Do you have others? Also can you get chemguide as a pdf file?Try Znotes, they'd probably have it all. As for chemistry chemguide is pretty good!
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Do you have others? Also can you get chemguide as a pdf file?Try Znotes, they'd probably have it all. As for chemistry chemguide is pretty good!
Not sure ummm but 2&3?which ions are present in a solution of ethanol in an excess of concentrated sulphuric acid?
1) CH3CH2O^-1
2) CH3CH2^+OH2
3) HSO4^-1
which ions are present in a solution of ethanol in an excess of concentrated sulphuric acid?
1) CH3CH2O^-1
2) CH3CH2^+OH2
3) HSO4^-1
The two equations are:Can anyone explain to me how to arrive to the answer .... https://drive.google.com/file/d/1BkV12DgTZwm7fl42yz1lTP0m7SrHlKRq/view?usp=drivesdk
Reaction is first order wrt O2 and 2nd order wrt NO. So concentration of NO is increased 3 times as well as [O2]. You get (3^2) x 3 considering the orders which'd give you 27 times the rate in reaction 1.View attachment 64527
Can anyone tell me why in a(ii) they multipled experiment 1's initial rate with 27 to get K?
where that 27 came from?
explain?
bro where did this 3 came from?Reaction is first order wrt O2 and 2nd order wrt NO. So concentration of NO is increased 3 times as well as [O2]. You get (3^2) x 3 considering the orders which'd give you 27 times the rate in reaction 1.
Edit : An alternative way would be to calculate the rate constant using any experiment of your choice and then using it along with concentrations in the 4th experiment to get your desired rate.
O2 is first order and it's concentration is tripled [3]^1 will be 3bro where did this 3 came from?
to reduce the rate of reaction lower temperature will be used i.e 298 K and to keep the amount of barium nitrate and aluminum constant a lower or neutral pH will be used for if the pH is increased more hydroxides on the right side will be produced resulting in increased amount of aluminium reacting with the nitrates thus decreasing their amounts. to keep the reactants amount constant lower pH will be maintained.When making sparkler fireworks, a mixture of barium nitrate powder with aluminium powder, water and glue is coated onto wires and allowed to dry. At this stage, the following exothermic reaction may occur. 16Al + 3Ba(NO3)2 + 36H2O → 3Ba(OH)2 + 16Al(OH)3 + 6NH3 Which conditions would be best to reduce the rate of this reaction during the drying process, and would also keep the aluminium and barium nitrate unchanged? temperature/K pH A 298 7 B 298 14 C 398 7 D 398 14 https://papers.gceguide.com/A Levels/Chemistry (9701)/9701_s14_qp_11.pdf plz help
Thanks again broThe two equations are:
CH4 + 2O2 --> CO2 + 2H2O
CH4 + 3/2O2 --> CO + 2H2O
multiply equation 1 by 99 and add to equation 2
99CH4 + 198O2 --> 99CO2 + 198H2O
CH4 + 3/2O2 --> CO + 2H2O
---------------------------------------------------------------------------------------- add
100CH4 + 199(1/2)O2 --> 99CO2 + CO + 200H2O
So, burning 100 moles needs 199(1/2) moles of oxygen
Therefore burning y moles needs 2y - y/200
or expressed as a decimal fraction:
2y - (0.01/2)y
i.e. answer A
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