as system increases in. volume, it absorbs 59.0 J of energy in the form of heat from the surroundings. the piston is working against a pressure of 0.537 atm. the final volume of the system if 56.5 L. what was the initial valume of the system if the internal energy of the system decreased by 107.7 J?

Calculating a Heat of Formation Using Hess’s LawAs discussed in lecture, the simplest and most general method for determining theenergy change during a chemical reaction involves the use of the heat of formation (ΔHf) for thereactants and products. Conceptually, the heat of formation is the heat released or absorbedwhen one mole of the substance is created from its elements at standard temperature andpressure. In some cases, this number can be measured directly (i.e. by reacting the elements at1.0 atm and 25oC and observing the heat given off). In most cases, however, this is notpractical. For instance, the direct calculation of the ΔHf for magnesium oxide would involveburning magnesium metal in a pure oxygen atmosphere; while such a reaction is certainlypossible, it would difficult to measure changes in temperature since the reaction is highlyexothermic and the product is a solid powder. Instead, in this lab you will be calculating the ΔHf for magnesium oxide by determiningthe heat of…

An ideal gas sealed in a rigid 5.87-L cylinder, initially at pressure Pi=10.10 atm, is cooled until the pressure in the cylinder is Pf=1.06 atm. A) What is the enthalpy change for this process? B) What is the change in internal energy for this process?

The question is given like this, it is not incomplete. There is no heat capacity of the calorimeter given. Can it be solved without that? It is high school chemistry so maybe it can be solved in an easier way? Many thanks.

6. Toluene, C;Hs, is used in the manufacture of explosives such as TNT. A 1.500 gram sample of liquid toluene was placed in a bomb calorimeter along with excess oxygen. When the combustion of the toluene was initiated, the temperature of the calorimeter rose from 25.000°C to 26.413°C. The products of the reaction were carbon dioxide and water, and the heat capacity of the calorimeter was 45.06 kJ/°c. Write a balanced thermochemical equation for the combustion of toluene.

Liquid hydrogen peroxide releases oxygen gas in its decomposition. 2 H2O2 → 2 H2O + O2 ΔΗ, = -196.1 kJ rxn How much heat in kJ is released when 701.278 g of H2O2 decomposes in a rocket fuel mixture? Type your answer...

||| O THERMOCHEMISTRY Calculating the heat of reaction from molar reaction enthalpy a... V A chemist measures the energy change AH during the following reaction: 2 H₂O(l) → 2 H₂(g) + O₂(g) Use the information to answer the following questions. This reaction is... Suppose 91.7 g of H₂O react. Will any heat be released or absorbed? If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits. esc Explanation ← Check ΔΗ= 572. kJ → endothermic. exothermic. Yes, absorbed. O Yes, released. No. E kJ x10 X MacBook Pro Search or type URL 2022 McGraw Hill LLC. All F

calculate heatE of a gas for a process in which the gas absorbs 25J of heat and does 7J of work by expanding

A chemist measures the energy change AH during the following reaction: Cl,(9)+H,(g) → 2 HCl(g) AH=-184. kJ Use the information to answer the following questions. O endothermic. This reaction is... x10 O exothermic. Suppose 62.6g of Cl, react. O Yes, absorbed. O Yes, released. Will any heat be released or absorbed? O No. If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. kJ Round your answer to 3 significant digits.

This is follow up problem 6.2A:  A gas is compressed at constant temperature from a volume of 8.45 L to a volume of 2.17 liters by an external pressure of 730 torr.  Calculate the work done (in J).  1 atm ⋅ L = 101.3 J.  Enter to 3 sig figs.