How much CO2 in liter at STP is emitted when 30.0g of propane burn with oxygen to form CO2 and water? use a balanced equation to solve the problem.
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How much CO2 in liter at STP is emitted when 30.0g of propane burn with oxygen...
10.6 Gas Stoichiometry 6. Propane gas (C3Hg) reacts with oxygen according to the balanced equation shown below. If 12.0 moles of propane react in this way, C3Hs (g) + 502(g) → 3C02(g) + 4H20 (6) a. How many moles of water can form? b. How many moles of carbon dioxide can form? C. At STP, what volume of CO2 can form? d. Are more moles of gas produced or consumed in this reaction?
1.What mass of oxygen is necessary to burn 106.9g of propane in a balanced fashion? 2.What is the theoretical yield of water, in grams? 3.How many grams of oxygen does it take to burn 15.4 g of glucose
A) What mass of oxygen is necessary to burn 168.8 g of propane in a balanced fashion? B) What is the theoretical yield of water, in grams?
(25)4. Consider thefollowing reaction representing the combustion of butane: C3H8 O2 CO2+ H20 (a) (b) (c) Balance the equation. How many moles of oxygen are required to burn 1 mole of propane? How many grams of oxygen are required to burn 1 kg of propane? to burn 1 kg of propane? If air is21 percent oxygen, what volume of air at STP would be required? burned?
Pentane (C5H12) burn in oxygen to form carbon dioxide and water according to the following reaction. What is the coefficient for water in the balanced equation? C5H12(l) + ? O2(g) → ? CO2(g) + ? H2O(g) 2 4 5 6 8
27) When propane (C3H8) reacts with oxygen, carbon dioxide and water are produced. The balanced equation for this reaction is: C3H8 (g) + 5O2 (g) ---> 3CO2 (g) + 4H2O (g) Suppose 17.8 moles of oxygen react. The reaction consumes ___ moles of propane (C3H8). The reaction produces ___ moles of carbon dioxide and ___ moles of water. How many grams of water are produced in the complete reaction of 27.2 grams of propane (C3H8)? ___ grams
How many grams of oxygen are required to burn 0.10 mole of propane, C3H8? C3H8 + 5O2 ® 3CO2 + 4H2O
Octane (C3H18) reacts with oxygen (O2) to form carbon dioxide (CO2) and water (H2O). When the equation below is balanced, the coefficient of octane is: C8H18 + O2-CO2 + H20
Review Question 10.010 Explain why two liters of hydrogen gas and one liter of oxygen gas react to form two liters of water, when the pressures and temperatures are held constant. Since the pressures and temperatures are constant, the ratio of the volumes is equivalent to the stoichiometric ratio. The balanced chemical equation is (Include physical states in your answer and use smallest integer coefficients to balance the equation.): I ? Edit Edit liter(s) of oxygen will form liter(s) of...
The compound C7H4N306, burns explosively with oxygen to produce CO2, water, and N2- Write a balanced chemical equation for this reaction and calculate the mass of oxygen required (in grams) to burn 100 g of this compound.