This is my sons acount
he is homeschooled and needs help with this homework
someone please help with any answers so i can help him
http://snapserve.net/teacher/141484/SCI401_-_Mod_15,_Test.pdf?110519034817
he is homeschooled and needs help with this homework
someone please help with any answers so i can help him
http://snapserve.net/teacher/141484/SCI401_-_Mod_15,_Test.pdf?110519034817
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1) When the two graphs start to touch each other - about the 18th second
2) If a chemical system in equilibrium experiences a change in concentration, temperature, pressure, etc. it shifts to compensate for that change.
3) It measures the concentration of H+ (H3O+) ions in a solution
4) HNO3 -> H(+) + NO3(-)
H(+) reacts with H2O to form H3O(+), but this is often omitted for simplicity :)
5) When the graphs start separating - 29 s (the biggest stress is at 33 s)
6) The strongest acid - the lowest pH (it is also the weakest base) - E
The strongest base - the highest pH (it is also the weakest acid) - B
7) Ka=[H+]*[A-]/[HA]
Since [HA] is equal, you should order them in increasing of [H+] - highest to lowest pH: A B D E C
8) K=[NO]^2*[Br2]/[NOBr]^2 = 0.010^2 * 0.0050 / 0.10^2 = 0.00005M
9) In the expression of K there aren't any solids, so K=[SO2], therefore c(SO2)=0.345M
10) b) the units are 1/M, so K=1/0.63M which is >1. If K>1, then the reaction need only 1 arrow. a) is also 1/M, when you calculate it, K<1
11) K=[H2SO3] / ([SO2]*[H2O])
2.1 * 10^-3 (then ot the power of -3) = 0.23/0.35*[H2O]
[H2O]=0.66/2.1*10^-3=31.3M. It should be <1, so this isn't an equilibrium. To lower it, you need to shift the reaction to the right side (towards H2SO3)
12) a. It will rise
b.It will rise
c. It will rise :))
A reaction always shifts to where there is a lower concentration of compounds.
13) a. It will become lower
b. It will rise
c. It will rise
When the pressure is increased, the reaction shifts to whatever side has the smallest number of moles of gases (here there are 3 moles on the left and 2 moles on the right). When the pressure is lowered, it's the other way around :)
14) Ka=[H+]*[ClO2-]/[HClO2]
15)Kb=Kw/Ka=Kw*[CH5P] / [CH5+]*[P-]. Kw is 10^(-14) at STP
2) If a chemical system in equilibrium experiences a change in concentration, temperature, pressure, etc. it shifts to compensate for that change.
3) It measures the concentration of H+ (H3O+) ions in a solution
4) HNO3 -> H(+) + NO3(-)
H(+) reacts with H2O to form H3O(+), but this is often omitted for simplicity :)
5) When the graphs start separating - 29 s (the biggest stress is at 33 s)
6) The strongest acid - the lowest pH (it is also the weakest base) - E
The strongest base - the highest pH (it is also the weakest acid) - B
7) Ka=[H+]*[A-]/[HA]
Since [HA] is equal, you should order them in increasing of [H+] - highest to lowest pH: A B D E C
8) K=[NO]^2*[Br2]/[NOBr]^2 = 0.010^2 * 0.0050 / 0.10^2 = 0.00005M
9) In the expression of K there aren't any solids, so K=[SO2], therefore c(SO2)=0.345M
10) b) the units are 1/M, so K=1/0.63M which is >1. If K>1, then the reaction need only 1 arrow. a) is also 1/M, when you calculate it, K<1
11) K=[H2SO3] / ([SO2]*[H2O])
2.1 * 10^-3 (then ot the power of -3) = 0.23/0.35*[H2O]
[H2O]=0.66/2.1*10^-3=31.3M. It should be <1, so this isn't an equilibrium. To lower it, you need to shift the reaction to the right side (towards H2SO3)
12) a. It will rise
b.It will rise
c. It will rise :))
A reaction always shifts to where there is a lower concentration of compounds.
13) a. It will become lower
b. It will rise
c. It will rise
When the pressure is increased, the reaction shifts to whatever side has the smallest number of moles of gases (here there are 3 moles on the left and 2 moles on the right). When the pressure is lowered, it's the other way around :)
14) Ka=[H+]*[ClO2-]/[HClO2]
15)Kb=Kw/Ka=Kw*[CH5P] / [CH5+]*[P-]. Kw is 10^(-14) at STP