T(°C) + 273
Initial temperature (T1) = –123°C =
–123°C + 273 = 150K
Final temperature (T2) = 27°C = 27°C + 273 = 300K
Step 3:
Determination of the final volume.
This can be obtained as follow:
V1/T1 = V2/T2
Initial Volume (V1) = 40mL
Initial temperature (T1) = 150K
Final temperature (T2) = 300
Final volume (V2) =..?
V1/T1 = V2 /T2
40/150 = V2 /300
Cross multiply
150 x V2 = 40 x 300
Divide both side by 150
V2 = (40 x 300) /150
V2 = 80mL
Therefore, the new volume of the gas is 80mL
Answer:
P₂ = 2.60 atm
Explanation:
Given data:
Initial pressure = 2.38 atm
Initial temperature = 25.0 °C
Final pressure = ?
Final temperature = 52.78°C
Solution:
Initial temperature = 25.0 °C (25.0+273 = 298 K)
Final temperature = 52.78°C (52.78+273 = 325.78 K)
According to Gay-Lussac Law,
The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.
Mathematical relationship:
P₁/T₁ = P₂/T₂
Now we will put the values in formula:
2.38 atm / 298 K = P₂/325.78 K
P₂ = 2.38 atm × 325.78 K / 298 K
P₂ = 775.35 atm. K /293 K
P₂ = 2.60 atm
Answer:
(a) m = 50.916 g
(b) CO2 is the limiting reagent and C is the reagent in excess.
(c) the mass excess left = 4.084 g
Explanation:
Balance the given equation first:
(a) Given:
mass of CO2 = 40.0 g
mass of C = 15.0 g
mass of CO = ?
To find the mass of CO that will be produced, we need to find the limiting reactant first. To find the limiting reactant we will calculate the number of moles of each reactant, the reactant with less number of moles is the limiting reactant.
CO2:
n = m/M where m is the mass and M is the molar mass
n = 40.0g/44.01 g/mol
n = 0.909 mol
C:
n = m/M
n = 15.0 g/12,0107 g/mol
n = 1.249 mol
CO2 is the limiting reagent and C is the reagent in excess.
Grams of CO that will be produced:
The molar ratio between CO2 and CO is 1:2
Therefore the number of moles of CO = 0.909 x 2 = 1.818 mol
m = n x M
m = 1.818 mol x 28,01 g/mol
m = 50.916 g
(c) To find how much of the reagent in excess will be left we will use the stoichiometry
n = 0.909 mol
m = 0.909 mol x 12.0107 g/mol
m = 10.916 g
15.0 g - 10.916 g = 4.084 g
Therefore the mass excess left = 4.084 g