A gas is confined to a cylinder under constant atmospheric pressure, as illustrated in the following figure. When the gas undergoes a particular chemical reaction, it absorbs 822 J of heat from its surroundings and has 0.69 kJ of P−V work done on it by its surroundings.
What is the value of ΔH for this process?
Express your answer with the appropriate units.
∆H = Heat change of the system + work done by(or) done on the system
Heat change of the system, q = + 822J
work done on the system , w = 0.69kJ = 690J
∆H = + 822J + 690J
∆H = + 1512J
A gas is confined to a cylinder under constant atmospheric pressure, as illustrated in the following...
A gas is confined to a cylinder under constant atmospheric pressure, as illustrated in the following figure. When the gas undergoes a particular chemical reaction, it absorbs 822 J of heat from its surroundings and has 0.69 kJ of P−V work done on it by its surroundings. What is the value of ΔE for this process? Express your answer with the appropriate units.
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