Hydrogen gas can be formed by the reaction of methane with water according to the following reaction:  CH4(g) + H2O(g) --> CO(g) +3H2(g) In a particular sample, 25.5 L of methane gas (measured at 0.963 atm and 298 K) is mixed with 22.8 L of water vapor (measured at 0.924 atm and 398 K). The reaction generates 26.2 L of di-hydrogen gas at STP. What is the percent yield of the reaction?

For many purposes we can treat butane (C,H10) as an ideal gas at temperatures above its boiling point of – 1. °C. 3 Suppose the pressure on a 8.0 m° sample of butane gas at 11.0°C is reduced to one-third its initial value. O yes Is it possible to change the temperature of the butane at the same time such that the volume of the gas doesn't change? olo O no If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C. Explanation Check © 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility

Questions 7 through 11 refer to the information and diagram below. 2 NO2(g) > N204(g) NO2(8) reacts to form N20a(g) according to the equation above. A pure sample of NO2(g) is placed into a rigid, evacuated 0.500 L container. The initial pressure of the NO2(g) is 960 torr. The temperature is held constant until the NO2(g) reaches equilibrium with its product. The figure below shows how the pressure of the system changes while reaching equilibrium. Pressure (torr) 960 760 Time 8. The pressure vs. time curve can be used to evaluate (A) only the value of Q. (B) only the equilibrium constant from the horizontal part. (C) only the kinetics of the reaction from the decreasing part. (D) the kinetics of the reaction from the decreasing part and the equilibrium constant from the horizontal part.

For the following reaction: C3H8(g) + 3CO₂(g) + 4H₂O(1) 502(g) The change in gaseous moles, An = To maximize the product yield, the volume of the container should ◆ , so that the pressure will be (> →