Answer:
Explanation:
Hello,
In this case, the heat, mass, specific heat and temperature change are related by:
Thus, if we want to compute the specific heat we simply solve for it:
Best regards.
HELPP!!!!!!!!!!! Can someone do this for me on paper
1 answer:
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Through manipulation of equations, we are able to obtain the equation:
![-pOH= log [ OH^{-}]](https://tex.z-dn.net/?f=-pOH%3D%20log%20%5B%20OH%5E%7B-%7D%5D%20)
Then we can transform the equation into:
![[ OH^{-}]= 10^{-pOH}](https://tex.z-dn.net/?f=%5B%20OH%5E%7B-%7D%5D%3D%2010%5E%7B-pOH%7D%20%20)
Then we are able to plug in the pOH and directly get [OH-]:
![[ OH^{-}] = 10^{-6.48}](https://tex.z-dn.net/?f=%5B%20OH%5E%7B-%7D%5D%20%3D%2010%5E%7B-6.48%7D%20)
![[ OH^{-}]=3.31* 10^{-7} M](https://tex.z-dn.net/?f=%5B%20OH%5E%7B-%7D%5D%3D3.31%2A%2010%5E%7B-7%7D%20M%20%20)
Then we can transform the equation into:
Then we are able to plug in the pOH and directly get [OH-]:
Answer:
Maximum mass of produces=50.8g;
Explanation:
Firstly balance the chemical reaction,
Molecular weight of =334g/mole;
Molecular weight of CO =28g/mole;
Number of mole of given=80g/(334g/mole)=0.239mole;
Number of mole of CO given=28g/(28g/mole)=1 mole
Moles are:
Number of mole of =0.239
Number of mole of CO=1;
From the balanced equation,
1 mole of reacts with 5 moles of CO;
Hence;
0.239 mole of will react with 5*0.239 moles of CO means
Moles of CO that reacts with =1.2 mole but we have given 1 mole therefore
Will be excess reagent and CO will be the limitting reagent
And mass of product depends on limiting reagent i.e. mass of CO.
5 mole of CO produces 1 mole of
;
1 mole of CO produces 1/5 mole of ;
Maximum mass of produces=mole*molecular weight;
Molecular weight of =254g/mole;
Maximum mass of produces = (1/5)*254=50.8g;
Maximum mass of produces=50.8g;