Pressure,
P = density * g* height
Where g is acceleration due to gravity.
Since pressure is same for both,
density(mercury)*g*h(mercury) = density(water)*g*h(water)
density(mercury)*h(mercury) = density(water)*h(water)
13.5 g/cm^3 * 751 mm = 1.00 g/cm^3 * h(water)
h(water) = 10138 mm
h(water) = 1013.8 cm
Answer: 1.01*10^3 cm
The density of mercury is 13.5 g/mL and the density of water is 1.00 g/mL. If a mercury barometer reads 751 mmHg, w...
The density of mercury is 13.5 g/mL and the density of water is 1.00 g/mL. If a mercury barometer reads 787 mmHg, what is the barometric pressure in centimeters of water (cmH2O)?
1. A student reads a barometer in the laboratory and finds the prevailing atmospheric pressure to be 699 mm Hg. Express this pressure in atmospheres, kilopascals, torrs, pounds per square inch, and pascals. Hint: 1 atm = 101.3 kPa = 760 torr = 760 mm Hg = 14.69 psi = 1.013×105 Pa mm Hg atm kPa torr psi Pa 699 2. An automobile tire is inflated to a pressure of 29.2 psi. Express this pressure in atmospheres, kilopascals, inches Hg,...
In principle many different liquids could be used in a barometer. Mercury is usually preferred by virtue of its low vapour pressure and high density. As part of a school project, you have decided to build a barometer using water. Assuming the maximum pressure that the instrument will need to read is 1.05 atm, determine the height of the column required if (a) you ignore the vapour pressure of water or (b) you take the vapour pressure of water (PH2O=3.17...
In the first cell, 42.51 mL of hydrogen gas were formed at the cathode.The temperature was 21.5C and the vapor pressure of water at this temperature is 19.240 torr. The Barometric pressure was 758.8 mm Hg and the height of water in the buret above the level of water in the beaker was 8.2 cm. Calculate: a. Partial Pressure of Hydrogen (H2) in buret (PH2 = Barometric – VP – Pheight) (The pressure due to the height of water still...
The density of water at O°C is 1.00 g/mL. At 30°C the density of water is 0.996 g/mL. What is the change in volume from 850.0 mL when the temperature changes from 0°C to 30°C?
Canvas Question 12 The density of water at 3.98 °C is 1.00 g/mL. What is the density in g/cm3? O 16.4 g/cm3 O 3.98 g/cm3 O 2.54 g/cm3 O 624 g/cm3 O 1.00 g/cm3
1. A copper wire is 26.61 cm long and weighs 1.265 g. The density of copper is 8.933 g/cm3. A. What is the radius of the wire in millimeters? B. What is the diameter of the wire? 2. An empty beaker weighs 22.47 g. When completely filled with water, the beaker and its contents have a total mass of 437.15 g. What volume does the beaker hold? Use ?=1.00 g/mL as the density of water. How much would the beaker...
Given: Room temperature: 293.0 K Barometric pressure: 764.0 mmHg Vapor of water: 17.5 mmHg Volume of O2 collected: 68.00 mL Density of H2O2: 1.01 g/mL % Composition H2O2: 3.02 % Volume of H2O2 used: 5.00 mL Letter of the unknown solution of H2O2: A Volume of O2 collected for the unknown: 43.00 mL Calculate the corrected barometric pressure. (mmHg) Calculate the volume of O2 at STP. (mL) Based on the reaction stoichiometry, calculate the number of moles of O2. (moles)...
A calorimeter contains 26.0 mL of water at 13.5 ∘C . When 2.50 g of X (a substance with a molar mass of 51.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 30.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...
When 1.10 g of a salt dissolves in 252 mL of water (density = 1.00 g/mL) in a coffee-cup calorimeter, the temperature rises from 16.1°C to 24.5°C. Determine q for the solution process, assuming that Ccal ≈ Cwater.