From the balanced chemical reaction,
5 mole*32g/mole= 160 g of oxygen upon reaction the change in energy is -2365 kJ
When 31.00 g of oxygen upon reaction the change in energy is(31.00g*(-2365kJ))/160g= -458.2 kJ
Therefore the change in energy is -458.2 kJ
A31.00 g sample of oxygen at 298K reacts with excess propane. Calculate the change in energy,...
When 1.14 g of octane (molar mass = 114 g/mol) reacts with excess oxygen in a constant volume calorimeter, the temperature of the calorimeter increases by 10.0°C. The heat capacity of the calorimeter is 6.97 kJ/°C. Determine the energy flow, qrxn. +6.97 kJ +69.7 kJ +6970 kJ –6970 kJ –69.7 kJ
Question 3 1 pts Gaseous ammonia reacts with oxygen to produce nitrogen and water vapor according to the following thermochemicl equation: 4 NH3(g) + 3029 +2 N2(g) + 6 H20 (g); AH = -1232 kJ How much heat (kJ) is produced when 17.9 g of ammonia are reacted in excess oxygen? (3 sig figs, fill in the number ONLY!) Question 4 0.5 pts Which of the following are intensive properties? Note that there may be more than one correct choice....
3.24 mol of surfer dioxide reacts with an excess of oxygen gas to phone sulfur trioxide assuming the reaction occurs as a temperature of 300 K and a pressure of 2.50 ATM what volume of sulfur trioxide want your list in L Table of Contents > Test 3 > Module 8 > After Class: Knewton HW and quiz > 8.4 Gas Laws: Ideal Gas Laws 18.4 Gas Laws: Ideal Gas Laws ---- Consider the reaction represented by the following chemical...
5.61 g of octane, C8H18, reacts with excess oxygen in a bomb calorimeter. The heat capacity of the calorimeter is 6.97 kJ/°C and the temperature increases by 18.0°C. How much heat, in units of kJ/mol, was absorbed by the bomb calorimeter?
When excess Cl2 at constant pressure reacts with 0.300 mol of CH4(g) 295 kJ of energy evolves. Calculate the value of ΔH for this reaction, as written. CH4(g) + Cl2(g) → CHCl3(l) + H2(g) ΔH = ? a) -1970 kJ b) -1770 kJ c) +1970 kJ d) -983 kJ e) +1770 kJ
1. Determine the standard Gibb's free energy change for the conversion of diamond into graphite in units of kJ/mol and is it spontaneous, nonspontaneous, or neither. Cdiamond (s) ? Cgraphite (s) f° for diamond = 2.9 kJ/mol f° for graphite = 0.0 kJ/mol (Please be careful wtih sig figs.) 2. For the following reaction, = 68.1 kJ/mol: 2 C(s) + 2 H2(g) ? C2H4(g) Determine for the reaction in units of kJ/mol at 1800. K, a partial pressure of C2H2 of...
1. The standard enthalpy change for the combustion of mole of propane is -2043.0 kJ. CH_(g) +5 0 (g) →3002(g) + 4H2O(g) Calculate Hº for propane based on the following standard molar enthalpies of formation. molecule CO (9) H2O(g) AH (kJ/mol-rxn) -393.5 -241.8 a. +1407.7 kJ/mol-rxn b. +104.7 kJ/mol-rxn c.-104.7 kJ/mol-rxn d -4190.7 kJ/mol-rxn e. -1407.7 kJ/mol-rxn 2. Which of the following statements is/are CORRECT? 1. If a reaction occurs at constant pressure, 4-AH. 2. The change in energy for...
12 Question (1 point) 421 g of octane, CH18 reacts with excess oxygen in a bomb calorimeter. The heat capacity of the calorimeter is 6.97 kJ/°C and the temperature increases by 50.0°C 1st attempt See Periodic Table See Hint How much heat. in units of /mol. was absorbed by the bomb calorimeter? kJ/mol
vice Desk Faculty Help Page Student Help Question 4 Incorrect Calculate w (in kJ) when 189 g iron (In) oxide (MM = 159.7 g/mol) reacts with excess carbon to produce carbon dioxide gas at 451 K: Mark 0.00 out of 1.00 2Fe2O3(s) + 3C(s) + 4Fe(s) + 3C02(g) P Flag question Answer: -4426.8 Hint, is the work (-) or (+)? Question 7 Incorrect Mark 0.00 out of 1.00 A reaction at 4.21 atm produces 24.6 L of a gas and...
MHE Reader Propane, C3Hs(&), reacts with oxygen gas to produce carbon dioxide gas and water vapor. a) b) 2. Write a balanced equation including states of matter for the reaction. If 4.55 g of propane reacts with excess oxygen under standard conditions, calculate the theoretical yields (in grams) for both carbon dioxide and water, and · the total amount of heat released/absorbed when the reaction is complete. c) Ethanol is currently being used as a replenishable fuel alternative/supplement because it...