Question

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

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

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Carrollton, GA is 335 meters above sea level. What is the atmospheric pressure in Carrollton? (The...
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....
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...
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...
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)...
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...
-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,...
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...
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...
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...
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.