| A | B |
|---|
| A sample of SO2 gas has a volume of 1.16 L at a temperature of 23 degrees celcius. At what temperature will the gas have a volume of 1.25 L ? | 46 degrees Celcius |
| A sample of ammonia gas occupies a volume of 1.58 L at 22.0 degrees celcius and a pressure of 0.983 atm. What volume will the sample occupy at 1.00 and zero degrees celcius ( that is, at STP) ? | 1.44 L |
| A student collects 285 mL of O2 at a temperature of 15.0 degrees celcius and a pressure of 99.9 kPa. The next day the sample occupies 292 mL at a temperature of 11.0 degrees celcius. What is the new pressure of the gas? | 96.2 kPa |
| A sample of gas at 2.50 atm and 6.50 L is COMPRESSED to 1.50 L at a constant (not changing) temperature. What is the new pressure? | 10.8 atm |
| A sample of gas at 255 K occupies a volume of 1.55 L . If the temperature is raised to 298 K what will the be the new volume? | 1.81 L |
| You have 200.0 cubic centimeters of nitrogen ( IV ) oxide at a temperature of 303.0 K and a pressure of 101.0 kPa. What volume will the NO2 occupy at 255.0 kPa and 371.0 K ? | 96.99 cc ( cubic centimeters) |
| A container of gas at 550.0 mm Hg and 35.0 degrees celcius is heated to 60.0 degress celcius. What is the pressure in mm Hg ? | 595 mm Hg |
| A gas at 925.0 mm Hg pressure and 50.00 degrees celcius is cooled to -25.00 degrees celcius. What is the final pressure in mm Hg ? | 710.2 mm Hg |
| What is the final pressure in atm if 5.25 L of a gas at 75.00 degrees celcius and 1.33 atm pressure is COMPRESSED to 2.75 L at 1.55 degress celcius ? | 3.12 atm |
| What pressure will be needed to change the volume of 22.4 L of helium at 25.0 kPa to a volume of 85.0 L ? | 6.59 kPa |
| A sample of SO2 gas has a volume of 9.50 L at a temperature of 320 K. At what temperature will the gas have a volume of 2.55 L ? | 86 K |
| A sample of ammonia gas occupies a volume of 27.4 L at 14.0 degrees celcius and a pressure of 1.20 atm. What volume will the sample occupy at 3.00 atm and 0 (zero) degrees celcius ? | 10.4 L |
| A student collects 355 mL of O2 gas at a temperature of 27 degrees celcius and a pressure of 127 kPa. The next day the sample occupies 257 mL at a temperature of 17 degrees celcius, what is the new pressure of the gas? | 1.7 x 10^2 kPa |
| What type of reactions occur when MORE ENERGY is released in the FORMING of new bonds than is required to break bonds formed in the products? | EXOthermic |
| What type of reaction occurs more when MORE ENERGY is REQUIRED to break existing bonds in reactants than is released when new bonds are formd in the products? | ENDOthermic |
| What type of reaction RELEASES ENERGY to its surrounding? | EXOthermic |
| What type of Energy change is shown in the following chemical reaction(equation)? Sn + Cl2 >>> SnCl2 with Change Heat equals -325 KJ . | EXOthermic |
| A 50.6 g sample of iron metal is heated from 19.7 degres celcius to 24.3 degres celcius. How many joules of heat will be absorbed? (***Recall that the SPECIFIC HEAT of iron is 0.4494 Joules/(degees Celcelcius x grams) ***) | 105 J |
| A sample of an unknown metal has a mass of 120.7 grams. As the sample cools from 90.5 degrees celcius to 25.7 degres celcius, it RELEASES 7020 J of energy. What is the SPECIFIC HEAT of the sample? ( ***Recall that Specific Heat is the amount of heat required to raise a UNIT of mass of homogeneous material exactly 1 K or 1 degree unit celcius in a very specific way given CONSTANT PRESSURE and VOLUIME***) | 0.898 Joules/(degrees celcius x grams) |
| A silver bar with a mass of 250.0 g is heated from 22.0 degrees celcius to 68.5 degrees celcius. How much heat does the silver bar absorb? Note that the Specific Heat of Silver is 0.235 Joules/ ( degrees Celcius x grams) | 2730 J |
| If the temperature of 34.4 g of ethanol increases from 25.0 degrees celcius to 78.8 degrees celcius, how much heat has been absorbed by the etanol? ( The specific heat of ethanol is 2.44 Joules/ ( degrees Celcius x grams) ) | 4520 J |
| The temperature of a sample of iron with a mass of 10.0 g changed from 50.4 degrees celcius to 25.0 degrees celcius with the RELEASE of 114 J of heat. What is the Specific Heat of iron? | 0.449 Joules/ ( Degrees Celcius x grams) |
| The specific heat of ethanol is 2.44 Joules / (Degrees celcius x grams). How many joules of energy are required to heat 50.0 g of etahanol from -20.0 degrees celcius to 68.0 degrees celcius? | 10700 J |
| How much heat does it take to warm 16.0 g of PURE WATER from 90 degrees celcius to 100 degrees celcius? The specific heat of water is 4.180 Joules / (Degrees Celcius x grams) | 669 J |
| How much heat does it take to warm 50.00 g of pure water from 20.00 degrees celcius to 80.00 degrees celcius? Again, the specific heat of water is 4.180 joules/ (degrees celcius x grams) | 12540 J |
| If the temperature of 56.2 g ethanol increases from 75.1 degrees celcius to 89.3 degrees celcius, how much heat has been absorbed by the ethanol? ***Note that the specific heat of etanol is 2.44 joules/ (degrees celcius x grams) *** | 1950 J |
| The temperature of a sample of water increases from 20.00 degrees celcius to 46.6 degrees celcius as it absorbs 5650 J of heat. What is the MASS of the sample? Note that water's specific heat is 4.18 joules/ (degrees celcius x grams) | 50.8 g |
