A container is filled with a sample of an ideal gas at a pressure of 1.5 atm. The gas is compressed isothermally to one-fourth of its original volume. What is the new pressure of the gas in atmospheres? A 3 B 1 C 4 D 6 8.

A container of N,0,(g) has a pressure of 0.445 atm. When the absolute temperature of the N,O,(g) is tripled, the gas completely decomposes, producing NO, (g) and NO(g). Calculate the final pressure of the gas mixture, assuming that the container volume does not change. final pressure: atm

#13: Two containers of identical volume are connected by a tube with a stopper to prevent gases inside the tanks from mixing with each other. Container A has a pressure of 2.00 atm and a volume of 10.0 L while container B has a pressure of 4.00 atm and a volume of 10.0 L. Both containers have an initial temperature of 27.0 °C and were then heated to 127 °C. Upon reaching 127 °C, the stopper was released. What is the new pressure in both containers after the stopper was released?

A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.