Q=mcΔT
q=(125g)(0.446 J/(g x °C))(78°C - 23.5°C)
q=(125 g)(0.446 J/(g x °C))(54.5°C) (Be sure to cancel all similar units)
q= 3038.375 J
Answer:
0.72 moles of hydrochloric acid are needed to completely react with 0.36 mol of lead.
Explanation:
The balanced reaction is:
Pb + 2 HCl → PbCl₂ + H₂
By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of reagent participate:
You can apply the following rule of three: if by stoichiometry of the reaction 1 mole of Pb reacts with 2 moles of HCl, 0.36 moles of Pb will react with how many moles of HCl?
amount of moles of HCl= 0.72 moles
<u><em>0.72 moles of hydrochloric acid are needed to completely react with 0.36 mol of lead.</em></u>
Explanation:
Dichlorine heptaoxide () can also be written as as one oxygen atom will be at the center and there will be two terminal groups.
This dichlorine heptaoxide is electrically neutral as there is no charge on this compound.
Number of valence electrons in an oxygen atom are 6, valence electrons in a chlorine atom are 7.
Hence, total number of valence electrons in will be as follows.
Total valence electrons =
= 56
Lewis structure of will have one oxygen atom at the center and two terminal groups. Each oxygen atom in will have 2 lone pair of electrons and oxygen atoms of groups will be attached to chlorine atoms through double bonds.