Determine the Delta H degree for the reaction C_(g) + O_2(t) rightarrow CO_2(g)

Question

Determine the Delta H degree for the reaction C_(g) + O_2(t) rightarrow CO_2(g) using Hess's Law and equations 1 and 2: CO_(g) rightarrow C_(g) + 1/2 O_2(g) Delta H degree = + 110.5 kJ CO_(g) + 1/2 O_ 2_(g) rightarrow CO_2(g) Delta H degree = -283.0 kJ A. -3.13 times 10^4 kJ B. +173 kJ C. -393J kJ D. +393.5 kJ How much natural gas (CH_4 - 16 g/mol) must be burned in order to produce 75,000 kJ of energy? CH_4(g) + 2O_2(g) rightarrow CO_2(g) + 2H_2O_(g) Delta H = -2000kJ A. 37.5 g B. 1500 kg C. 26.7 g D. 600g The energy of a 600mn photon is 3.3 times 10^-19 J. What is the energy of a 300nm photon? A. 3.3 times 10^-20 J B. 1.65 times 10^-18 J C. 6.6 times 10^-19 J D. 2 times 10^-20 J A wifi network has an operating frequency of 2.4 times 10^9 Hz. What is the wavelength of this network? A. 0.125 m B. 1.25 times 10^-9 m C. 7.2 m D. 6.26 times 10^-8 m

Explanation / Answer

Ans 5 :

CO -------> C + 1/2 O2 ,   dH° = +110 kJ/mol
CO + 1/2 O2 -----> CO2,   dH° = -283 kJ/mol.

Adding the two equations together and cancel out the intermediate, CO, on both sides leads to

C + O2 -> CO2,   dH° = (-110)+(283) = +173 kJ/mol.

Hence option B is correct answer

Ans 6 ) 16 g/mol of CH4 produces 2000 Kj of energy

So 75000 Kj will be produced by ?

= 16 * 75000 / 2000

= 600 g

Hence option D is correct

Ans 7 ) We have E = hc /

E = 6.626 × 10 -34 joule·s * 2.998 × 108 m/s / 300 * 10^-9 m

E = 6.6 * 10^-19 J

hence option c is correct

Ans 8 ) V = * c

2.4 * 10 ^ 9 per sec = *  2.998 × 108 m/s

   = 0.72 m

hence option c is correct

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