For a particular reaction at 148.1 °C, Δ?=−1428.51 kJ, and         Δ?=393.69 J/K  .  Calculate Δ? for this reaction at −62.8 °C.   Δ?=Δ?−?Δ? thus,  Δ?=Δ?+?Δ?

For each of the following processes, indicate whether the signs of ∆S and ∆H are expected to be positive, negative, or about zero. A piece of charcoal is combusted to form CO21g2 and H2O1g2

What is entropy, and what is ΔS for a reaction, and what does it mean if ΔS is positive or negative?

For the reaction 2 A(g) → A2(g), Q = -20.00 kJ for the formation of onemole of A2(g) at constant volume and a temperature of 25.00◦C. If we did thissame reaction at constant pressure, what would be the values of Q, W, ∆U,and ∆H for the formation of one mole of A2(g) at a temperature of 25.00◦C?

The specific heat capacity of ice is 2.04 J/g⋅∘C and its heat of fusion is -332 J/g. Calculate the q for melting 127 g of ice to 16 degrees C. Find the w for this process. Find ΔE for this process. Find ΔH for this process.

For a particular reaction at 148.1 °C, delta G=−1428.51 kJ, and       delta S =393.69 J/K  .  Calculate delta G for this reaction at −62.8 °C.   Free energy is related to enthalpy, temperature, and entropy through the equation delta G = delta H -T(delta S) Δ?=Δ?−?Δ? delta H = delta G + T (delta S) Solve for the enthalpy of the reaction. Assume that enthalpy and entropy will not change between the two temperatures. Use the values from the prior scenario (temperature) to determine the new free energy value using the first equation.

For a particular reaction, Δ?=−14.20 kJ and Δ?=−198.5 J/K. Calculate Δ? for this reaction at 298 K