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| A car wastes (25/50/75) percent of the energy produced from the burning of gasoline. |
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Definition
| 75% waste, through heat and friction. |
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Ethanol has a heat of combustion of 1407 kJ/mole. How much energy is released from the burning of 18.0 grams of ethanol?
hint - you need to know the molecular formula of ethanol. |
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The recommended daily intake of copper is 3 mg per day. In the course of a lifetime, 80 years, how many grams of copper does this daily intake add up to?
SHOW DIMENSIONAL ANALYSIS WORK! |
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The specific heat of liquid water is 4.2 J per gram per degree celsius, while the specific heat of ice is 2.0 J per gram per degree celsius.
If you have equal masses of liquid water and ice, and give each sample 25 J of energy, which sample will change its temperature more? |
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Definition
The ice.
Think of specific heat as a measure of resistance to temperature change. The smaller the specific heat, the smaller the resistance to temperature change. |
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Term
| A molecule's energy is found in its ___________. |
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The density of water is 1.0 g/mL. Convert this value to mg/L.
SHOW DIMENSIONAL ANALYSIS WORK. |
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A potato chip burns and raises the temperature of 95 g of water from 8 to 29 °C. The mass of the potato chip decreases by 0.86 g. Calculate the heat of combustion (in units of kJ/g) of the potato chip.
The specific heat of water is 4.2 J per gram per °C. |
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How many liters of crude oil are in 1 barrel of crude oil?
Useful conversions: 4 qt = 1 gallon, 0.946 L = 1 qt, 1 barrel = 42 gallons
SHOW DIMENSIONAL ANALYSIS WORK
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| A candle burns, and its mass drops by 0.85 grams. Where did the mass go? |
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Definition
When a candle burns, the wax reacts with oxygen in the air to produce CO2 and H2O.
The lost mass can be found in the mass of the CO2 and H2O produced. |
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Term
| The heat of combustion of butane is 2859 kJ/mol. Write a balanced thermochemical equation. |
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Definition
| 2 C4H10 + 13 O2 → 8 CO2 + 10 H2O + 5718 kJ |
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The heat of combustion of butanol is 2713 kJ/mole. Write a balanced thermochemical equation.
Hint: you need to figure out the molecular formula of butanol first. |
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Definition
| 1 C4H10O + 6 O2 → 4 CO2 + 5 H2O + 2713 kJ |
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Term
| When water absorbs energy, the temperature of the water (incerases/decreases) and the process is (exo/endo) thermic. |
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Term
Which water flow rate measurement is larger:
1 cL/min or 450 cL/hour? |
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Definition
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Term
| How many centiliters are in 1 mL? |
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Definition
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Term
| The products of a combustion reaction have (more/less) energy than the reactants. |
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Definition
| Since the reaction is exothermic (all combustion reactions are exothermic) the answer is less. |
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Term
| Combustion reactions are (exo/endo)thermic. |
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Term
8,500 J of energy is released by a 14 gram water sample. What temperature change does it undergo?
The specific heat of water is 4.2 J per gram per °C. |
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Crude oil is a (renewable/nonrenewable) resource because________________.
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| Nonrenewable, because the natural processes of the Earth do not produce crude oil in a reasonable time frame. It takes millions of years to decompose organic matter into crude oil. |
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| All reactions require a certain amount of energy to start. This energy is called the _____________. |
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Term
Convert a water flow rate of 4.2 liters per hour to units of centiliters per second. |
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Term
The mass of an electron is 9.11 x 10-28 grams. Convert this mass to pounds.
Useful conversion: 1 kg = 2.2 pounds |
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Definition
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| Butane has a density of 0.57 g/mL. Butane's heat of combustion is 49.3 kJ/g. How much energy would 5.5 mL of butane release? |
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| The specific heat of stainless steel is 0.51 J per gram per degree Celsius. A 15 gram sample changes its temperature from 40 °C to 80 °C. How much energy was (absorbed/released)? |
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| Draw an enthalpy diagram for a reaction having a ΔH of +30 kJ, EA = 40 kJ, and a product energy of 50 kJ. |
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Definition
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Definition
1. 15 kJ
2. -15 kJ
3. 40 kJ |
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| Water has a (low/high) specific heat capacity. |
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Definition
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Term
| In the equation q=mCΔT, the symbol for heat energy is |
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Definition
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| In the equation q=mCΔT, the symbol for specific heat capacity is |
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Definition
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| The molecular formula of ethane is |
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Definition
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| The molecular formula of butyne is |
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Definition
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| The molecular formula of propene is |
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Definition
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Write the thermochemical equation for the combustion of propene.
The molar heat of combustion of propene is 1924 kJ/mole. |
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Definition
2 C3H6 + 9 O2 → 6 CO2 + 6 H2O + 3848 kJ |
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The molar heat of combustion of propene is 1924 kJ per mole. How many molecules of propene are needed to produce 73 kJ of energy?
hint: you will need the mole to particle conversion here. |
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| An unknown metal with a mass of 26.5 g absorbs 1200 J of energy, and the temperature rises from 25 ºC to 138 ºC. What is the specific heat capacity of this metal? |
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| The specific heat of sand is 0.9 J per gram per degree Celsius. If 4,500 J of energy are added to a 150 gram sample of sand, by how much does the temperature rise? |
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