1. If you were to make a barometer out of water instead of Hg, how high must the
ID: 589201 • Letter: 1
Question
1. If you were to make a barometer out of water instead of Hg, how high must the column of water be to exert a pressure equal to that of a 760 mm column of Hg? The density of water is 1.0 g/mL and the density of Hg is 13.6 g/mL column must be high (you supply the units). 2. If the gas in a 2.0 L cylinder at 30.0 atm and 25° C is completely transferred into a 15.0 L vessel at 50°C, what will be the pressure of that gas? pressure atm 3. For the reaction below, how many liters of N2 (g) at 450 C and 6.00 atm are required to produce 1.00 mole of NHs (g)? N2(g) + 3H2 (g) 2NH3 (g) volume of N2 4. A mixture of 0.435 moles of N2, 0.123 moles of O2, and 0.725 mole of Ne is in a 10.0 liter container at 35°C. What is the partial pressure of each gas? PNe A graduated cylinder is filled brim full of water inverted into a beaker of water and used to collect hydrogen produced by a chemical reaction. After the reaction is completed, the volume of gas in the graduated cylinder is 76.0 mL. If the temperature is 30°C and the barometric pressure is 748 torr, how many moles of H2 were collected over the water? You may use your book as necessary 5. moles of H2 Assume that the enthalpies of formation are as follows: AH,-=-3883 kNmol for Nick(aq), and AH -167.2 kJ for HCI(aq). What is the AH for the reaction: 6. NiCl2(aq) +- Ha(g) ? HCl(aq) Ni(s) + kJExplanation / Answer
1)
Pressure (P) = height of the column(h)xdensity of liquid (d)x gravitational force (g)
For Hg:
P = hHg x dHg x g .......(1)
For H2O:
P = hH2O x dH2O x g .....(2)
From equations (1) and (2).
hH2O x dH2O = hHg x dHg
Substitute the given values.
hH2O x (1.0 g/mL) = (760 mm) x ( 13.6 g/mL)
hH2O = (760 mm) x ( 13.6 g/mL) / ( 1.0 g/mL) = 10336 mm
So, the column of water must be 10336 mm high.
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