You have the following info: C3H8(l) + O2(g) ---> CO2(g) + H2O(g) ∆Hrxn = -2044 kJ...
You have the following info: C3H8(l) + O2(g) ---> CO2(g) + H2O(g) ∆Hrxn = -2044 kJ
Given 4.73 Kg of C3H8(g) react and the gas produced from the reaction is collected in a 5.00 L container at 298 K.
Molar masses: C3H8 = 44.09 g/mol, H2O = 18.02 g/mol, CO2 = 40.02 g/mol
1) What is the heat of the reaction given the conditions described (i.e. what is qrxn)?
2) Is the reaction exothermic or endothermic?
3) Is heat a product or reactant for this reaction?
4) Assuming that the reaction works perfectly, what pressure of gas should be collected in the container at 298 K?
Homework Answers
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You have the following info: C3H8(l) +
O2(g) ---> CO2(g) + H2O(g)
∆Hrxn = -2044 kJ...
You have the following info: C3H8(t) + O2(g) → CO2(g) + H2O(g) AHrx = -2044 kJ...
You have the following info: C3H8(t) + O2(g) → CO2(g) + H2O(g) AHrx = -2044 kJ Given 3.97 kg of C3H8(9) react and the gas produced from the reaction is collected in a 5.00 L container at 298 K. Molar masses: C3H8 = 44.09 g/mol, H2O = 18.02 g/mol, CO2 = 40.02 g/mol a) What is the heat of the reaction given the conditions described (i.e. what is Gnx)? b) is the reaction exothermic or endothermic? c) Is heat a...
Combustion of 2.5000 g of propane (C3H8) releases 115.75 kJ of heat when it is burned...
Combustion of 2.5000 g of propane (C3H8) releases 115.75 kJ of heat when it is burned to form CO2 (g) and H2O (l). The standard formation enthalpies of CO2 (g) and H2O (l) are -393.5 kJ/mol and -285.5 kJ/mol respectively. Calculate the Hrxn for the combustion of propane in kJ/mol Calculate ∆?? ? for propane
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The...
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The enthalpy of combustion of CH2(g) to make H2O(l) and CO2(g) is -2760 kJ mol-1. The enthalpy of formation of H2O(l) is -286 kJ mol-1. All the data are for 298 K. The heat capacities for O2(g), CHA(8), CH3(g), H2O(l) and CO2(8) are 29, 61, 71, 75 and 37 JK"mor", respectively. Deduce a) 4U298 for the combustion of C4H8(g). 5) AH for the combustion of...
Consider the reaction: H2(g) + (1/2)O2(g) -------> H2O(l) ΔH° = -286 kJ Which of the following...
Consider the reaction: H2(g) + (1/2)O2(g) -------> H2O(l) ΔH° = -286 kJ Which of the following is true? (Select all that apply) the reaction is endothermic heat is given off by the surroundings the reaction is exothermic heat is absorbed by the system the enthalpy of the products is less than the that of the reactants
Given the following heat of formation values, calculate the heat of reaction for the following: C3H8(g)...
Given the following heat of formation values, calculate the heat of reaction for the following: C3H8(g) + O2(g) CO2(g) + H2O(1). AfH values in kJ/mol: C3H8(g): -103.8, O2(g): 0, CO2(g): -393.5, H2O(l): -285.8. 3.613 x 102 kJ/mol -2.220 103 kJ/mol 1.413* 102 kJ/mol -5.755 x 102 kJ/mol If a lighter contains 4.0 mL of liquid butane (density of butane = 0.8 g/cm3), how much heat can we get out of it, from the combustion of butane? 2 C4H 10(g) +...
Use the combustion of methane for the following question: CH4 (g) + O2 (g) → CO2...
Use the combustion of methane for the following question: CH4 (g) + O2 (g) → CO2 (g) + H2O (l) ∆H = -890 kJ/mol A)Is the reaction exothermic or endothermic? B)If I combust 2 mol of methane, how much heat is absorbed or released - use the appropriate sign to indicate in your answer. C) If I combust 12.5 g of methane, how much energy in kJ is absorbed or released? Use the appropriate sign in your answer.
GIVEN INFO LP gas burns according to the following exothermic reaction: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) ΔH∘rxn= −2044kJ What mass...
GIVEN INFO LP gas burns according to the following exothermic reaction: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) ΔH∘rxn= −2044kJ What mass of LP gas is necessary to heat 1.4 L of water from room temperature (25.0 C) to boiling (100.0 C)? Assume that during heating, 16% of the heat emitted by the LP gas combustion goes to heat the water. The rest is lost as heat to the surroundings. Express your answer using two significant figures. FINAL ANWSER SHOULD BE IN GRAMS ?
7) Find AH° for the reaction C3Hg(8) + 5 O2(8) - 3 CO2(8) + 4 H2O(l)....
7) Find AH° for the reaction C3Hg(8) + 5 O2(8) - 3 CO2(8) + 4 H2O(l). AH° = -2046 kJ for the reaction: C3H8(8) + 5 O2(8) - 3 CO2(g) + 4H2O(8) The heat of vaporization of water is 44.0 kJ/mol. The standard enthalpy of formation of water and water vapor are -285.9kj/mol and -241.8 kj/mol, respectively. Note that H20 is a liquid in the first reaction and a gas in the second. 0-1870 kJ 0-2222 kJ O-2002 kJ 0-2090...
Methanol (CH3OH) burns according to the equation 2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l), ΔH°rxn =...
Methanol (CH3OH) burns according to the equation 2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l), ΔH°rxn = –1454 kJ/mol. A) How much heat, in kilojoules, is given off when 150.0 g of methanol is burned? [ Select ] B) How many grams of CO2 are produced when the amount of heat determined in part A is released? [ Select ] Molar masses: CH3OH = 32.04 g/mol O2 = 32.00 g/mol CO2 = 44.01 g/mol H2O = 18.02 g/mol
4. Consider the following reaction at equilibrium CO(g) + H2O(g) + CO2(g) + H2(g) 2.50 mole...
4. Consider the following reaction at equilibrium CO(g) + H2O(g) + CO2(g) + H2(g) 2.50 mole of CO(g) and 2.50 mole of H2O(g) gas at 588 K are mixed in a 10.00 L container. (Kc = 31.4 at 588 K) Calculate the concentration of CO(g), H2O(g), CO (g), and H.(g) at equilibrium. 5. Consider the following reaction: CO(g) + H2O(g) + CO2(g) + H2(g) (a) If a 10.00L container has 2.50 mole of CO(g), 2.50 mole of H2O(g), 5.00 mole...
You have the following info: C3H8(t) + O2(g) → CO2(g) + H2O(g) AHrx = -2044 kJ Given 3.97 kg of C3H8(9) react and the gas produced from the reaction is collected in a 5.00 L container at 298 K. Molar masses: C3H8 = 44.09 g/mol, H2O = 18.02 g/mol, CO2 = 40.02 g/mol a) What is the heat of the reaction given the conditions described (i.e. what is Gnx)? b) is the reaction exothermic or endothermic? c) Is heat a...
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The enthalpy of combustion of CH2(g) to make H2O(l) and CO2(g) is -2760 kJ mol-1. The enthalpy of formation of H2O(l) is -286 kJ mol-1. All the data are for 298 K. The heat capacities for O2(g), CHA(8), CH3(g), H2O(l) and CO2(8) are 29, 61, 71, 75 and 37 JK"mor", respectively. Deduce a) 4U298 for the combustion of C4H8(g). 5) AH for the combustion of...
Given the following heat of formation values, calculate the heat of reaction for the following: C3H8(g) + O2(g) CO2(g) + H2O(1). AfH values in kJ/mol: C3H8(g): -103.8, O2(g): 0, CO2(g): -393.5, H2O(l): -285.8. 3.613 x 102 kJ/mol -2.220 103 kJ/mol 1.413* 102 kJ/mol -5.755 x 102 kJ/mol If a lighter contains 4.0 mL of liquid butane (density of butane = 0.8 g/cm3), how much heat can we get out of it, from the combustion of butane? 2 C4H 10(g) +...
7) Find AH° for the reaction C3Hg(8) + 5 O2(8) - 3 CO2(8) + 4 H2O(l). AH° = -2046 kJ for the reaction: C3H8(8) + 5 O2(8) - 3 CO2(g) + 4H2O(8) The heat of vaporization of water is 44.0 kJ/mol. The standard enthalpy of formation of water and water vapor are -285.9kj/mol and -241.8 kj/mol, respectively. Note that H20 is a liquid in the first reaction and a gas in the second. 0-1870 kJ 0-2222 kJ O-2002 kJ 0-2090...
4. Consider the following reaction at equilibrium CO(g) + H2O(g) + CO2(g) + H2(g) 2.50 mole of CO(g) and 2.50 mole of H2O(g) gas at 588 K are mixed in a 10.00 L container. (Kc = 31.4 at 588 K) Calculate the concentration of CO(g), H2O(g), CO (g), and H.(g) at equilibrium. 5. Consider the following reaction: CO(g) + H2O(g) + CO2(g) + H2(g) (a) If a 10.00L container has 2.50 mole of CO(g), 2.50 mole of H2O(g), 5.00 mole...
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