A sample is completely reacted in a \"coffee cup\" calorimeter. The calorimeter

Question

A sample is completely reacted in a "coffee cup" calorimeter. The calorimeter contains 871 g of water, and the measured temperature increase is 3.73 degree C. what is the energy of the reaction? [SHw = 1.00 cal/g degree C] A) 3.25 times 10^6 cal B) 325 cal C) 3.25 cal D) 0.00325 cal E) 3250 cal Calculate the moles of a 1.2 L solution at 2.9 atm and 14 degree C. A) 0.15 mol B) 3.0 mol C) 6.8 mol D) 0.33 mol E) 0.015 mol A given mass of fluorine at room temperature occupies a volume of 0.600 L at 2.00 atm pressure. What pressure must be applied to compress the gas to a volume of only 0.160 L? A) 0.192 atm (B) 7.50 atm C) 0.0480 atm D) 1.50 atm E) 0.133 atm The reaction A + B + C rightarrow D + E is third order for reactant A, second order for B, and first order for C. What is the rate law equation for this reaction? A) rate = k[A]^3[B]^2[C] B) rate = k[3A] [2B] [C] C) rate = k[3A]^3[2B]^2[C] D) rate = k[A] [B] [C] E) rate = [A] [B] [C]

Explanation / Answer

31) Energy of the reaction will be equal to = mass*SHw *(change in temperature)

Now mass=871gm

SHw=1cal/gC

and change in temperature= 3.73 C.

So energy = 871*1*3.73= 3249.203 cal (d)

32)PV=nRT
n=PV/RT=1.2*2.9/0.0821*(14+273) as temperature must be in Kelvin

n=0.148 moles
approximately equal to 0.15 (A) ans.

33)As nothing is specified in the question we will take it as an isothermal process meaning temperature remains constant. So, P1V1=P2V2 . Putting the values we get P2 = 7.5 atm. (B)

34)Your answer is correct.

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