Answer:
0.5188 M or 0.5188 mol/L
Explanation:
Concentration is calculated as <u>molarity</u>, which is the number of moles per litre.
***Molarity is represented by either "M" or "c" depending on your teacher. I will use "c".
The formula for molarity is:
n = moles (unit mol)
V = volume (unit L)
<u>Find the molar mass (M) of potassium hydroxide.</u>
<u>Calculate the moles of potassium hydroxide.</u>
Carry one insignificant figure (shown in brackets).
<u>Convert the volume of water to litres.</u>
Here, carrying an insignificant figure doesn't change the value.
<u>Calculate the concentration.</u>
<= Keep an insignificant figure for rounding
<= Rounded up
<= You use the unit "M" instead of "mol/L"
The concentration of this standard solution is 0.5188 M.
Partial pressure (N2) = mole fraction * total pressure
{ 1 mole of any ideal gas occupy same volume of 1 mole of any other ideal gas under same condition of temperature and pressure so mole fraction in the sample is simply 78.08% = 0.7808 this is because equal volume of each gas has equal moles
partial pressure N2 = 0.7808 * 760 .0
partial pressure = 593.4 mmhg ( 1 torr = 1mmhg )
Answer:
Theoretical yield =26.03 g
Percent yield = 87%
Limiting reactant = CaO
Explanation:
Given data:
Mass of CaO = 14.4 g
Mass of CO₂ = 13.8 g
Actual yield of CaCO₃ = 22.6 g
Theoretical yield = ?
Percent yield = ?
Limiting reactant = ?
Solution:
Chemical equation:
CaO + CO₂ → CaCO₃
Number of moles of CaO:
Number of moles = Mass /molar mass
Number of moles = 14.4 g / 56.1 g/mol
Number of moles = 0.26 mol
Number of moles of CO₂:
Number of moles = Mass /molar mass
Number of moles = 13.8 g / 44 g/mol
Number of moles = 0.31 mol
Now we will compare the moles of CO₂ and CaO with CaCO₃ .
CO₂ : CaCO₃
1 : 1
0.31 : 0.31
CaO : CaCO₃
1 : 1
0.26 : 0.26
The number of moles of CaCO₃ produced by CaO are less it will be limiting reactant.
Mass of CaCO₃: Theoretical yield
Mass of CaCO₃ = moles × molar mass
Mass of CaCO₃ =0.26 mol × 100.1 g/mol
Mass of CaCO₃ = 26.03 g
Percent yield:
Percent yield = actual yield / theoretical yield × 100
Percent yield = 22.6 g/ 26.03 g × 100
Percent yield = 0.87× 100
Percent yield = 87%
Limiting reactant:
The number of moles of CaCO₃ produced by CaO are less it will be limiting reactant.
Answer:
See Explanation
Explanation:
Let us consider the first two reactions, the initial concentration of CO was held constant and the concentration of Hbn was doubled.
2.68 * 10^-3/1.34 * 10^-3 = 6.24 * 10^-4/3.12 * 10^-4
2^1 = 2^1
The rate of reaction is first order with respect to Hbn
Let us consider the third and fourth reactions. The concentration of Hbn is held constant and that of CO was tripled.
1.5 * 10^-3/5 * 10^-4 = 1.872 * 10^-3/6.24 * 10^-4
3^1 = 3^1
The reaction is also first order with respect to CO
b) The overall order of reaction is 1 + 1=2
c) The rate equation is;
Rate = k [CO] [Hbn]
d) 3.12 * 10^-4 = k [5 * 10^-4] [1.34 * 10^-3]
k = 3.12 * 10^-4 /[5 * 10^-4] [1.34 * 10^-3]
k = 3.12 * 10^-4/6.7 * 10^-7
k = 4.7 * 10^2 mmol-1 L s-1
e) The reaction occurs in one step because;
1) The rate law agrees with the experimental data.
2) The sum of the order of reaction of each specie in the rate law gives the overall order of reaction.
B) Glass Windows..... Hope it helps :)
