Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Chapter 19, Problem 19.44E
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Iron metal reacts with oxygen gas to produce iron(III) oxide. What will be the effect of increasing the pressure of oxygen gas in a closed reaction vessel?
There is no effect; a catalyst is needed.
More iron oxide will be produced.
The rate of production of iron oxide will slow down.
Less reaction will take place.
The reaction mixture will catch fire.
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Consider the reaction: NO2(g) + CO(g) -->NO(g) + CO2(g).
Could you follow the progress of this reaction by monitoring the pressure of the gas in the container in which it was occurring?
Chapter 19 Solutions
Physical Chemistry
Ch. 19 - Prob. 19.1ECh. 19 - What is the kinetic energy of a single atom of...Ch. 19 - Prob. 19.3ECh. 19 - One mole of Ne atoms confined to a volume of 10.0L...Ch. 19 - Prob. 19.5ECh. 19 - Prob. 19.6ECh. 19 - Prob. 19.7ECh. 19 - Prob. 19.8ECh. 19 - Prob. 19.9ECh. 19 - Prob. 19.10E
Ch. 19 - Prob. 19.11ECh. 19 - Interstellar space can be considered as having...Ch. 19 - Prob. 19.13ECh. 19 - SF6 is a gas at room temperature, 295K. What is...Ch. 19 - Prob. 19.15ECh. 19 - Prob. 19.16ECh. 19 - If relativistic effects were ignored, what...Ch. 19 - Prob. 19.18ECh. 19 - Prob. 19.19ECh. 19 - Prob. 19.20ECh. 19 - Prob. 19.21ECh. 19 - Prob. 19.22ECh. 19 - Prob. 19.23ECh. 19 - Prob. 19.24ECh. 19 - What is the ratio of vrms/vmostprob for any gas at...Ch. 19 - Prob. 19.26ECh. 19 - Prob. 19.27ECh. 19 - Prob. 19.28ECh. 19 - Prob. 19.29ECh. 19 - Prob. 19.30ECh. 19 - Prob. 19.31ECh. 19 - The previous exercise gives an expression for...Ch. 19 - Prob. 19.33ECh. 19 - Prob. 19.34ECh. 19 - Prob. 19.35ECh. 19 - What must the pressure be if the mean free path of...Ch. 19 - Prob. 19.37ECh. 19 - Prob. 19.38ECh. 19 - Prob. 19.39ECh. 19 - Explain why the molecular diameter for argon, at...Ch. 19 - Prob. 19.41ECh. 19 - Prob. 19.42ECh. 19 - Prob. 19.43ECh. 19 - A 1.00-mol sample of Xe gas is kept at a...Ch. 19 - Prob. 19.45ECh. 19 - Prob. 19.46ECh. 19 - Prob. 19.47ECh. 19 - Prob. 19.48ECh. 19 - Prob. 19.49ECh. 19 - Consider a gas mixture containing equal...Ch. 19 - The inverse of the collision rate, 1/z, is the...Ch. 19 - Prob. 19.52ECh. 19 - Prob. 19.53ECh. 19 - Prob. 19.54ECh. 19 - Prob. 19.55ECh. 19 - Estimate the rate at which Hg effuses out a hole...Ch. 19 - Prob. 19.57ECh. 19 - Knudsen effusion cells are used to determine vapor...Ch. 19 - Prob. 19.59ECh. 19 - Prob. 19.60ECh. 19 - Prob. 19.61ECh. 19 - Prob. 19.62ECh. 19 - Prob. 19.63ECh. 19 - Prob. 19.64ECh. 19 - Prob. 19.65ECh. 19 - Prob. 19.66ECh. 19 - Prob. 19.67ECh. 19 - Prob. 19.68ECh. 19 - Prob. 19.69ECh. 19 - Prob. 19.70ECh. 19 - Prob. 19.71ECh. 19 - Prob. 19.72ECh. 19 - Prob. 19.73E
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- Consider a gas mixture containing equal concentrations of argon and helium. Without performing any calculations, determine which is higher: the number of collisions between helium and helium, the number of collisions between argon and argon, or the number of collisions between helium and argon?arrow_forwardUse the kinetic theory to justify the following observations: (a) the rate of a reaction in the gas phase depends on the energy with which two molecules collide, which in turn depends on their speeds; (b) in the Earth’s atmosphere, light gases, such as H2 and He, are rare but heavier gases, such as O2, CO2, and N2, are abundant.arrow_forwardWhich of the following reactions, carried out in a closed container, will result in a reduced total pressure? a. CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) b. 2N2O(g) → 2N2(g) + O2(g) c. 2HI(g) → H2(g) + I2(g) d. 2H2(g) + O2(g) → 2H2O(l) e. None of these reactions will result in a pressure reduction.arrow_forward
- Which of the following reactions, carried out in a closed container, will result in a reduced total pressure? Select one: O a. CH4(g) + 202(g) → CO2(g) + 2H2O(g) b. 2N20(g) → 2N2(g) + O2(g) c. 2HI(g) → H2(g) + I2(g) O d. 2H2(g) + O2(g) 2H20() e. None of these reactions will result in a pressure reduction.arrow_forward7. What does the variable 'R' represent in regards to gas laws? Ideal gas constant Reaction rate Real temperature Real pressurearrow_forward19. This reaction occurs in a closed container: A (g) + 2 B (g) → 2 C (g) A reaction mixture initially contains 1.5 mol of A and 2.0 mol of B. Assuming that the volume and temperature of the reaction mixture is constant, how does the pressure change, and what is the percentage change if the reaction goes to completion.arrow_forward
- 8. What Is the difference between high and low pressure? In high pressure, there are more particle collisions happening than in low pressure. In low pressure, there are more particle collisions happening than in high pressure. There are the same number of particle collisions in high and low pressure. Pressure is not caused by the collisions of particles.arrow_forwardA reaction at −9.0°C evolves 815.mmol of chlorine pentafluoride gas. Calculate the volume of chlorine pentafluoride gas that is collected. You can assume the pressure in the room is exactly 1atm. Be sure your answer has the correct number of significant digits.arrow_forwardCalculate the collision frequency, z, and the collision density, ZAA, in carbon monoxide, d = 360 pm, at 30 °C and 120 kPa. What is the percentage increase when the temperature is raised by 10 K at constant volume?arrow_forward
- The generic reaction occurs in a closed container: 2A(g) +Big) → 2Cg) A reaction mixture initially contains 2.0L of gas A and 1.5L of gas B. Assuming that the volume and temperature of the reaction mixture remain constant, what is the precent change in pressure if the reaction goes to completion?arrow_forwardA mixture of ideal gases having a total mass of 35 g is placed in a 13 L vessel at 269.0 K. The equilibrium pressure is measured to be 1.6 bar. Calculate the average molar mass of the gas mixture.arrow_forwardRobert Boyle, in his discovery of the “spring of the air, “ was working on the property of gases called compressibility. The compressibility of gases is extreme to that of liquids, like brake fluid and water. Briefly describe the mechanism of what really happens when you compress a gas.arrow_forward
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