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?
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Given: C6H6(g) + O2(g) LaTeX: \longrightarrow ⟶ CO2(g) + H2O(g) [unbalanced] takes place at 745 mmHg...
Given the following data: (1) 2 H2(g) + CO2(g) LaTeX: \longrightarrow ⟶ CH4(g) + O2(g) DGorxn = 343 KJ (2) 2 H2(g) + O2(g) LaTeX: \longrightarrow ⟶ 2 H2O(l) DGorxn = -474 KJ Calculate DGorxn (kJ) for (3) CH4(g) + 3 O2(g) + 2 H2(g) LaTeX: \longrightarrow ⟶ CO2(g) + 4 H2O(l) DGorxn = ??? Only enter a numerical value.
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
2. Given the unbalanced equation: C3H8 + O2 CO2 + H2O a. How many moles of oxygen gas are required to make 4.00 moles of carbon dioxide? b. How many moles of C3H8 must be used to produce 2.00 grams of water?
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)
Given the equation: C2H6 (g) + O2 (g) → CO2 (g) + H2O (g) (not balanced) Determine the number of liters of O2 consumed at STP when 60.0 grams of C2H6 is burned.
Show the calculation of the volume of H2O gas formed by the combustion of 18.6 grams of C6H6 at 30oC and 1.10 atm?The combustion of benzene (C6H6) takes place by the following reaction equation. 2 C6H6 (g) + 15 O2 (g) → 12 CO2 (g) + 6 H2O (g) Please Help!
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
Ex: Given the following reaction equation: C6H6 (l) + O2 (g) → Calculate the volume of CO2 produced when 35 g of C6H6 react at 38 oC and 658 mmHg CO2 (g) H20 (I)
In the reaction: C2H6(g) + O2(g) CO2(g) + H2O(g), how many moles of carbon dioxide are formed by the reaction of 4.00 moles of oxygen? 0 5.43 moles 0 4.00 moles O 3.43 moles 0 6.78 moles O 7.83 moles
***Please type answer if possible*** GAS VOLUME STOICHIOMETRY PROBLEMS 1. The combustion of ethanol (C2H5OH) takes place by the following reaction equation. C2H5OH (l) + 3 O2 (g) → 2 CO2 (g) + 3 H2O (g) What is the volume of CO2 gas produced by the combustion of excess ethanol by 23.3 grams of O2gas at 25oC and 1.25 atm? GAS VOLUME STOICHIOMETRY PROBLEMS 2. Acetic acid (CH3COOH) is formed from its elements by the following reaction equation: ...