HELP PLEASE! How is this done??

[T84]

Please help me understand this.

Please show me how, why, and where. Show all work please.

 

1) C4 H10 O (g) + 6 O2 ---> 4 CO2 + 5 H2O (g)

Calculate the work, at 25*C, for the combustion of 37.0g of C4 H10 O with a sufficiency of oxygen. R= 8.31 J/mole x K Answer is -2480 J

 

2) In a Coffee cup calorimeter, with a heat capacity of 44 J/*C, 50.0 mL of 0.100 M NaOH is reacted with 50.0mL of 0.100 M HBr. The temperature of the calorimeter and it's contects rises by 1.08*C as the reaction occurs. Assuming the specific heat of the resulting solution is 4.18 J/g*C and it's density is 1.02 g/mL, calculate the heat of the reaction in units of kJ per mole of NaOH reacted. Answer is -102 kJ/mole

[modest]

Please help me understand this.

Please show me how, why, and where. Show all work please.

 

1) C4 H10 O (g) + 6 O2 ---> 4 CO2 + 5 H2O (g)

Calculate the work, at 25*C, for the combustion of 37.0g of C4 H10 O with a sufficiency of oxygen. R= 8.31 J/mole x K Answer is -2480 J

 

Work is equal to change in volume times pressure w = dV X p.

You have 37g of gas butinol. You need to convert this to mols then add the mols of oxygen. With that, you can convert to volume at 25C via PV=nRT. Then calculate the volume of the products using the balanced equation given. You will then have the change in volume dV. Then convert to Joules via 1 Liter-atmosphere = 101 Joules. That will be your answer.

 

Now that I say that, it sounds overwhelming. If you want to work through it step by step, I'll check each step. Step one is converting 37 grams of C4H10O to mols.

 

~modest