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B makes sense because the rate of condensation is much slower than the rate of evapouration
@taramgrant0543664 that was wrong
Wait I didn't really like that answer so I wanted to double check and it should have been c. I assumed that evapouration would get ahead but it stays constant the condensation speeds up to accomidate making the rates equal
Two gases are placed in a sealed flask and allowed to react. Which statement is true about the concentrations of the reactants and products when this closed system reaches dynamic equilibrium? They will be equal and constant. They will be equal but continuously changing. They will not necessarily be equal, and they will be continuously changing. They will not necessarily be equal, but they will be constant.
this one was wrong too we had picked c
It could've been d
it was thanks
What is the oxidation number of fluorine (F) in F2? +1 −1 0 −3
They should be electrically neutral
When F2 bond to another, the oxidation # on each atom is 0. If oxidation state is maintained at -1, it would lead the molecule to have a net -2 charge. Such oxidation # assignment is inaccurate, since F2 molecules are electrically neutral.
so 0 would be correct
Which of the following describes an element that is oxidized in a reaction? It gains electrons during a reaction. It has a decrease in its oxidation number. Al yields Al3+ + 3e− F2 + 2e− yields 2 F−
In oxidation you. Lose electrons
so b? @taramgrant0543664
C is an oxidation reaction, it's not B because if you lose electrons you become more positive increasing the oxidation number, it's not D as that is a reduction reaction and a is describing the reduction reaction
Which of the following chemical reactions is an oxidation-reduction reaction? CuSO4 + BaCl2 yields BaSO4 + CuCl2 AgNO3 + NaCl yields AgCl + NaNO3 Pb(NO3)2 + 2NaCl yields PbCl2 + 2NaNO3 Zn + H2SO4 yields ZnSO4 + H2
Check the charges on each element for the product side and reactant side. If any element had a change in its charge, it's an oxidation/reduction reaction. AgNO3 + NaCl --> AgCl + NaNO3 Reactant side: Ag has a charge of +1 N has a charge of + 5 O has a charge of - 2 (-2 * 3 = -6 total) Na has a charge of +1 Cl has a charge of -1 Product side: Ag has a charge of +1 Cl has a charge of -1 Na has a charge of +1 N has a charge of +5 O has a charge of -2 No species in the reaction had a change in charge meaning it's not a reduction/oxidation reaction.
so d is corrrect?
Yes D is correct
Consider the following reaction: Cl2 + 2NaBr yields 2NaCl + Br2 Which element is oxidized and which is reduced in the reaction? Br is reduced and Na is oxidized. Cl is reduced and Br is oxidized. Cl is reduced and Na is oxidized. Na is reduced and Br is oxidized.
Left side Cl -> 0 Na -> +1 Br -> -1 Right side Cl -> -1 Na-> +1 Br-> 0 Lose electrons oxidized, gain electrons reduced
Cl is being reduced, but Ana the charge remains the same so it is not being oxidized or reduced
B IS CORRECT?
Yes it is B, Br is losing electrons and therefore oxidized
What is true of an element that was reduced in a chemical reaction? It lost electrons. It gained electrons. It increased electronegativity. It decreased electronegativity.
If it loses electrons it's oxidized, if it gains electrons it's reduced
If it was reduced then it should have gained electrons, it does not affect electronegativity
b is correct?
Which of the following describes an element that is reduced in a reaction? It acts in the reactant that is the reducing agent. It has a decrease in its oxidation number. Cd yields Cd2+ + 2e− Zn + Cu2+ yields Zn2+ + Cu
Well we can take out A since the reducing agent donates or loses electrons so if it loses electrons it becomes oxidized. We can also rule out B because the number wouldn't decrease it would increase
D is a redox reaction so c is the only one specifically referring to an element that is being reduced
@taramgrant0543664 c is wrong
so d should be correct?
I'm pretty sure a and b are wrong so then I guess it must be D