# Question: Consider two gases A and B each in a 1 0

Consider two gases, A and B, each in a 1.0- L container with both gases at the same temperature and pressure. The mass of gas A in the container is 0.34 g, and the mass of gas B in the container is 0.48 g.

a. Which gas sample has the most molecules present? Explain.

b. Which gas sample has the largest average kinetic energy? Explain.

c. Which gas sample has the fastest average velocity? Explain.

d. How can the pressure in the two containers be equal to each other since the larger gas B molecules collide with the container walls more forcefully?

a. Which gas sample has the most molecules present? Explain.

b. Which gas sample has the largest average kinetic energy? Explain.

c. Which gas sample has the fastest average velocity? Explain.

d. How can the pressure in the two containers be equal to each other since the larger gas B molecules collide with the container walls more forcefully?

**View Solution:**## Answer to relevant Questions

Consider the following samples of gases at the same temperature. Arrange each of these samples in order from lowest to highest. a. Pressure b. Average kinetic energy c. Density d. Root mean square velocity Some samples of ...Draw a qualitative graph to show how the first property varies with the second in each of the following (assume 1 mole of an ideal gas and T in kelvins). a. PV versus V with constant T b. P versus T with constant V c. T ...Calculate the pressure exerted by 0.5000 mole of N2 in a 1.0000- L container at 25.0oC. (See Table) a. Use the ideal gas law. b. Use the van der Waals equation. c. Compare the results from parts a and b. Table Calculate the root mean square, the most probable, and the average velocities for N2(g) at 227oC. Atmospheric scientists often use mixing ratios to express the concentrations of trace compounds in air. Mixing ratios are often expressed as ppmv (parts per million volume): ppmv of X = vol of X at STP total vol of air at ...Post your question