Manganese (Mn), a metal used in alloys, melts at 2275 °F. What is this temperature in kelvins, rounded to the nearest kelvin?

Which statement or model does NOT belong to the kinetic molecular theory of an ideal gas?

A fixed amount of ideal gas occupies 44.8 L at 4.00 atm. What is its pressure after isothermal compression to 22.4 L? Use 1 atm = 760 mmHg.

A fixed amount of ideal gas occupies 4.4 L at 27 °C. It is cooled to 0 °C at constant pressure under a movable piston. What is its final volume? Use the approximation T(K) ≈ t(°C) + 273.

A fixed amount of ideal gas in a rigid cylinder has a pressure of 30.0 atm at 240 K. What is its pressure, in torr, when heated to 400 K? Use 1 atm = 760 torr.

A fixed amount of ideal gas initially occupies 2.00 L at 3.00 atm and 25 °C. Its pressure and volume change to 12.0 atm and 1.00 L. What is its approximate final temperature? Use the approximation T(K) ≈ t(°C) + 273.

A sealed balloon contains an ideal gas at 2.000 atm, 200.0 L, and 27.0 °C. What is its volume when the pressure becomes 4.000 atm and the temperature becomes 47.0 °C? Use the approximation T(K) ≈ t(°C) + 273.

In a hypothetical ideal-gas model, 6.0 mol of gas occupies 3.0 L at 2.0 atm. At the same temperature, what pressure would 3.0 mol of the gas exert in 6.0 L?

A 96.0 g sample of an ideal gas occupies 73.8 L at 27 °C and 760 mmHg. Which gas is consistent with its calculated molar mass? Use R = 0.0820 L·atm/(mol·K), 760 mmHg = 1 atm, and the approximation T(K) ≈ t(°C) + 273.

Each ideal-gas sample below occupies the same volume at the same pressure. Which sample has the highest temperature?

An ideal, nonreacting gas mixture contains 2.00 mol of O₂, 1.00 mol of CO₂, and 3.00 mol of N₂ in a 20.0 L flask at 0 °C. What is its total pressure? Use R = 0.0820 L·atm/(mol·K). Use the approximation T(K) ≈ t(°C) + 273.

An ideal, nonreacting mixture of 32.0 g of methane and 44.0 g of carbon dioxide occupies 44.8 L at 5.00 atm. What is its temperature? Use molar masses of 16.0 g/mol for CH₄ and 44.0 g/mol for CO₂, and R = 0.0820 L·atm/(mol·K).

A 34.0 g sample of NH₃, treated as an ideal gas, occupies 44.8 L at 1.00 × 10³ mmHg. What is its approximate temperature in degrees Celsius? Use M(NH₃) = 17.0 g/mol, R = 0.0820 L·atm/(mol·K), and 760 mmHg = 1 atm. For this estimate, use t(°C) ≈ T(K) − 273.

What is the density, in g/L, of ideal CO₂ gas at 3.00 atm and 27 °C? Use M(CO₂) = 44.0 g/mol and R = 0.0820 L·atm/(mol·K). Use the approximation T(K) ≈ t(°C) + 273.

An ideal O₂ gas sample has a density of 4.3 g/L at 0 °C. What is its approximate pressure? Use M(O₂) = 32.0 g/mol and R = 0.0820 L·atm/(mol·K). Use the approximation T(K) ≈ t(°C) + 273.

An ideal gas has a density of 3.2 g/L at STP, defined here as 0 °C and 1 atm. Which gas is consistent with this density? Use a molar volume of approximately 22.4 L/mol.

A 56.0 g sample of an ideal molecular gas has a density of 5.00 g/L at STP (0 °C and 1 atm). How many molecules does it contain? Use a molar volume of 22.4 L/mol and N_A = 6.02 × 10²³ mol⁻¹.

At the same temperature, which gas has the greatest root-mean-square particle speed?

For which pair of gases is the ratio of the faster effusion rate to the slower effusion rate greatest? Compare the gases at the same temperature and pressure through identical small openings. Use approximate molar masses: H₂ = 2, He = 4, Ar = 40, CO₂ = 44, N₂ = 28, and O₂ = 32 g/mol.

An unknown gas effuses twice as fast as SO₂ at the same temperature and pressure through identical small openings. What is its molar mass? Use M(SO₂) = 64.0 g/mol.

The ideal gases in the rigid bulbs shown are nonreacting and initially at the same temperature. The temperature remains constant when the stopcock opens, and the connecting tube’s volume is negligible. What is the final partial pressure of gas A?

The ideal gases in the rigid bulbs shown are nonreacting and initially at the same temperature. The temperature remains constant when the stopcock opens, and the connecting tube’s volume is negligible. What is the final total pressure?

An ideal gas mixture contains 2.00 mol of H₂, 3.00 mol of NH₃, and 4.00 mol of O₂ at a total pressure of 7.00 atm. Assuming no reaction occurs, what is the partial pressure of H₂?

An ideal, nonreacting gas mixture contains 28.0 g of CO, 34.0 g of NH₃, and 10.0 g of H₂. What is its total pressure if the partial pressure of NH₃ is 5.00 atm? Use molar masses of 28.0, 17.0, and 2.00 g/mol, respectively.

An ideal mixture contains only N₂ and CO₂, with partial pressures of 3.00 atm and 5.00 atm, respectively. What is the mole fraction of N₂?

Sodium azide was used to generate nitrogen in some older automobile airbags. What mass of NaN₃ is needed to produce 44.8 L of N₂ at STP (0 °C and 1 atm), assuming complete reaction? Use a molar volume of 22.4 L/mol and M(NaN₃) = 65.0 g/mol.
2 NaN₃(s) → 2 Na(s) + 3 N₂(g)

After 651 g of solid HgO decomposes completely on heating, the oxygen is collected at 1.20 atm and 25 °C. What volume of O₂ is collected? Use the rounded molar mass M(HgO) = 217 g/mol, R = 0.0820 L·atm/(mol·K), and T(K) ≈ t(°C) + 273. The net reaction, with mercury shown in its collected liquid state, is:
2 HgO(s) → 2 Hg(l) + O₂(g)

A 56.0 g sample of N₂ reacts completely with excess H₂, producing NH₃ that occupies 44.8 L at 0 °C. Assuming ideal-gas behavior and quantitative yield, what is the NH₃ pressure? Use M(N₂) = 28.0 g/mol, R = 0.0820 L·atm/(mol·K), and T(K) ≈ t(°C) + 273.
N₂(g) + 3 H₂(g) → 2 NH₃(g)