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9. The density of air at 1.000 atm and 25 °C is 1.186 g/L. a) b) Calculate the average molecular mass of air. From...
The density of air at 1.000 atm and 25 °C is 1.186 g/L. 9. Calculate the average molecular mass of air. a) From thi...
The density of air at 1.000 atm and 25 °C is 1.186 g/L. 9. Calculate the average molecular mass of air. a) From this value, and assuming that air contains only molecular nitrogen and b) molecular oxygen gases, cal culate the mass % of N2 and O2 in air.
The density of air at 776.0 torr and 24.0°C is 1.216 g/L. Part 1: Calculate the...
The density of air at 776.0 torr and 24.0°C is 1.216 g/L. Part 1: Calculate the average molar mass of air. 29.05 g/mol Part 2 out of 2 From this value, and assuming that air contains only molecular nitrogen and molecular oxygen gases, calculate the mass percent of N, and of Oz in air. N2 % Re 02 % 3 attempts left Check my work Next part Gu
5 L of an apple juice in a container was saturated at a pressure of 6...
5 L of an apple juice in a container was saturated at a pressure of 6 atm and a temperature of 25 oC with air and sealed. The Henry’s Law constants for nitrogen and for oxygen are 6.1×10-4 mol L-1 atm1 and 1.3×10-3 mol L-1 atm-1 respectively. (i) Calculate the molarity and the mass of nitrogen and oxygen dissolved in the juice. (ii) Calculate the mass of nitrogen (N2) and the mass of oxygen (O2) released when the container was...
Assuming air has a density of 1.17 g/L and .973 atm what is the average molar...
Assuming air has a density of 1.17 g/L and .973 atm what is the average molar mass of air?
calculate the density of O2 gas( in g/L) at 1.22 atm and 25 degrees C
calculate the density of O2 gas( in g/L) at 1.22 atm and 25 degrees C
1. Calculate the mass in grams of 4.6 L of NO gas at 26.0oC and a...
1. Calculate the mass in grams of 4.6 L of NO gas at 26.0oC and a pressure of 1,293 mm Hg (1 atm=760 mm Hg. Round your answer to one decimal place and do not include units. 2. Air from a newly discovered planet contains nitrogen, oxygen, and an unidentified gas. A sample of air collected at Bismarck at -22 °C and 98.90 kPa had 78.0 % N2, 21.0% O2, and 1.0% other. Find the partial pressures of the oxygen...
1. If nitrogen gas has a density of 1.14 g/L, and an unknown gas has a...
1. If nitrogen gas has a density of 1.14 g/L, and an unknown gas
has a density of 4.2 g/L at the same temperature and pressure, what
is the ratio of the rate of effusion of the known gas to the rate
of effusion of nitrogen?
2. The combustion reaction for octane burning in oxygen is:
2 C8H18 (l) + 25 O2(g)
→ 16 CO2(g) +18 H2O(g)
∆H = -10869 kJ .
Suppose an oxygen bomb calorimeter is loaded with oxygen...
Air is a mixture of gases with the following mass percentage composition: 75.52% N2, 23.15% O2,...
Air is a mixture of gases with the following mass percentage
composition: 75.52% N2, 23.15% O2, 1.28% Ar, and 0.046% CO2 (a)
What are the partial pressures of N2, O2, Ar, and CO2, when the
total pressure is 1.100 atm? (b) Calculate the molar Gibbs energy
of mixing of air at 25 °C assuming ideal-gas behavior. (c)
Determine the molar enthalpy of mixing and the molar entropy of
mixing for air at 1.100 atm and 25 °C.
5. (3 pts)...
QUESTION 3 0.5 points Save Answer If nitrogen gas has a density of 1.14 g/L, and...
QUESTION 3 0.5 points Save Answer If nitrogen gas has a density of 1.14 g/L, and an unknown gas has a density of 5.67 g/L at the same temp and pressure, what is the ratio of the rate of effusion of the known gas to the rate of effusion of nitrogen? rate effusion unknown - 2 rate effusion N2 QUESTION 4 0.5 points Save Answer The combustion reaction for octane burning in oxygen is: 2 C8H18 (1) + 25 O2(g)...
A flask is filled with 1.000 atm NO(g) and 1,000 atm O2 el. At equilibrium, the...
A flask is filled with 1.000 atm NO(g) and 1,000 atm O2 el. At equilibrium, the pressure of O2 -0.506 atm. Calculate Kp. Report answer to 2 sig figs. 2 NO2(g) + 2NO(g) + O2(g) At a certain temperature, K = 6.5 x 102 for the reaction: 2 NO(g) + 2 H2(g) = N2 (g) + 2 H20 (9) K= 6.5 x 102 Calculate K for the reaction: 2 N2(g) + 4H20 (g) = 4 NO (@) + 4H2 (g)...
The density of air at 1.000 atm and 25 °C is 1.186 g/L. 9. Calculate the average molecular mass of air. a) From this value, and assuming that air contains only molecular nitrogen and b) molecular oxygen gases, cal culate the mass % of N2 and O2 in air.
The density of air at 776.0 torr and 24.0°C is 1.216 g/L. Part 1: Calculate the average molar mass of air. 29.05 g/mol Part 2 out of 2 From this value, and assuming that air contains only molecular nitrogen and molecular oxygen gases, calculate the mass percent of N, and of Oz in air. N2 % Re 02 % 3 attempts left Check my work Next part Gu
1. If nitrogen gas has a density of 1.14 g/L, and an unknown gas
has a density of 4.2 g/L at the same temperature and pressure, what
is the ratio of the rate of effusion of the known gas to the rate
of effusion of nitrogen?
2. The combustion reaction for octane burning in oxygen is:
2 C8H18 (l) + 25 O2(g)
→ 16 CO2(g) +18 H2O(g)
∆H = -10869 kJ .
Suppose an oxygen bomb calorimeter is loaded with oxygen...
Air is a mixture of gases with the following mass percentage
composition: 75.52% N2, 23.15% O2, 1.28% Ar, and 0.046% CO2 (a)
What are the partial pressures of N2, O2, Ar, and CO2, when the
total pressure is 1.100 atm? (b) Calculate the molar Gibbs energy
of mixing of air at 25 °C assuming ideal-gas behavior. (c)
Determine the molar enthalpy of mixing and the molar entropy of
mixing for air at 1.100 atm and 25 °C.
5. (3 pts)...
QUESTION 3 0.5 points Save Answer If nitrogen gas has a density of 1.14 g/L, and an unknown gas has a density of 5.67 g/L at the same temp and pressure, what is the ratio of the rate of effusion of the known gas to the rate of effusion of nitrogen? rate effusion unknown - 2 rate effusion N2 QUESTION 4 0.5 points Save Answer The combustion reaction for octane burning in oxygen is: 2 C8H18 (1) + 25 O2(g)...
A flask is filled with 1.000 atm NO(g) and 1,000 atm O2 el. At equilibrium, the pressure of O2 -0.506 atm. Calculate Kp. Report answer to 2 sig figs. 2 NO2(g) + 2NO(g) + O2(g) At a certain temperature, K = 6.5 x 102 for the reaction: 2 NO(g) + 2 H2(g) = N2 (g) + 2 H20 (9) K= 6.5 x 102 Calculate K for the reaction: 2 N2(g) + 4H20 (g) = 4 NO (@) + 4H2 (g)...
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