Question

The reaction of 1.00 mole of H2(g) with 0.500 mole of O2(g) to produce 1.00 mole of steam, H2O(g), at 100°C and 1.00 atm pressure evolves 242 kJ of heat. Calculate ΔE per mole of H2O(g) produced. The universal gas constant is 8.314 J/mol·K. a. +240 kJ b. -240 kJ c. +242 kJ d. -242 kJ e. -238 kJ

Name: the reaction of 100 mole of h2g with 0500 mole of o2g to produce 100 mole of steam h2og at 100ac and 100 atm pressure evolves 242 kj of heat calculate ae per mole of h2og produced the univer 41823
Uploaded: 2022-09-24T09:41:22-08:00
Duration: 2 min 9 s
Channel: Sri K
Description: the reaction of 100 mole of h2g with 0500 mole of o2g to produce 100 mole of steam h2og at 100ac and 100 atm pressure evolves 242 kj of heat calculate ae per mole of h2og produced the univer 41823

          The reaction of 1.00 mole of H2(g) with 0.500 mole of O2(g) to produce 1.00 mole of steam, H2O(g), at 100°C and 1.00 atm pressure evolves 242 kJ of heat. Calculate ΔE per mole of H2O(g) produced. The universal gas constant is 8.314 J/mol·K.
a. +240 kJ
b. -240 kJ
c. +242 kJ
d. -242 kJ
e. -238 kJ

Added by Paul R.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sri K

09/24/2022

Step 1

5 moles of O2 to produce 1 mole of H2O. Given: ΔH = -242 kJ Since 1 mole of H2 reacts with 0.5 moles of O2 to produce 1 mole of H2O, the energy change per mole of H2O produced is -242 kJ. Show more…

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The reaction of 1.00 mole of H2(g) with 0.500 mole of O2(g) to produce 1.00 mole of steam, H2O(g), at 100°C and 1.00 atm pressure evolves 242 kJ of heat. Calculate ΔE per mole of H2O(g) produced. The universal gas constant is 8.314 J/mol·K. a. +240 kJ b. -240 kJ c. +242 kJ d. -242 kJ e. -238 kJ