Chemistry Chapter 6 Homework Assignment

A goose is flying south for the winter at a constant speed. Keep in mind that one mile is 1.61 km , and one pound is 454 g . The goose has a mass of 21.4 lb (pounds) and is flying at 10.7 miles/h (miles per hour). What is the kinetic energy of the goose in joules?

111 J

An ideal gas (which is is a hypothetical gas that conforms to the laws governing gas behavior) confined to a container with a massless piston at the top. (Figure 2) A massless wire is attached to the piston. When an external pressure of 2.00 atm is applied to the wire, the gas compresses from 6.40 to 3.20 L . When the external pressure is increased to 2.50 atm, the gas further compresses from 3.20 to 2.56 L . In a separate experiment with the same initial conditions, a pressure of 2.50 atm was applied to the ideal gas, decreasing its volume from 6.40 to 2.56 L in one step. If the final temperature was the same for both processes, what is the difference between q for the two-step process and q for the one-step process in joules? Express your answer with the appropriate units.

162 J

Suppose that a person eats a diet of 2381 Calories per day. Convert this energy into kWh.

2.767 kWh

For the reaction given in Part A, how much heat is absorbed when 2.50 mol of A reacts? Express your answer to three significant figures and include the appropriate units.

321 kJ

Suppose that a person eats a diet of 2381 Calories per day. Convert this energy into J.

9.962×106 J

Suppose that a person eats a diet of 2381 Calories per day. Convert this energy into kJ.

9962 kJ

Assuming constant pressure, rank these reactions from most energy released by the system to most energy absorbed by the system, based on the following descriptions: Surroundings get colder and the system decreases in volume. Surroundings get hotter and the system expands in volume. Surroundings get hotter and the system decreases in volume. Surroundings get hotter and the system does not change in volume. Also assume that the magnitude of the volume and temperature changes are similar among the reactions. Rank from most energy released to most energy absorbed. To rank items as equivalent, overlap them.

Most energy released B D C A Most energy absorbed

Classify the following by the sign of ΔE for the system. Drag the appropriate items to their respective bins. If no definitive classification can be made, drag the item into the bin labeled "Not enough data."

Negative - the system expands and the surroundings get hotter Positive - the system contracts and the surrounding get colder Not enough data - the system contracts and the surroundings get hotter - the system expands and the surroundings get colder

What is the SI unit of energy?

joule

List some other common units of energy. Check all that apply.

kilowatt-hour calorie

An ideal gaseous reaction (which is a hypothetical gaseous reaction that conforms to the laws governing gas behavior) occurs at a constant pressure of 50.0 atm and releases 63.1 kJ of heat. Before the reaction, the volume of the system was 7.60 L . After the reaction, the volume of the system was 3.00 L . Calculate the total internal energy change, ΔE, in kilojoules. Express your answer with the appropriate units.

ΔE = -39.9 kJ

A mole of X reacts at a constant pressure of 43.0 atm via the reaction X(g)+4Y(g)→2Z(g), ΔH∘=−75.0 kJ Before the reaction, the volume of the gaseous mixture was 5.00 L. After the reaction, the volume was 2.00 L. Calculate the value of the total energy change, ΔE, in kilojoules. Express your answer with the appropriate units.

ΔE = -62.0 kJ

Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)→NO2(g), ΔH∘A=33.2 kJ 12N2(g)+12O2(g)→NO(g), ΔH∘B=90.2 kJ Express your answer with the appropriate units.

ΔH∘ = -114.0 kJ

Calculate the enthalpy of the reaction 4B(s)+3O2(g)→2B2O3(s) given the following pertinent information: B2O3(s)+3H2O(g)→3O2(g)+B2H6(g), ΔH∘A=+2035 kJ 2B(s)+3H2(g)→B2H6(g), ΔH∘B=+36 kJ H2(g)+12O2(g)→H2O(l), ΔH∘C=−285 kJ H2O(l)→H2O(g), ΔH∘D=+44 kJ Express your answer with the appropriate units.

ΔH∘ = -2552 kJ

Calculate the standard enthalpy change for the reaction 2A+B⇌2C+2D Use the following data:

ΔH∘rxn = 257 kJ