How many collisions does single Ar atom make in 1.0 s when the temperature is 25 degrees Celsius and the pressure is (i) 10 atm, (ii) 1.0 atm? (Ar: M= 39.95×10^-3 kg/mol

please explain

The reaction CO (g) + H2O(g)    CO2(g) 2 + H2(g) has ΔH = -41 kJ/mol. Does the amount of H2 in an equilibrium mixture increase or decrease when the temperature is decreased?

STP (standard temperature and pressure) is used as a reference point for the molar volume of an ideal gas. In the USA, most chemists, most general chemistry texts, and OWL use STP =0°C, 1 atm, where the molar volume = 22.4 L/mol. If the reference pressure is chosen to be 1 bar, the molar volume is 22.7 L/mol. Do not confuse the two. A 0.99 mol sample of hydrogen gas occupies a volume of L at STP.

A sample of helium is initially at 605 torr in a volume of 2.85 L. At 24.7 °C you found the density of He to be 0.130 g/L and the density of Ar to be 1.30 g/L even though both samples had the same number of moles. Which one of the following best explains why the densities are different? A B C D Argon is a heavier atom than helium, so it has more mass in the same volume occupied by the gas. Argon is a larger atom than helium so it occupies more volume. An argon atom is more dense than a helium atom. The densities are different only because of rounding.

For the gas - phase equilibrium A(g) + 2 B(g) = C(g) the initial partial pressures of A, B, and C are all 0.300 atm. After equilibrium is established at 25 \deg C, it is found that the partial pressure of C is 0.220 atm. What is AG\deg for this reaction? (R = 8.314 J/mol ·K).

At 25.0 °C the Henry's Law constant for dinitrogen monoxide (N,0) gas in water is 0.025 M/atm. Calculate the mass in grams of N,0 gas that can be dissolved in 450. mL of water at 25.0 °C and a N,0 partial pressure of 1.31 atm. Be sure your answer has the correct number of significant digits. ?