A chemical reaction produces a large increase in the number of moles of gas. Determine whether constant pressure or constant volume conditions would produce the largest amount of heat. constant pressure both conditions will produce the same amount of heat not enough information given constant volume

Why does a leak in a car tire (at constant temperature) decrease the pressure of the tire? A. The number of molecules decreases. B. It removes kinetic energy from the system. C. The temperature decreases. D. The volume decreases.

Which statement best defines specific heat? The amount of heat required to increase the temperature of 1 mol of a substance by 1 °C. The amount of heat required to increase the temperature of a specific object, such as a calorimeter, by 1 °C. The amount of heat required to increase the temperature of 1 g of a substance by 1 °C. The amount of heat required to increase the temperature of 1 L of a substance by 1 °C.

You may also assume X behaves as an ideal gas in the vapor phase. Suppose a small sample of X at 50 °C is put into an evacuated flask and heated at a constant rate until 10.0 kJ/mol of heat has been added to the sample. Graph the temperature of the sample that would be observed during this experiment. temperature (°C) 150- 140- 130- 120- 110- 100 90 80- 70- 60 50 0 heat added (kJ/mol) 10. X

A reaction at 32.0 degrees Celsius evolves 882. mmol of carbon dioxide gas. Calculate the volume of carbon dioxide gas that is collected . You can assume the pressure in the room is exactly 1 atm.

The pressure of a gas is measured as 60. torr. Represent this pressure in atmospheres. (1 atm = 760 torr) Show work.

Нурothesis Theory Law Answer Bank Scientists, after many experiments, An untested explanation. An explanation that has been A doctor thinks, but has explain how the temperature of a gas tested and verified. not verified, why a patient depends on the energy of its molecules. has stomach pain. A description that predicts what happens, but does not explain how.

Please answer number 5. Here is the complete question #5. 5.) In a car engine, a 425 mL cylinder and piston system is filled with a mixture of 0.83 g and 0.37 g of octane and oxygen gas, respectively. Both gases are at a temperature of 28 °C. If the total gas mixture is compressed to a pressure of 5.2 atm before combustion, calculate the total volume of the gas mixture at this point in time.

Classify each situation by the equation that would quantify it. a. A container of ammonia cleaner is stored in the janitor's closet off a lecture hall after being used at night for cleaning. The container has a very small hole in the lid. The next morning the entire lecture hall smells of ammonia. How would you calculate the speed of the ammonia molecules as they move out into the lecture hall? b. The pressure on a tire pump is read. The handle of the pump is pushed down as far as possible. The reading of the pressure on the gauge is taken again. How would you calculate the final pressure? c. The burner under a hot air balloon is ignited and the balloon expands. How would you calculate the expanded volume of the balloon? d. A front-end collision causes the air bag in an automobile to deploy by the reaction of sodium azide to produce nitrogen gas. How would you calculate how much sodium azide is needed to fill a standard size bag with nitrogen under STP conditions? e. Aerosol cans have…

How many grams of argon gas are needed to have 5.15 mol of argon gas? 1.822.97g 2.205.74g 3.102.87g 4.411.49g 5.5.15g