A 5.50L flask was used to collect a 5.65g sample of propane (C3H8). The pressure was measured to be 956mmHg. What is the temperature of the gas in the flask?
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A 5.50L flask was used to collect a 5.65g sample of propane (C3H8). The pressure was...
a.) A 2.50 L flask was used to collect a 2.65 g sample of propane gas, . After the sample was collected, the gas pressure was found to be 743 mmHg. What was the temperature of the propane in the flask? ______°C b.)Butane,C4H10 , is an easily liquefied gaseous fuel. Calculate the density of butane gas at 0.791 atm and 24°C. Give the answer in grams per liter. Density = ______g/L c.) A 0.488-g sample of a colorless liquid was...
The combustion of propane gas (C3H8) is used to fuel barbeque grills. In order to produce 5.65 moles of water how many moles of oxygen gas are needed? C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l
For the gas propane (C3H8), (a) how many grams are in 1.50 moles of C3H8, (b) how many moles are in 25.0 grams of C3H8, (c) how many molecules of C3H8 are in 25.0 moles of C3H8 and finally (d) what is the percent carbon in C3H8?
A 75.0 L steel tank at 20.0 degrees C contains propane gas, C3H8, at a pressure of 1.39 atm. Assuming ideal behavior, how many moles of C atoms are in the tank?
8.24 kg of propane gas is being used as fuel. Based on the reaction C3H8 + O2 ? CO2 + H2O, how many kilograms of carbon dioxide have been produced? (Note: Please make sure to balance the equation) 2.75 kg 8.24 kg 24.72 kg 31.26 kg
A Fuel Gas Consists Of 75% Butane (C4H10), 10% Propane (C3H8) And 15% Butene (C4H8) By Volume. ... Question: A fuel gas consists of 75% butane (C4H10), 10% propane (C3H8) and 15% butene (C4H8) by volume. It... A fuel gas consists of 75% butane (C4H10), 10% propane (C3H8) and 15% butene (C4H8) by volume. It is to be fed to the combustion chamber in 10% excess air at 25ºC, where it is completely burnt to carbon dioxide and water. The...
he propane fuel (C3H8) used in gas BBQs burns according to this thermochemical equation: C3H8 + 5O2 --> 3CO2 + 4H2O delta H = -2217kJ If a pork roast must absorb 1.6x10^3 kJ to fully cook, and if ONLY 10% of the heat produced by the BBQ is actually absorbed by the roast, what mass of CO2 is emitted into the atmosphere during the grilling of the pork roast.
Heat was added to a 45.0g sample of liquid propane, C3H8(l), at a rate of 500.0J/min. The temperature remained constant at -42.1 degrees C, the normal boiling point of propane, for 38.9 minutes. Calculate the molat enthalpy of vaporization of propane.
The propane fuel (C3H8) used in gas barbeques burns according to the following thermochemical equation: C3H8(g)+5O2(g)?3CO2(g)+4H2O(g) If a pork roast must absorb 1700kJ to fully cook, and if only 14% of the heat produced by the barbeque is actually absorbed by the roast, what mass of CO2 is emitted into the atmosphere during the grilling of the pork roast? Express your answer using two significant figures.
The propane fuel (C3H8) used in gas barbeques burns according to this thermochemical equation. If a pork roast must absorb 1.5×103 kJ to fully cook, and if only 15 % of the heat produced by the barbeque is actually absorbed by the roast, what mass of CO2 is emitted into the atmosphere during the grilling of the pork roast?