sachin123 said:delta H = delta U + P(delta V)
Delta H refers to the change in enthalpy of a system, while q refers to the heat exchanged between a system and its surroundings. In other words, delta H is a measure of the overall energy change in a system, while q specifically measures the transfer of thermal energy.
Yes, both delta H and q can have positive or negative values. A positive delta H indicates an endothermic process, where the system absorbs heat from the surroundings. A negative delta H indicates an exothermic process, where the system releases heat to the surroundings. Similarly, a positive q indicates heat being transferred into the system, while a negative q indicates heat being transferred out of the system.
Delta H and q are both related to the change in internal energy of a system. They are connected by the equation q = delta H + delta nRT, where delta n is the change in the number of moles of gas and R is the gas constant. This equation is known as the heat capacity equation.
Yes, delta H is typically measured in joules (J) or kilojoules (kJ), while q can be measured in a variety of units depending on the specific situation. For example, q can be measured in joules, calories, or British thermal units (BTUs) depending on the system being studied.
A change in temperature will affect both delta H and q. An increase in temperature will lead to an increase in both delta H and q, while a decrease in temperature will result in a decrease in both delta H and q. This is because temperature is directly related to the internal energy of a system, which is a component of both delta H and q.