if the density of water is 1.00g/ml and desity of density of mercury is 13.6g/mL,how high a coloumn of water in meters can be supported by standard atmospheric pressure?by 1 bar?

For an ideal gas, calculate the following quantities.(a) The pressure of the gas if 0.135 mol occupies 207 mL at 25°C. atm(b) The temperature (in kelvins) at which 0.0250 mol occupies 1.00 L at 0.583 atm. K(c) The number of moles in 3.00 L at -7°C and 725 torr. Remember 1atm = 760 torr. mol(d) The volume occupied by 4.72  10-3 mol at 40.°C and a pressure of 1.57 kPa. Remember 1 atm = 101.325 kPa

(a) (c) A column of water in a buret is 336 mm Hg high. How high would that column be if it were mercury instead of water? (d) In order for the pressures to be equal, density and height of a column are inversely proportional, therefore the following relationship applies: (denHg)(hHg) = (denH20)(hH20) Note: the density of mercury is 13.6 g/mL and the density of water is 1.00 g/mL. An electrolysis experiment was run for 15 minutes and 45 seconds at an average current of 189 milliamps (mA). The mass lost by the copper anode was 0.0589 grams. (b) Calculate the number of coulombs transferred. (Remember: coulomb = amps x sec) Show full calculation of the height in mercury (remember to use proper significant figures.) Calculate the moles of copper lost from the anode. Based on the moles of copper lost determined in 1c, calculate the moles of electrons transferred. Remember, the reaction at the copper anode is: Cu(s)---> Cu¹² (aq) + 2 e

.0380 of Mg strip reacted completely with 6 M HCL in the gas buret and 35.8 mL of hydrogen gas is collected over water at 20 c. The pressure of the "wet" hydrogen gas is adjusted to the outside atmospheric tempertature, a pressure of 747.50 torr. The vapor pressure of water at 20 c is 17.54 torr. using the volume of hydrogen gas collected and the universal gas law, PV = nRT, where R is the gas constant 0.08206 L•atm/mol•K, calculate the experimental number of moles of hydrogen produced.

The solubility of N, in blood can be a serious problem (the "bends") for divers breathing compressed air (78% N, by volume) at depths greater than 50. ft. Find the volume (in mL) of N2, measured at 25 °C and 1.00 atm, released per liter of blood when a diver at a depth 50. ft rises to the surface. The total pressure (water weight plus atmospheric pressure) on the diver at 50. ft is 2.47535 atm. (kH, for N, in water at 25 °C is 6.6 × 10^-4) Be sure to use the correct number of significant figures.

When 3.50 g of Ba(s) is added to 100.00 g of water in a container open to the atmosphere, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 47.40°C. If the specific heat of the solution is 4.18 J/(g ⋅ °C), calculate ΔH for the reaction, as written. Ba(s) + 2 H2O(l) → Ba(OH)2(aq) + H2(g)       ΔH = ?

(a) A piston at 5.7 atm contains a gas that occupies a volume of 3.5 L. What pressure would have to be placed on the piston to force the volume to adjust to 1.54 L? atm(b) A piston at 63.0°C contains a gas that occupies a volume of 2.5 L. To what temperature would the gas have to be heated to increase the volume to 4.1 L at constant pressure? °C(c) A piston at 7395 torr contains a gas that occupies a volume of 4.7 L. What pressure would have to be placed on the piston to force the volume to adjust to 1.69 L? atm

(b) If a 2.302g sample of impure cobalt(III) carbonate is heated, and 415mL of carbon dioxide is collected at 23°C and a pressure of 1.512atm, what is the percent cobalt(III) carbonate in the sample? (b) If a 2.302 g sample of impure cobalt(III) carbonate is heated, and 415 mL of carbon dioxide is collected at 23°C and a pressure of 1.512 atm, what is the percent. cobalt(III) carbonate in the sample?

5. A sample of helium gas, He, has a volume of 1.80 L, a pressure of 8.00 atm at a temperature of 39 °C. At what temperature (°C) will the helium have a volume of 49.0 mL and a pressure of 420 mmHg (n constant)? 6. How many milliliters of 8.95% (v/v) ethanol solution can be prepared from 50.25 mL of ethanol?

A scuba diver’s tank contains 0.30 kg oxygen (O2) compressed into a volume of 2.32 L.(a) Use the ideal gas law to estimate the gas pressure     inside the tank at 5°C, and express it in atmospheres     and in pounds per square inch.(b) What volume would this oxygen occupy at 30°C and      a pressure of 0.98 atm?