A 2.0 L vessel is filled with 7.3 ´ 10 ^{-2} mol hydrogen at 1.55 atm. What is the temperature of this gas?
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A 2.0 L vessel is filled with 7.3 ´ 10 -2 mol hydrogen at 1.55 atm....
If 3.05 mol of a gas has a volume of 43.3 L and a pressure of 1.55 atm, what is the temperature? Use R= 0.0821 atm. L/mol K. K
An empty 3.70 L steel vessel is filled with 2.00 atm of CH4(g) and 8.00 atm of O2(g) at 300 ∘C. A spark causes the CH4 to burn completely, according to the equation: CH4(g)+2O2(g)→CO2(g)+2H2O(g) ΔH∘ = -802kJ 1. What is the final temperature inside the vessel after combustion, assuming that the steel vessel has a mass of 12.475 kg , the mixture of gases has an average molar heat capacity of 21J/(mol⋅∘C), and the heat capacity of steel is 0.499J/(g⋅∘C)?...
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1. a. The pressure inside a hydrogen-filled container was 2.10 atm at 21 ∘C. What would the pressure be if the container was heated to 87 ∘C ? b. At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 95 ∘C ? c. Calculate the number of molecules in a deep breath of...
Part A The pressure inside a hydrogen-filled container was 2.10 atm at 21 ∘C. What would the pressure be if the container was heated to 99 ∘C ? Express your answer with the appropriate units. Part B At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 35 ∘C ? Express your answer...
Part A The pressure inside a hydrogen-filled container was 2.10 atm at 21 ∘C. What would the pressure be if the container was heated to 88 ∘C ? Express your answer with the appropriate units. Part B At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 95 ∘C ? Express your answer...
1. Calculate the volume of the gas, in liters, if 1.55 mol has a pressure of 1.20 atm at a temperature of -6 ∘C. (Answer in L) 2.Calculate the absolute temperature of the gas at which 3.33×10−3 mol occupies 498 mL at 760 torr . (Answer in K) 3.Calculate the pressure, in atmospheres, if 2.65×10−3 mol occupies 415 mL at 140 ∘C. (Answer in atm) 4.Calculate the quantity of gas, in moles, if 127 L at 60.0 ∘C has a...
5. (10 pts) A 1.00 L reaction vessel is filled with N204 (g) at a pressure of 0.154 atm. The gas is then allowed to decompose by the following equilibrium process N204(g) ^ 2NO2(g) a) At equilibrium, the total pressure in the container is 0.212 atm. What is the equilibriunm pressure of NO2 (g)? b) What is the Kp (numerical value) for the above equilibrium process?
A sample of gas in a 35.0 L cylinder-piston assembly has a pressure of 1.55 atm at 125oC. If the pressure on the gas increases to 3.0 atm while the volume of the gas decreases to 25.0 L, what is the temperature (oC) of the gas?
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