The value of delta H^+ for the reaction below is -186 kj. Calculate the heat (kj
ID: 1062145 • Letter: T
Question
The value of delta H^+ for the reaction below is -186 kj. Calculate the heat (kj) released from the reaction ot 25 g of cl_2- H_2(g) + c;l_2(g)| rightarrow 2HCl(g) 66 -186 47 5.3 times 10^2 33 The amount of heat required to raise the temperature of 1 g of a sample by 1 degree C is called the hotness factor the heat capacity the internal energy the specific heat the enthalpy The specific heat of k ad is 0.13 J/(g.degree C). How much heat (in J) is required to raise the temperature of 15 g of lead from 22 degree C to 37 degree C? 29 2.0 0.13 -0.13 5.8 times 10^-4 The SI unit for heat is joule calorie Kelvin j/(g, degree C) ergExplanation / Answer
Q.No-10
Mass of Cl2 = 25g Molecular Mass of Cl2 = 71g/mol
Mole of Cl2 = 25g / 71 g/mol = 0.352 Mole
From reaction,
1 Mole of Cl2 gives delta H = -186 KJ
Hence 0.352 Mole of Cl2 will give delta H = -186* 0.352 = -65.4 7 KJ (approx 66 KJ)
So heat will release 66 KJ
Q.No-11 (D)
Q.No-12
We know Q= ms(T2-T1)
Where Q is heat energy, m is mass of substance, s is specific heat capacity, T1 is initial temperature and T2 is final temperature
Heat energy, Q = 15g * 0.13 J g-1oC-1 * (37-22)oC
Q = 29.25 J --------(A)
Q.No-13 -------(A)
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