Ex: Given the following reaction equation: C6H6 (l) + O2 (g) → Calculate the volume of...
The balanced combustion reaction for C6H6 is 2 C6H6(l) + 15 O2 (g) -----> 12 CO2 (g) + 6 H2O(l) + 6542 kJ If 8.800 g C6H6 is burned and the heat produced from the burning is added to 5691 g of water at 21 C, What is the final temperature of the water? final temperature= ___________ C
Given: C6H6(g) + O2(g) LaTeX: \longrightarrow ⟶ CO2(g) + H2O(g) [unbalanced] takes place at 745 mmHg and 25oC, if 4.00 liters of benzene (C6H6) are consumed in this reaction, how many liters of water can be formed?
10) pts) For the unbalanced equation: C6H6 (1) + O2(g) → CO2(g) + H20 (1) AH = - 6535 kJ. What is AH when 45.67 g of CO2 is produced? Cottotit O2(g) 02 (g) thout Solo 2 11) (12 pts) A scientist mixed 25.00 mL of 2.00 M KOH with 25.00 mL of 2.00 M HBr. The temperature of the mixed solution rose from 22.7 °C to 31.9°C. Assume that the volumes are additive, and the density of the solution...
The thermochemical equation of combustion of methane is: CH4(g) + 2O2(g) → CO2(g) + 2 H2O(l) ΔΗ =-890.3 kJ 1. Calculate the AH when 5.00 g CH4 react with excess of oxygen. 2. Calculate AH when 2L CH4 at 49 °C and 782 mmHg react with an excess of oxygen 3. Calculate AH when 2L CH4 react with L O2 in a reaction vessel kept at 49 °C and 782 mmHg.
Calculate ΔHo for C6H6 (l) + 15/2 O2 (g) → 6 CO2 (g) + 3 H2O (l) from ΔHof C6H6 (l) = 49.0 kJ ΔHof CO2 (g) = - 393.5 kJ ΔHof H2O (l) = -285.8 k J
Balance the following chemical equation (if necessary): C6H6(1) + O2(g) → H2O(g) + CO2(g)
11. Use the equation below to calculate the following. a. Balance the reaction. K2CO3 (aq) + _HCH3O2 (aq) → KCH:O2 (aq) + H20 (1) +_ CO2 (g) b. Moles of H2O that can be obtained from 25.0 mL of 0.150 M HC2H302 c. Volume of 0.210 MK2CO3 needed to produce 17.5 mol KC,H,O, d. Volume of 1.25 M HC,H,O2 needed to react with 75.2 mL 0.750 M K.CO; e. Liters of CO2 gas at 25°C and 0.750 atm, produced by...
1. For the reaction N2(g) + 3H2(g) → 2NH3(g), if 2.25 L H2 reacts, what volume of NH3 forms if both are at the same temperature and pressure? 2.Given the balanced reaction below: 2 C6H6(g) + 15 O2(g) ⟶ 12 CO2(g) + 6 H2O(g) If 2.45 liters of benzene are consumed in this reaction, how many liters of water can be formed? Benzene is C6H6
Consider the unbalanced equation for the following reaction: O2(g) + C6H5COOH(aq) → CO2(g) + H2O(l) If 54.0 grams of C6H5COOH(aq) reacts with an excess of O2(g) and 103. grams of CO2(g) is formed, determine the percent yield of CO2(g). (the answer is 76.0%, I want to know the process)
Consider the following unbalanced equation: O2(g) + C4H10(g) → CO2(g) + H2O(l) If 3.56×102 moles of O2(g) and 47.3 moles of C4H10(g) are allowed to react to produce 1.10×102 moles of CO2(g), what is the percent yield of the reaction? 29.2% 58.1% 89.5% 89.9% 65.7%