Natural formation of lead occurs by radioactive decay of uranium and thorium through radon (222Rn). Four stable isotopes are known, 204Pb, 206Pb, 207Pb and 208Pb, the first three of which are used for estimating the ages of rocks. Lead compounds exist mainly in +2 or +4 oxidation states, the former being more common.
Answer:
![\boxed {\boxed {\sf 104 \%}}](https://tex.z-dn.net/?f=%5Cboxed%20%7B%5Cboxed%20%7B%5Csf%20104%20%5C%25%7D%7D)
Explanation:
Percent ratio is the ratio of the actual yield to the theoretical yield. The formula is below.
![Percent \ Yield} = \frac{{Actual \ Yield}}{{Theoretical \ Yield}} \times 100 \%](https://tex.z-dn.net/?f=Percent%20%5C%20Yield%7D%20%3D%20%5Cfrac%7B%7BActual%20%5C%20Yield%7D%7D%7B%7BTheoretical%20%5C%20Yield%7D%7D%20%5Ctimes%20100%20%5C%25)
The reaction of sodium and chlorine should theoretically yield 12.5 grams, but the actual yield was 13.0 grams.
- actual yield= 13.0 g
- theoretical yield = 12.5 g
Substitute these values into the formula.
![Percent \ Yield} = \frac{{13.0 \ g }}{{12.5 \ g}} \times 100 \%](https://tex.z-dn.net/?f=Percent%20%5C%20Yield%7D%20%3D%20%5Cfrac%7B%7B13.0%20%5C%20g%20%7D%7D%7B%7B12.5%20%5C%20g%7D%7D%20%5Ctimes%20100%20%5C%25)
Divide.
![Percent \ Yield} = 1.04 \times 100 \%](https://tex.z-dn.net/?f=Percent%20%5C%20Yield%7D%20%3D%201.04%20%5Ctimes%20100%20%5C%25)
Multiply.
![Percent \ Yield= 104 \%](https://tex.z-dn.net/?f=Percent%20%5C%20Yield%3D%20104%20%5C%25)
For this reaction, the percent yield is 104%
Answer:
Dalton's atomic theory consisted of several postulates.
Explanation:
<span><span>
All matter consists of indivisible particles called atoms.
</span><span>
Atoms of the same element are similar in shape and mass, but differ from the atoms of other elements.
</span><span>
Atoms cannot be created or destroyed.
</span><span>
Atoms of different elements may combine with each other in a fixed, simple, whole number ratio to form compound atoms.
</span><span>
Atoms of same element can combine in more than one ratio to form two or more compounds.
</span><span>
Atoms are the smallest unit of matter that can take part in a chemical reaction.
</span></span>
Answer:
1.41 moles H2O2(with sig figs)
Explanation:
okay so what is the molar mass of H2O2= (1.008 g/mol)2+(16.00g/mol)2= (2.016+ 32.00) g/ mol
= 34. 02 g/mol
48.0g H2O2* 1 mol H2O2/ 34.02 g H2O2= 1.41 mol H2O2
Answer:
![K_p= 0.00016](https://tex.z-dn.net/?f=K_p%3D%200.00016)
Explanation:
The relation between Kp and Kc is given below:
Where,
Kp is the pressure equilibrium constant
Kc is the molar equilibrium constant
R is gas constant
T is the temperature in Kelvins
Δn = (No. of moles of gaseous products)-(No. of moles of gaseous reactants)
For the first equilibrium reaction:
Given: Kc = 0.50
Temperature = ![400^oC=[400+273]K=673K](https://tex.z-dn.net/?f=400%5EoC%3D%5B400%2B273%5DK%3D673K)
R = 0.082057 L atm.mol⁻¹K⁻¹
Δn = (2)-(3+1) = -2
Thus, Kp is:
![K_p= 0.00016](https://tex.z-dn.net/?f=K_p%3D%200.00016)