Question

Calculate the barometric pressure in a city that is 1500 meters above the sea level, where the average temperature is 20.

Answer #1

Carrollton, GA is 335 meters above sea level. What is the
atmospheric pressure in Carrollton? (The density of air is 1.29
kg/m3.)

A lake at an elevation of 15,000 feet, where the barometric
pressure is 515.7 mm Hg.
-What is the barometric pressure in units of atm?
-What is the partial pressure of oxygen at this
elevation?
-What is the maximum concentration of oxygen in water (in
mg/L) under these conditions, at a temperature of 25.0°C?

NASA launches a rocket at t=0 seconds. Its height, in meters
above sea-level, as a function of time is given by
h(t)=−4.9t^2+277t+283
Assuming that the rocket will splash down into the ocean, at what
time does splashdown occur?
How high above sea-level does the rocket get at its peak?

1. A typical barometric pressure in a fictional location is
about 718 mmHg. Calculate this pressure in atm and kPa.
2. A 2.51 L volume of hydrogen measured at −148 °C is warmed to
100.°C. Calculate the volume (in L) of the gas at the higher
temperature, assuming no change in pressure.

Electrolysis problem. Calculate the partial pressure of H2
(using barometric pressure and vapor pressure of water) and the
Faradays required to generate 0.01358 moles of hydrogen gas given
the following information.
10 mL of 3 M H2SO4 was diluted in 100 ml. 49.8 mL of this
solution was used in electrolysis (initial buret reading was at 50
mL and final was at 0.2). The electrolysis was conducted at 20 V
for seven minutes and forty seconds. I calculated the moles...

-At sea level, a pressure gauge on a closed rigid tank reads
20.0 psi. The tank is moved to a location where the atmospheric
pressure is 13.00 psi. What is the gauge pressure (psi) for the
tank at this new location?
- A temperature change of 26.0 °F is equivalent
to what in C

a) Determine the variation of Earth's atmosphere in function of
altitude (y), above the sea level, assuming a constant geavity (g)
and that the density of the air is proportional to the
pressure.
b) At what altitude the pressure of the air is the same as halve
the pressure at sea level?
c) Graph pressure against altitude.

A 300–mL volume of hydrogen is collected over water at 22 °C
under a barometric pressure of 740 mmHg. What is the volume of this
hydrogen, at the same temperature and barometric pressure, when
dry? (vapor pressure of water at 22 °C = 20 mmHg)
the answer is 292 mL. PLEASE EXPLAIN HOW YOU GET THIS ANSWER
:(

What is the density at 105 m above the ground (which is at sea
level) if the temperature at this height is 315 K, assuming you can
use the ideal gas law?

Determine the percentage of mass of the atmosphere that resides
between sea level and a height of 25.7 km. Assume an average
pressure of 1.00 atm at sea level and a temperature of the
atmosphere of 15 °C. The average molar mass of air is 28.96 g/mol.
You may or may not need Earth's radius, which is 6,371 km.

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