An 80.0 g sample of a gas was heated from 25 °C to 225 °C. During this process, 346 J of work was done by the system and its internal energy increased by 6505 J. What is the specific heat of the gas? c = J/(g · "C) - TOOLS x10

When methanol, CH, OH, is burned in the presence of oxygen gas, O,, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH, OH(g) + 0,(g) → CO,(g) + 2 H,O(1) ΔΗ --764 kJ How much methanol, in grams, must be burned to produce 837 kJ of heat?

Calculate the energy required to heat 1.80kg of ammonia from 21.5°C to 41.0°C . Assume the specific heat capacity of ammonia under these conditions is ·4.70J·g−1K−1 Round your answer to 3 significant digits.

Exactly 15.1 mL of water at 26.0 °C is added to a hot iron skillet. All of the water is converted into steam at 100.0°C. The mass of the pan is 1.20 kg and the molar heat capacity of iron is 25.19 J/(mol·°C). What is the temperature change of the skillet?

An 80.0 g sample of a gas was heated from 25 °C to 225 °C. During this process, 346 J of work was done by the system and its internal energy increased by 7115 J. What is the specific heat of the gas? J/(g. °C)

A balloon filled with gas is compressed under an external pressure of 3.0 atm from 4.0 L to 1.0 L. How much work (in Joules) is transferred during the compression? 1 Latm= 101.325J

In a certain process, 400 J of heat is added to a system and the system simultaneously does 100 J of work. The change in internal energy of the system is 500 J 400 J 300 J -100 J -300 J

The combustion of 1.925 g of propanol (C₂H,OH) increases the temperature of a bomb calorimeter from 298.00 K to 302.14 K. The heat capacity of the bomb calorimeter is 15.61 kJ/K. Determine AH for the combustion of propanol to carbon dioxide gas and liquid water. kJ/mol ΔΗ = TOOLS x10

A bomb calorimeter has a heat capacity of 6.067 kJ/°C. A sample of vitamin (C31H4602) has an internal energy (DE) = -2.278 X 104 kJ/mol. When 1.434 g of the vitamin sample are burned in oxygen in the calorimeter, determine the final temperature in °C if the initial temperature is 14.51 °C.

A chemist carefully measures the amount of heat needed to ralse the temperature of a 1.48 kg sample of C,H,0, from 32.9 °C to 50.0 °C. The experlment 4-8 2 shows that 4.02 x 10* J of heat are needed. What can the chemist report for the molar heat capacity of C,H,0,? Be sure your answer has the correct number of significant digits.